Mocktest

Question 2/223

4 / -1

Mark Review

The following concentrations were observed at 500K for the formation of NH₃ from N₂ and H₂. At equilibrium :

[N₂] = 2 × 10⁻²M, [H₂] = 3 × 10⁻²M and [NH₃] = 1.5 × 10⁻²M. Equilibrium constant for the reaction is___

[29-Jan-2024 Shift 2]

The following concentrations were observed at 500K for the formation of NH₃ from N₂ and H₂. At equilibrium :

[N₂] = 2 × 10⁻²M, [H₂] = 3 × 10⁻²M and [NH₃] = 1.5 × 10⁻²M. Equilibrium constant for the reaction is___

[29-Jan-2024 Shift 2]

Question 3/223

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Mark Review

For the given reaction, choose the correct expression of K_C from the following :-

[31-Jan-2024 Shift 1]

For the given reaction, choose the correct expression of K_C from the following :-

[31-Jan-2024 Shift 1]

A

B

C

D

Question 4/223

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Mark Review

Given below are two statements :

Statement (I) : Aqueous solution of ammonium carbonate is basic.
Statement (II) : Acidic/basic nature of salt solution of a salt of weak acid and weak base depends on Ka and Kb value of acid and the base forming it.

In the light of the above statements, choose the most appropriate answer from the options given below :

[27-Jan-2024 Shift 1]

Given below are two statements :

Statement (I) : Aqueous solution of ammonium carbonate is basic.
Statement (II) : Acidic/basic nature of salt solution of a salt of weak acid and weak base depends on Ka and Kb value of acid and the base forming it.

In the light of the above statements, choose the most appropriate answer from the options given below :

[27-Jan-2024 Shift 1]

A

Both Statement I and Statement II are correct

B

Statement I is correct but Statement II is incorrect

C

Both Statement I and Statement II are incorrect

D

Statement I is incorrect but Statement II is correct

Question 5/223

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Mark Review

Which of the following is strongest Bronsted base?

[27-Jan-2024 Shift 1]

Which of the following is strongest Bronsted base?

[27-Jan-2024 Shift 1]

A

B

C

D

Question 6/223

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Mark Review

The pH at which Mg(OH)₂[K sp = 1 × 10⁻¹¹] begins to precipitate from a solution containing 0.10M Mg²⁺ ions is____

[30-Jan-2024 Shift 1]

The pH at which Mg(OH)₂[K sp = 1 × 10⁻¹¹] begins to precipitate from a solution containing 0.10M Mg²⁺ ions is____

[30-Jan-2024 Shift 1]

Question 7/223

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Mark Review

The pH of an aqueous solution containing 1M benzoic acid (pKa = 4.20) and 1M sodium benzoate is 4.5. The volume of benzoic acid solution in 300 mL of this buffer solution is_____ mL.

[30-Jan-2024 Shift 2]

The pH of an aqueous solution containing 1M benzoic acid (pKa = 4.20) and 1M sodium benzoate is 4.5. The volume of benzoic acid solution in 300 mL of this buffer solution is_____ mL.

[30-Jan-2024 Shift 2]

Question 8/223

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Mark Review

Ka for CH₃COOH is 1.8 × 10⁻⁵ and Kb for NH₄OH is 1.8 × 10⁻⁵. The pH of ammonium acetate solution will be

[1-Feb-2024 Shift 1]

Ka for CH₃COOH is 1.8 × 10⁻⁵ and Kb for NH₄OH is 1.8 × 10⁻⁵. The pH of ammonium acetate solution will be

[1-Feb-2024 Shift 1]

Question 9/223

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Mark Review

Solubility of calcium phosphate (molecular mass, M) in water is W_g per 100mL at 25^∘C. Its solubility product at 25^∘C will be approximately.

[1-Feb-2024 Shift 2]

Solubility of calcium phosphate (molecular mass, M) in water is W_g per 100mL at 25^∘C. Its solubility product at 25^∘C will be approximately.

[1-Feb-2024 Shift 2]

A

B

C

D

Question 10/223

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Mark Review

The dissociation constant of acetic is x×10−5. When 25‌mL of 0.2M‌CH3‌COONa solution is mixed with 25‌mL of 0.02‌M‌CH3‌COOH solution, the pH of the resultant solution is found to be equal to 5 . The value of x is___

[24-Jan-2023 Shift 1]

The dissociation constant of acetic is x×10−5. When 25‌mL of 0.2M‌CH3‌COONa solution is mixed with 25‌mL of 0.02‌M‌CH3‌COOH solution, the pH of the resultant solution is found to be equal to 5 . The value of x is___

[24-Jan-2023 Shift 1]

Question 11/223

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Mark Review

If the pKa of lactic acid is 5 , then the pH of 0.005M calcium lactate solution at 25∘C is ______×10−1 (Nearest integer)
Lactic acid
CH3−

H

|

C

‌

|

OH

−COOH

[24-Jan-2023 Shift 2]

If the pKa of lactic acid is 5 , then the pH of 0.005M calcium lactate solution at 25∘C is ______×10−1 (Nearest integer)
Lactic acid
CH3−

H

|

C

‌

|

OH

−COOH

[24-Jan-2023 Shift 2]

Question 12/223

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Mark Review

A litre of buffer solution contains 0.1 mole of each of NH3 and NH4‌Cl. On the addition of 0.02 mole of HCl by dissolving gaseous HCl, the pH of the solution is found to be ________ ×10−3( Nearest integer)
[. Given : pKb(NH3)=4.745
log‌2=0.301
log‌3=0.477
T=298K]

[25-Jan-2023 Shift 1]

A litre of buffer solution contains 0.1 mole of each of NH3 and NH4‌Cl. On the addition of 0.02 mole of HCl by dissolving gaseous HCl, the pH of the solution is found to be ________ ×10−3( Nearest integer)
[. Given : pKb(NH3)=4.745
log‌2=0.301
log‌3=0.477
T=298K]

[25-Jan-2023 Shift 1]

Question 13/223

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Mark Review

When the hydrogen ion concentration [H+]changes by a factor of 1000 , the value of pH of the solution _______.

[25-Jan-2023 Shift 2]

When the hydrogen ion concentration [H+]changes by a factor of 1000 , the value of pH of the solution _______.

[25-Jan-2023 Shift 2]

A

increases by 1000 units

B

decreases by 3 units

C

decreases by 2 units

D

increases by 2 units

Question 14/223

4 / -1

Mark Review

Match List I with List II

Choose the correct answer from the options given below :-

[25-Jan-2023 Shift 2]

Match List I with List II

Choose the correct answer from the options given below :-

[25-Jan-2023 Shift 2]

A

A-I, B-IV, C-II, D-III

B

A-III, B-II, C-I, D-IV

C

A-III, B-II, C-IV, D-I

D

A-III, B-IV, C-II, D-I

Question 15/223

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Mark Review

Millimoles of calcium hydroxyide required to produce 100‌mL of the aqueous solution of pH‌12 is x×10−1. The value of x is _______(Nearest integer).
Assume complete dissociation.

[29-Jan-2023 Shift 1]

Millimoles of calcium hydroxyide required to produce 100‌mL of the aqueous solution of pH‌12 is x×10−1. The value of x is _______(Nearest integer).
Assume complete dissociation.

[29-Jan-2023 Shift 1]

Question 16/223

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Mark Review

600‌mL of 0.01M‌HCl is mixed with 400‌mL of 0.01MH2SO4. The pH of the mixture is _______ ×10−2. (Nearest integer)
[Given log‌2=0.30,‌‌log‌3=0.48
log‌5=0.69‌‌log‌7=0.84
log‌11=1.04]

[30-Jan-2023 Shift 1]

600‌mL of 0.01M‌HCl is mixed with 400‌mL of 0.01MH2SO4. The pH of the mixture is _______ ×10−2. (Nearest integer)
[Given log‌2=0.30,‌‌log‌3=0.48
log‌5=0.69‌‌log‌7=0.84
log‌11=1.04]

[30-Jan-2023 Shift 1]

Question 17/223

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Mark Review

The correct order of pKa values for the following compounds is:

[30-Jan-2023 Shift 2]

The correct order of pKa values for the following compounds is:

[30-Jan-2023 Shift 2]

A

c > a > d > b

B

b > d > a > c

C

b>a>d>c

D

a>b> c > d

Question 18/223

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Mark Review

The logarithm of equilibrium constant for the reaction Pd2++4Cl−⇌PdCl42− is _______ (Nearest integer)
‌‌ Given ‌:‌

2.303‌RT

F

=0.06V
‌Pd(aq)2++2e−⇌Pd( s)‌‌E∘=0.83V
‌PdCl42−(aq)+2e−⇌Pd( s)+4Cl−(aq)
‌E∘=0.65V

[31-Jan-2023 Shift 1]

The logarithm of equilibrium constant for the reaction Pd2++4Cl−⇌PdCl42− is _______ (Nearest integer)
‌‌ Given ‌:‌

2.303‌RT

F

=0.06V
‌Pd(aq)2++2e−⇌Pd( s)‌‌E∘=0.83V
‌PdCl42−(aq)+2e−⇌Pd( s)+4Cl−(aq)
‌E∘=0.65V

[31-Jan-2023 Shift 1]

Question 19/223

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Mark Review

Incorrect statement for the use of indicators in acid-base titration is :

[31-Jan-2023 Shift 2]

Incorrect statement for the use of indicators in acid-base titration is :

[31-Jan-2023 Shift 2]

A

Methyl orange may be used for a weak acid vs weak base titration.

B

Methyl orange is a suitable indicator for a strong acid vs weak base titration

C

Phenolphthalein is a suitable indicator for a weak acid vs strong base titration

D

Phenolphthalein may be used for a strong acid vs strong base titration.

Question 20/223

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Mark Review

At 298K, the solubility of silver chloride in water is 1.434×10−3gL−1. The value of −log‌K sp for silver chloride is
(Given mass of Ag is 107.9gmol−1 and mass of Cl is _______ 35.5gmol−1)

[31-Jan-2023 Shift 2]

At 298K, the solubility of silver chloride in water is 1.434×10−3gL−1. The value of −log‌K sp for silver chloride is
(Given mass of Ag is 107.9gmol−1 and mass of Cl is _______ 35.5gmol−1)

[31-Jan-2023 Shift 2]

Question 21/223

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Mark Review

Consider the following reaction approaching equilibrium at 27∘C and 1‌atm pressure
A+B

Kf=103

⇌

Kr=102

C+D
The standard Gibb's energy change (∆rG∘) at 27∘C is (-) _______ kJ‌mol−1
(Nearest integer).
(Given : R=8.3JK−1mol−1 and ln‌10=2.3 )

[29-Jan-2023 Shift 1]

Consider the following reaction approaching equilibrium at 27∘C and 1‌atm pressure
A+B

Kf=103

⇌

Kr=102

C+D
The standard Gibb's energy change (∆rG∘) at 27∘C is (-) _______ kJ‌mol−1
(Nearest integer).
(Given : R=8.3JK−1mol−1 and ln‌10=2.3 )

[29-Jan-2023 Shift 1]

Question 22/223

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Mark Review

At 298K
‌N2(g)+3H2(g)⇌2NH3(g),K1=4×105
‌N2(g)+O2(g)⇌2‌NO(g),K2=1.6×1012
‌H2(g)+‌

1

2

O2(g)⇌H2O(g),K3=1.0×10−13
Based on above equilibria, the equilibrium constant of the reaction,
2NH3(g)+‌

5

2

O2(g)⇌2‌NO(g)+3H2O(g)is _______ ×10−33
(Nearest integer)

[29-Jan-2023 Shift 2]

At 298K
‌N2(g)+3H2(g)⇌2NH3(g),K1=4×105
‌N2(g)+O2(g)⇌2‌NO(g),K2=1.6×1012
‌H2(g)+‌

1

2

O2(g)⇌H2O(g),K3=1.0×10−13
Based on above equilibria, the equilibrium constant of the reaction,
2NH3(g)+‌

5

2

O2(g)⇌2‌NO(g)+3H2O(g)is _______ ×10−33
(Nearest integer)

[29-Jan-2023 Shift 2]

Question 23/223

4 / -1

Mark Review

Consider the following equation:
2SO2(g)+O2(g)⇌2SO3(g),∆H=−190‌kJ
The number of factors which will increase the yield of SO3 at equilibrium from the following is _______
A. Increasing temperature
B. Increasing pressure
C. Adding more SO2
D. Adding more O2
E. Addition of catalyst

[30-Jan-2023 Shift 2]

Consider the following equation:
2SO2(g)+O2(g)⇌2SO3(g),∆H=−190‌kJ
The number of factors which will increase the yield of SO3 at equilibrium from the following is _______
A. Increasing temperature
B. Increasing pressure
C. Adding more SO2
D. Adding more O2
E. Addition of catalyst

[30-Jan-2023 Shift 2]

Question 24/223

4 / -1

Mark Review

For reaction: SO2(g)+‌

1

2

O2(g)⇌SO3(g) KP=2×1012 at 27∘C and 1 atm pressure. The Kc for the same reaction is _______ ×1013. (Nearest integer)
(Given R=0.082L‌atm‌K−1‌mol−1 )

[31-Jan-2023 Shift 1]

For reaction: SO2(g)+‌

1

2

O2(g)⇌SO3(g) KP=2×1012 at 27∘C and 1 atm pressure. The Kc for the same reaction is _______ ×1013. (Nearest integer)
(Given R=0.082L‌atm‌K−1‌mol−1 )

[31-Jan-2023 Shift 1]

Question 25/223

4 / -1

Mark Review

For independent process at 300 K.

The number of non-spontaneous process from the following is____

[24-Jan-2023 Shift 1]

For independent process at 300 K.

The number of non-spontaneous process from the following is____

[24-Jan-2023 Shift 1]

Question 26/223

4 / -1

Mark Review

Water decomposes at 2300K
H2O(g)→H2(g)+‌

1

2

O2(g)
The percent of water decomposing at 2300K and 1 bar is ________ (Nearest integer).
Equilibrium constant for the reaction is 2×10−3 at 2300K

[29-Jan-2023 Shift 1]

Water decomposes at 2300K
H2O(g)→H2(g)+‌

1

2

O2(g)
The percent of water decomposing at 2300K and 1 bar is ________ (Nearest integer).
Equilibrium constant for the reaction is 2×10−3 at 2300K

[29-Jan-2023 Shift 1]

Question 27/223

4 / -1

Mark Review

At 25∘C, the enthalpy of the following processes are given:
‌H2(g)+O2(g)→2‌OH(g)∆H0=78‌kJ‌mol−1
‌H2(g)+1∕2O2(g)→H2O(g)∆H0=−242‌kJ‌mol−1
‌H2(g)→2H(g)∆H0=436‌kJ‌mol−1
‌1∕2O2(g)→O(g)∆H0=249‌kJ‌mol−1
What would be the value of X for the following reaction? _______ (Nearest integer)
H2O(g)→H(g)+OH(g)∆Ho=X‌kJ‌mol−1

[1-Feb-2023 Shift 1]

At 25∘C, the enthalpy of the following processes are given:
‌H2(g)+O2(g)→2‌OH(g)∆H0=78‌kJ‌mol−1
‌H2(g)+1∕2O2(g)→H2O(g)∆H0=−242‌kJ‌mol−1
‌H2(g)→2H(g)∆H0=436‌kJ‌mol−1
‌1∕2O2(g)→O(g)∆H0=249‌kJ‌mol−1
What would be the value of X for the following reaction? _______ (Nearest integer)
H2O(g)→H(g)+OH(g)∆Ho=X‌kJ‌mol−1

[1-Feb-2023 Shift 1]

Question 28/223

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Mark Review

(i) X(g)⇌Y(g)+Z(g)Kp1=3
(ii) A(g)⇌2B(g)‌‌Kp2=1
If the degree of dissociation and initial concentration of both the reactants X(g) and A(g) are equal, then the ratio of the total pressure at equilibrium (‌

p1

p2

) is equal to x:1. The value of x is ________ (Nearest integer)

[1-Feb-2023 Shift 1]

(i) X(g)⇌Y(g)+Z(g)Kp1=3
(ii) A(g)⇌2B(g)‌‌Kp2=1
If the degree of dissociation and initial concentration of both the reactants X(g) and A(g) are equal, then the ratio of the total pressure at equilibrium (‌

p1

p2

) is equal to x:1. The value of x is ________ (Nearest integer)

[1-Feb-2023 Shift 1]

Question 29/223

4 / -1

Mark Review

The effect of addition of helium gas to the following reaction in equilibrium state, is :
PCI5(g)⇌PCl3(g)+Cl2(g)

[1-Feb-2023 Shift 2]

The effect of addition of helium gas to the following reaction in equilibrium state, is :
PCI5(g)⇌PCl3(g)+Cl2(g)

[1-Feb-2023 Shift 2]

*This question may have multiple correct answers

A

the equilibrium will shift in the forward direction and more of Cl2 and PCl3 gases will be produced.

B

the equilibrium will go backward due to suppression of dissociation of PCl5.

C

helium will deactivate PCl5 and reaction will stop.

D

addition of helium will not affect the equilibrium.

Question 30/223

4 / -1

Mark Review

For a concentrated solution of a weak electrolyte ( Keq= equilibrium constant) A2B3 of concentration ' c ', the degree of dissociation " α ' is

[6-Apr-2023 shift 1]

For a concentrated solution of a weak electrolyte ( Keq= equilibrium constant) A2B3 of concentration ' c ', the degree of dissociation " α ' is

[6-Apr-2023 shift 1]

A

(‌
Keq
108c4
)‌
1
5

B

(‌
Keq
6c5
)‌
1
5

C

(‌
Keq
5c4
)‌
1
5

D

(‌
Keq
25c2
)‌
1
5

Question 31/223

4 / -1

Mark Review

The number of correct statement/s involving equilibria in physical from the following is ________

[10-Apr-2023 shift 1]

The number of correct statement/s involving equilibria in physical from the following is ________

[10-Apr-2023 shift 1]

A

Equilibrium is possible only in a closed system at a given temperature.

B

Both the opposing processes occur at the same rate.

C

When equilibrium is attained at a given temperature, the value of all its parameters

D

For dissolution of solids in liquids, the solubility is constant at a given temperature.

Question 32/223

4 / -1

Mark Review

The equilibrium composition for the reaction PCl3+Cl2⇌PCl5 at 298K is given below.
[PCl3]eq‌=0.2‌mol‌L−1‌‌[Cl2]eq=0.1‌mol‌L−1,
[PCl5]eq‌=0.40‌mol‌L−1
If 0.2‌mol of Cl2 is added at the same temperature, the equilibrium concentrations of PCl5 is ______‌‌×10−2‌mol‌L−1 .
Given : Kc for the reaction at 298K is 20

[6-Apr-2023 shift 2]

The equilibrium composition for the reaction PCl3+Cl2⇌PCl5 at 298K is given below.
[PCl3]eq‌=0.2‌mol‌L−1‌‌[Cl2]eq=0.1‌mol‌L−1,
[PCl5]eq‌=0.40‌mol‌L−1
If 0.2‌mol of Cl2 is added at the same temperature, the equilibrium concentrations of PCl5 is ______‌‌×10−2‌mol‌L−1 .
Given : Kc for the reaction at 298K is 20

[6-Apr-2023 shift 2]

Question 33/223

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Mark Review

A mixture of 1 mole of H2O and 1 mole of CO is taken in a 10 litre container and heated to 725K. At equilibrium 40% of water by mass reacts with carbon monoxide according to the equation : CO(g)+H2O(g)⇌ CO2(g)+H2(g). The equilibrium constant Ke×102 for the reaction is ________ (Nearest integer)

[11-Apr-2023 shift 1]

A mixture of 1 mole of H2O and 1 mole of CO is taken in a 10 litre container and heated to 725K. At equilibrium 40% of water by mass reacts with carbon monoxide according to the equation : CO(g)+H2O(g)⇌ CO2(g)+H2(g). The equilibrium constant Ke×102 for the reaction is ________ (Nearest integer)

[11-Apr-2023 shift 1]

Question 34/223

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Mark Review

4.5 moles each of hydrogen and iodine is heated in a sealed ten litre vessel. At equilibrium, 3 moles of HI were found. The equilibrium constant for H2(g)+I2(g)⇌2‌HI(g) is ________

[11-Apr-2023 shift 2]

4.5 moles each of hydrogen and iodine is heated in a sealed ten litre vessel. At equilibrium, 3 moles of HI were found. The equilibrium constant for H2(g)+I2(g)⇌2‌HI(g) is ________

[11-Apr-2023 shift 2]

Question 35/223

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Mark Review

The titration curve of weak acid vs. strong base with phenolphthalein as indictor) is shown below. The K‌phenolphthalein ‌=4×10−10
Given :log‌2=0.3

The number of following statements/s which is/are correct about phenolphthalein is ________

[8-Apr-2023 shift 1]

The titration curve of weak acid vs. strong base with phenolphthalein as indictor) is shown below. The K‌phenolphthalein ‌=4×10−10
Given :log‌2=0.3

The number of following statements/s which is/are correct about phenolphthalein is ________

[8-Apr-2023 shift 1]

A

It can be used as an indicator for the titration of weak acid with weak base.

B

It begins to change colour at pH=8.4

C

It is a weak organic base

D

It is colourless in acidic medium

Question 36/223

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Mark Review

Given below are two statements :
Statement I : Methyl orange is a weak acid.
Statement II : The benzenoid form of methyl orange is more intense/deeply coloured than the quinonoid form.
In the light of the above statement, choose the most appropriate answer from the options given below:

[8-Apr-2023 shift 2]

Given below are two statements :
Statement I : Methyl orange is a weak acid.
Statement II : The benzenoid form of methyl orange is more intense/deeply coloured than the quinonoid form.
In the light of the above statement, choose the most appropriate answer from the options given below:

[8-Apr-2023 shift 2]

A

Both statement I and statement II are incorrect

B

Both statement I and Statement II are correct

C

Statement I is correct but statement II is incorrect

D

Statement I is incorrect but statement II is correct

Question 37/223

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Mark Review

The solubility product of BaSO4 is _______ 1×10−10 at 298K. The solubility of BaSO4 in 0.1MK2SO4 (aq) solut is ×10−9gL−1 (Nearest integer)
Given: Molar mass of BaSO4 is 233gmol−1

[8-Apr-2023 shift 2]

The solubility product of BaSO4 is _______ 1×10−10 at 298K. The solubility of BaSO4 in 0.1MK2SO4 (aq) solut is ×10−9gL−1 (Nearest integer)
Given: Molar mass of BaSO4 is 233gmol−1

[8-Apr-2023 shift 2]

Question 38/223

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Mark Review

An analyst wants to convert 1L‌HCl of pH=1 to a solution of HCl of pH‌2. The volume of water needed to do this dilution is _______ mL. (Nearest integer)

[12-Apr-2023 shift 1]

An analyst wants to convert 1L‌HCl of pH=1 to a solution of HCl of pH‌2. The volume of water needed to do this dilution is _______ mL. (Nearest integer)

[12-Apr-2023 shift 1]

Question 39/223

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Mark Review

25.0‌mL of 0.050‌MBa(NO3)2 is mixed with 25.0‌mL of 0.020M‌NaF.K sp of BaF2 is 0.5×10−6 at 298K. The ratio of [Ba2+][F−]2 and K sp is _________ . (Nearest integer)

[13-Apr-2023 shift 1]

25.0‌mL of 0.050‌MBa(NO3)2 is mixed with 25.0‌mL of 0.020M‌NaF.K sp of BaF2 is 0.5×10−6 at 298K. The ratio of [Ba2+][F−]2 and K sp is _________ . (Nearest integer)

[13-Apr-2023 shift 1]

Question 40/223

4 / -1

Mark Review

20‌mL of 0.1M‌NaOH is added to 50‌mL of 0.1M acetic acid solution. The pH of the resulting solution is _______ ×10−2 (Nearest integer)
‌‌ Given : ‌pKa(CH3‌COOH)=4.76
‌log‌2=0.30
‌log‌3=0.48

[13-Apr-2023 shift 2]

20‌mL of 0.1M‌NaOH is added to 50‌mL of 0.1M acetic acid solution. The pH of the resulting solution is _______ ×10−2 (Nearest integer)
‌‌ Given : ‌pKa(CH3‌COOH)=4.76
‌log‌2=0.30
‌log‌3=0.48

[13-Apr-2023 shift 2]

Question 41/223

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Mark Review

Which of the following statement(s) is/are correct?
(A) The pH of 1×10−8M‌HCl solution is 8
(B) The conjugate hase of H2PH4−is HPO42−
(C) Kw increases with increase in temperature.
(D) When a solution of a weak monoprotic acid is titrated against a strong base at half neutralisation point.
pH=‌

1

2

pKa
Choose the correct answer from the options given below

[15-Apr-2023 shift 1]

Which of the following statement(s) is/are correct?
(A) The pH of 1×10−8M‌HCl solution is 8
(B) The conjugate hase of H2PH4−is HPO42−
(C) Kw increases with increase in temperature.
(D) When a solution of a weak monoprotic acid is titrated against a strong base at half neutralisation point.
pH=‌

1

2

pKa
Choose the correct answer from the options given below

[15-Apr-2023 shift 1]

A

(A), (B). (C)

B

(A), (D)

C

(B), (C)

D

(B), (C). (D)

Question 42/223

4 / -1

Mark Review

For a reaction at equilibrium
A(g)⇌B(g)+‌

1

2

C(g)
the relation between dissociation constant (K), degree of dissociation (α) and equilibrium pressure (p) is given by:

[24-Jun-2022-Shift-1]

For a reaction at equilibrium
A(g)⇌B(g)+‌

1

2

C(g)
the relation between dissociation constant (K), degree of dissociation (α) and equilibrium pressure (p) is given by:

[24-Jun-2022-Shift-1]

A

K=‌
α
1
2
p
3
2
(1+‌
3
2
α)‌
1
2
(1−α)

B

K=‌
α
3
2
p
1
2
(2+α)‌
1
2
(1−α)

C

K=‌
(αp)
3
2
(1+‌
3
2
α)‌
1
2
(1−α)

D

K=‌
(αp)
3
2
(1+α)(1−α)‌
1
2

Question 43/223

4 / -1

Mark Review

PCl5 dissociates as
PCl5(g)⇌PCl3(g)+Cl2(g)
5 moles of PCl5 are placed in a 200 litre vessel which contains 2 moles of N2 and is maintained at 600 K. The equilibrium prẽššưre is 2.46‌atm. The equilibrium constant Kp for the dissociation of PCl5 is ____×10−3. (nearest integer)
(Given : R=0.082Latm−1mol−1; Assume ideal gas behaviour)

[24-Jun-2022-Shift-2]

PCl5 dissociates as
PCl5(g)⇌PCl3(g)+Cl2(g)
5 moles of PCl5 are placed in a 200 litre vessel which contains 2 moles of N2 and is maintained at 600 K. The equilibrium prẽššưre is 2.46‌atm. The equilibrium constant Kp for the dissociation of PCl5 is ____×10−3. (nearest integer)
(Given : R=0.082Latm−1mol−1; Assume ideal gas behaviour)

[24-Jun-2022-Shift-2]

Question 44/223

4 / -1

Mark Review

The standard free energy change (∆G∘) for 50% dissociation of N2O4 into NO2 at 27∘C and 1 atm pressure is −xJmol−1. The value of x is_______ (Nearest Integer)
[Given : .R=8.31JK−1mol−1,log‌1.33=0.1239‌ln‌10=2.3]

[25-Jun-2022-Shift-1]

The standard free energy change (∆G∘) for 50% dissociation of N2O4 into NO2 at 27∘C and 1 atm pressure is −xJmol−1. The value of x is_______ (Nearest Integer)
[Given : .R=8.31JK−1mol−1,log‌1.33=0.1239‌ln‌10=2.3]

[25-Jun-2022-Shift-1]

Question 45/223

4 / -1

Mark Review

2‌NOCl(g)⇌2‌NO(g)+Cl2(g)
In an experiment, 2.0 moles of NOCl was placed in a one-litre flask and the concentration of NO after equilibrium established, was found to be 0.4‌mol∕L. The equilibrium constant at 30∘C is______ ×10−4

[27-Jun-2022-Shift-1]

2‌NOCl(g)⇌2‌NO(g)+Cl2(g)
In an experiment, 2.0 moles of NOCl was placed in a one-litre flask and the concentration of NO after equilibrium established, was found to be 0.4‌mol∕L. The equilibrium constant at 30∘C is______ ×10−4

[27-Jun-2022-Shift-1]

Question 46/223

4 / -1

Mark Review

4.0 moles of argon and 5.0 moles of PCl5 are introduced into an evacuated flask of 100 litre capacity at 610K. The system is allowed to equilibrate. At equilibrium, the total pressure of mixture was found to be 6.0‌atm. The Kp for the reaction is
[Given : .R=0.082L‌atm‌K−1‌mol−1]

[29-Jun-2022-Shift-2]

4.0 moles of argon and 5.0 moles of PCl5 are introduced into an evacuated flask of 100 litre capacity at 610K. The system is allowed to equilibrate. At equilibrium, the total pressure of mixture was found to be 6.0‌atm. The Kp for the reaction is
[Given : .R=0.082L‌atm‌K−1‌mol−1]

[29-Jun-2022-Shift-2]

A

2.25

B

6.24

C

12.13

D

15.24

15.24 Question 47/223

4 / -1

Mark Review

A box contains 0.90g of liquid water in equilibrium with water vapour at 27∘C. The equilibrium vapour pressure of water at 27 ‌∘C is 32.0 Torr. When the volume of the box is increased, some of the liquid water evaporates to maintain the equilibrium pressure. If all the liquid water evaporates, then the volume of the box must be ____litre. [nearest integer]
(Given : R=0.082L‌atm‌K−1‌mol−1 )
(Ignore the volume of the liquid water and assume water vapours behave as an ideal gas.)

[29-Jun-2022-Shift-2]

A box contains 0.90g of liquid water in equilibrium with water vapour at 27∘C. The equilibrium vapour pressure of water at 27 ‌∘C is 32.0 Torr. When the volume of the box is increased, some of the liquid water evaporates to maintain the equilibrium pressure. If all the liquid water evaporates, then the volume of the box must be ____litre. [nearest integer]
(Given : R=0.082L‌atm‌K−1‌mol−1 )
(Ignore the volume of the liquid water and assume water vapours behave as an ideal gas.)

[29-Jun-2022-Shift-2]

Question 48/223

4 / -1

Mark Review

Solute A associates in water. When 0.7g of solute A is dissolved in 42.0g of water, it depresses the freezing point by 0.2∘C. The percentage association of solute A in water, is :
[Given : Molar mass of A=93gmol−1. Molal depression constant of water is 1.86K‌kg‌mol−1.]

[25-Jun-2022-Shift-2]

Solute A associates in water. When 0.7g of solute A is dissolved in 42.0g of water, it depresses the freezing point by 0.2∘C. The percentage association of solute A in water, is :
[Given : Molar mass of A=93gmol−1. Molal depression constant of water is 1.86K‌kg‌mol−1.]

[25-Jun-2022-Shift-2]

A

50%

B

60%

C

70%

D

80%

Question 49/223

4 / -1

Mark Review

Given below are two statements one is labelled as Assertion A and the other is labelled as Reason R :
Assertion A : The amphoteric nature of water is explained by using Lewis acid/base concept.
Reason R: Water acts as an acid with NH3 and as a base with H2S.
In the light of the above statements choose the correct answer from the options given below :

[25-Jun-2022-Shift-2]

Given below are two statements one is labelled as Assertion A and the other is labelled as Reason R :
Assertion A : The amphoteric nature of water is explained by using Lewis acid/base concept.
Reason R: Water acts as an acid with NH3 and as a base with H2S.
In the light of the above statements choose the correct answer from the options given below :

[25-Jun-2022-Shift-2]

A

Both A and R are true and R is the correct explanation of A.

B

Both A and R are true but R is NOT the correct explanation of A.

C

A is true but R is false.

D

A is false but R is true.

Question 50/223

4 / -1

Mark Review

50‌mL of 0.1MCH3‌COOH is being titrated against 0.1M‌NaOH. When 25‌mL of NaOH has been added, the pH of the solution will be ____×10−2. (Nearest integer)
(Given : .pKa(CH3‌COOH)=4.76)
log‌2=0.30
log‌3=0.48
log‌5=0.69
log‌7=0.84
log‌11=1.04

[26-Jun-2022-Shift-1]

50‌mL of 0.1MCH3‌COOH is being titrated against 0.1M‌NaOH. When 25‌mL of NaOH has been added, the pH of the solution will be ____×10−2. (Nearest integer)
(Given : .pKa(CH3‌COOH)=4.76)
log‌2=0.30
log‌3=0.48
log‌5=0.69
log‌7=0.84
log‌11=1.04

[26-Jun-2022-Shift-1]

Question 51/223

4 / -1

Mark Review

pH value of 0.001M‌NaOH solution is___

[27-Jun-2022-Shift-2]

pH value of 0.001M‌NaOH solution is___

[27-Jun-2022-Shift-2]

Question 52/223

4 / -1

Mark Review

A student needs to prepare a buffer solution of propanoic acid and its sodium salt with pH 4. The ratio of ‌

[CH3CH2COO−]

[CH3CH2‌COOH].

required to make buffer is
Given : Ka(CH3CH2‌COOH)=1.3×10−5

[28-Jun-2022-Shift-2]

A student needs to prepare a buffer solution of propanoic acid and its sodium salt with pH 4. The ratio of ‌

[CH3CH2COO−]

[CH3CH2‌COOH].

required to make buffer is
Given : Ka(CH3CH2‌COOH)=1.3×10−5

[28-Jun-2022-Shift-2]

A

0.03

B

0.13

C

0.23

D

0.33

0.33 Question 53/223

4 / -1

Mark Review

The solubility of AgCl will be maximum in which of the following?

[29-Jun-2022-Shift-1]

The solubility of AgCl will be maximum in which of the following?

[29-Jun-2022-Shift-1]

A

0.01M‌KCl

B

0.01M‌HCl

C

0.01MAgNO3

D

Deionised water

Question 54/223

4 / -1

Mark Review

Ka1,Ka2 and Ka3 are the respective ionization constants for the following reactions (a), (b) and (c).
(a) H2C2O4⇄H++HC2O4−
(b) HC2O4−⇄H++HC2O42−
(c) H2C2O4⇄2H++C2O42−
The relationship between Ka1,Ka2 and Ka3 is given as

[25-Jul-2022-Shift-2]

Ka1,Ka2 and Ka3 are the respective ionization constants for the following reactions (a), (b) and (c).
(a) H2C2O4⇄H++HC2O4−
(b) HC2O4−⇄H++HC2O42−
(c) H2C2O4⇄2H++C2O42−
The relationship between Ka1,Ka2 and Ka3 is given as

[25-Jul-2022-Shift-2]

A

Ka3=Ka1+Ka2

B

Ka3=Ka1−Ka2

C

Ka3=Ka1∕Ka2

D

Ka3=Ka1×Ka2

Question 55/223

4 / -1

Mark Review

At 298K, the equilibrium constant is 2×1015 for the reaction :
Cu(s)+2Ag+(aq)⇌Cu2+(aq)+2‌Ag(s)
The equilibrium constant for the reaction
‌

1

2

Cu2+(aq)+Ag(s)⇌‌

1

2

‌Cu(s)+Ag+(aq)
is x×10−8. The value of x is ________. (Nearest Integer)

[26-Jul-2022-Shift-1]

At 298K, the equilibrium constant is 2×1015 for the reaction :
Cu(s)+2Ag+(aq)⇌Cu2+(aq)+2‌Ag(s)
The equilibrium constant for the reaction
‌

1

2

Cu2+(aq)+Ag(s)⇌‌

1

2

‌Cu(s)+Ag+(aq)
is x×10−8. The value of x is ________. (Nearest Integer)

[26-Jul-2022-Shift-1]

Question 56/223

4 / -1

Mark Review

At 600K,2‌mol of NO are mixed with 1‌mol of O2.
2NO(g)+O2(g)⇄2NO2(g)
The reaction occurring as above comes to equilibrium under a total pressure of 1‌atm. Analysis of the system shows that 0.6‌mol of oxygen are present at equilibrium. The equilibrium constant for the reaction is ____(Nearest integer)

[28-Jul-2022-Shift-2]

At 600K,2‌mol of NO are mixed with 1‌mol of O2.
2NO(g)+O2(g)⇄2NO2(g)
The reaction occurring as above comes to equilibrium under a total pressure of 1‌atm. Analysis of the system shows that 0.6‌mol of oxygen are present at equilibrium. The equilibrium constant for the reaction is ____(Nearest integer)

[28-Jul-2022-Shift-2]

Question 57/223

4 / -1

Mark Review

20‌mL of 0.1 MNH4‌OH is mixed with 40‌mL of 0.05‌MHCl. The pH of the mixture is nearest to:
(Given: Kb(NH4‌OH)=1×10−5,log‌2=0.30,log‌3=0.48,log‌5=0.69,log‌7=0.84,log‌11=1.04 )

[25-Jul-2022-Shift-1]

20‌mL of 0.1 MNH4‌OH is mixed with 40‌mL of 0.05‌MHCl. The pH of the mixture is nearest to:
(Given: Kb(NH4‌OH)=1×10−5,log‌2=0.30,log‌3=0.48,log‌5=0.69,log‌7=0.84,log‌11=1.04 )

[25-Jul-2022-Shift-1]

A

3.2

B

4.2

C

5.2

D

6.2

6.2 Question 58/223

4 / -1

Mark Review

Class XII students were asked to prepare one litre of buffer solution of pH‌8.26 by their Chemistry teacher: The amount of ammonium chloride to be dissolved by the student in 0.2M ammonia solution to make one litre of the buffer is
(Given: pKb(NH3)=4.74
Molar mass of NH3=17gmol−1
Molar mass of NH4‌Cl=53.5gmol−1 )

[26-Jul-2022-Shift-2]

Class XII students were asked to prepare one litre of buffer solution of pH‌8.26 by their Chemistry teacher: The amount of ammonium chloride to be dissolved by the student in 0.2M ammonia solution to make one litre of the buffer is
(Given: pKb(NH3)=4.74
Molar mass of NH3=17gmol−1
Molar mass of NH4‌Cl=53.5gmol−1 )

[26-Jul-2022-Shift-2]

A

53.5g

B

72.3g

C

107.0g

D

126.0g

Question 59/223

4 / -1

Mark Review

At 310K, the solubility of CaF2 in water is 2.34×10−3g∕100‌mL. The solubility product of CaF2 is _______ ×10−8(mol∕L)3. (Give molar mass : CaF2=78gmol−1 )

[27-Jul-2022-Shift-1]

At 310K, the solubility of CaF2 in water is 2.34×10−3g∕100‌mL. The solubility product of CaF2 is _______ ×10−8(mol∕L)3. (Give molar mass : CaF2=78gmol−1 )

[27-Jul-2022-Shift-1]

Question 60/223

4 / -1

Mark Review

The plot of pH-metric titration of weak base NH4‌OH vs strong acid HCl looks like :

[27-Jul-2022-Shift-2]

The plot of pH-metric titration of weak base NH4‌OH vs strong acid HCl looks like :

[27-Jul-2022-Shift-2]

A

B

C

D

Question 61/223

4 / -1

Mark Review

Ka for butyric acid (C3H7‌COOH) is 2×10−5. The pH of 0.2M solution of butyric acid is _______ ×10−1. (Nearest integer)
[Given log‌2=0.30]

[28-Jul-2022-Shift-1]

Ka for butyric acid (C3H7‌COOH) is 2×10−5. The pH of 0.2M solution of butyric acid is _______ ×10−1. (Nearest integer)
[Given log‌2=0.30]

[28-Jul-2022-Shift-1]

Question 62/223

4 / -1

Mark Review

If the solubility product of PbS is 8×10−28, then the solubility of PbS in pure water at 298K is ××10 −16‌mol‌L−1. The value of x is _______. (Nearest Integer)
[Given : √2=1.41 ]

[29-Jul-2022-Shift-1]

If the solubility product of PbS is 8×10−28, then the solubility of PbS in pure water at 298K is ××10 −16‌mol‌L−1. The value of x is _______. (Nearest Integer)
[Given : √2=1.41 ]

[29-Jul-2022-Shift-1]

Question 63/223

4 / -1

Mark Review

200‌mL of 0.01‌MHCl is mixed with 400‌mL of 0.01MH2SO4. The pH of the mixture is _______.
Given: log‌2=0.30,log‌3=0.48,log‌5=0.70,log‌7=0.84,log‌11=1.04

[29-Jul-2022-Shift-2]

200‌mL of 0.01‌MHCl is mixed with 400‌mL of 0.01MH2SO4. The pH of the mixture is _______.
Given: log‌2=0.30,log‌3=0.48,log‌5=0.70,log‌7=0.84,log‌11=1.04

[29-Jul-2022-Shift-2]

A

1.14

B

1.78

C

2.34

D

3.02

3.02 Question 64/223

4 / -1

Mark Review

The solubility of Ca(OH)2 in water is [Given: The solubility product of Ca(OH)2 in water =5.5×10−6 ]

[25 Feb 2021 Shift 2]

The solubility of Ca(OH)2 in water is [Given: The solubility product of Ca(OH)2 in water =5.5×10−6 ]

[25 Feb 2021 Shift 2]

A

1.11×10−2

B

1.11×10−6

C

1.77×10−2

D

1.77×10−6

Question 65/223

4 / -1

Mark Review

The solubility product of Pbl2 is 8.0×10−9. The solubility of lead iodide in 0.1 molar solution of lead nitrate is x×10−6mol∕L. The value of x is ....... (Rounded off to the nearest integer).
[Given, : √2=1.41 ]

[24 Feb 2021 Shift 2]

The solubility product of Pbl2 is 8.0×10−9. The solubility of lead iodide in 0.1 molar solution of lead nitrate is x×10−6mol∕L. The value of x is ....... (Rounded off to the nearest integer).
[Given, : √2=1.41 ]

[24 Feb 2021 Shift 2]

Question 66/223

4 / -1

Mark Review

The pH of ammonium phosphate solution, if pKa of phosphoric acid and pKb of ammonium hydroxide are 5.23 and 4.75 respectively, is .......... .

[26 Feb 2021 Shift 2]

The pH of ammonium phosphate solution, if pKa of phosphoric acid and pKb of ammonium hydroxide are 5.23 and 4.75 respectively, is .......... .

[26 Feb 2021 Shift 2]

Question 67/223

4 / -1

Mark Review

The solubility of AgCN in a buffer solution of pH=3 is x. The value of x is...... .
[Assume : No cyano complex is formed; Ksp(AgCN)=2.2×10−16 and Ka(HCN)=6.2×10−10]

[25 Feb 2021 Shift 1]

The solubility of AgCN in a buffer solution of pH=3 is x. The value of x is...... .
[Assume : No cyano complex is formed; Ksp(AgCN)=2.2×10−16 and Ka(HCN)=6.2×10−10]

[25 Feb 2021 Shift 1]

A

0.625×10−6

B

1.6×10−6

C

2.2×10−16

D

1.9×10−5

Question 68/223

4 / -1

Mark Review

A homogeneous ideal gaseous reaction AB2(g)⇌A(g)+2B(g) is carried out in a 25L flask at 27∘C. The initial amount of AB2 was 1 mole and the equilibrium pressure was 1.9atm. The value of Kp is x×10−2. The value of x is ............ .

[26 Feb 2021 Shift 1]

A homogeneous ideal gaseous reaction AB2(g)⇌A(g)+2B(g) is carried out in a 25L flask at 27∘C. The initial amount of AB2 was 1 mole and the equilibrium pressure was 1.9atm. The value of Kp is x×10−2. The value of x is ............ .

[26 Feb 2021 Shift 1]

Question 69/223

4 / -1

Mark Review

At 1990K and 1atm pressure, there are equal number of Cl2 molecules and Cl atoms in the reaction mixture. The value of KP for the reaction Cl2(g)⇌2Cl(g) under the above conditions is x×10−1. The value of x is___ (Rounded off to the nearest integer)

[24feb2021shift1]

At 1990K and 1atm pressure, there are equal number of Cl2 molecules and Cl atoms in the reaction mixture. The value of KP for the reaction Cl2(g)⇌2Cl(g) under the above conditions is x×10−1. The value of x is___ (Rounded off to the nearest integer)

[24feb2021shift1]

Question 70/223

4 / -1

Mark Review

For the reaction A(g)→(B)(g), the value of the equilibrium constant at 300K and 1atm is equal to 100.0. The value of ∆rG for the reaction at 300K and 1atm in Jmol−1 is −xR, where x is________ (Rounded off to the nearest integer) (R=8.31‌J‌mol−1‌K−1 and ln‌10=2.3)

[24feb2021shift1]

For the reaction A(g)→(B)(g), the value of the equilibrium constant at 300K and 1atm is equal to 100.0. The value of ∆rG for the reaction at 300K and 1atm in Jmol−1 is −xR, where x is________ (Rounded off to the nearest integer) (R=8.31‌J‌mol−1‌K−1 and ln‌10=2.3)

[24feb2021shift1]

Question 71/223

4 / -1

Mark Review

The solubility of CdSO4 in water is 8.0×10−4molL−1. Its solubility in 0.01M H2SO4 solution is ........ ×10−6molL−1. (Round off to the nearest integer) (Assume that, solubility is much less than 0.01M )

[18 Mar 2021 Shift 2]

The solubility of CdSO4 in water is 8.0×10−4molL−1. Its solubility in 0.01M H2SO4 solution is ........ ×10−6molL−1. (Round off to the nearest integer) (Assume that, solubility is much less than 0.01M )

[18 Mar 2021 Shift 2]

Question 72/223

4 / -1

Mark Review

The oxygen dissolved in water exerts a partial pressure of 20kPa in the vapour above water. The molar solubility of oxygen in water is ..... ×10−5mol‌dm−3. (Round off to the nearest integer).
[Given, Henry's law constant (KH) =8.0×104kPa for O2, density of water with dissolved oxygen =1.0kgdm−3 ].

[17 Mar 2021 Shift 1]

The oxygen dissolved in water exerts a partial pressure of 20kPa in the vapour above water. The molar solubility of oxygen in water is ..... ×10−5mol‌dm−3. (Round off to the nearest integer).
[Given, Henry's law constant (KH) =8.0×104kPa for O2, density of water with dissolved oxygen =1.0kgdm−3 ].

[17 Mar 2021 Shift 1]

Question 73/223

4 / -1

Mark Review

Two salts A2X and MX have the same value of solubility product of 4.0×10−12. The ratio of their molar solubilities i.e ‌

S(A2X)

S(MX)

=......
(Round off to the nearest integer)

[16 Mar 2021 Shift 1]

Two salts A2X and MX have the same value of solubility product of 4.0×10−12. The ratio of their molar solubilities i.e ‌

S(A2X)

S(MX)

=......
(Round off to the nearest integer)

[16 Mar 2021 Shift 1]

Question 74/223

4 / -1

Mark Review

0.01 moles of a weak acid HA(Ka=2.0×10−6) is dissolved in 1.0L of 0.1MHCl solution. The degree of dissociation of HA is ...... ×10−5 (Round off to the nearest integer). [Neglect volume change on adding HA. Assume degree of dissociation ≪<1 ]

[17 Mar 2021 Shift 1]

0.01 moles of a weak acid HA(Ka=2.0×10−6) is dissolved in 1.0L of 0.1MHCl solution. The degree of dissociation of HA is ...... ×10−5 (Round off to the nearest integer). [Neglect volume change on adding HA. Assume degree of dissociation ≪<1 ]

[17 Mar 2021 Shift 1]

Question 75/223

4 / -1

Mark Review

Given below are two statements: One is labelled as Assertion A and the other labelled as Reason R.
Assertion A During the boiling of water having temporary hardness, Mg(HCO3)2 is converted to MgCO3 .
Reason R The solubility product of Mg(OH)2 is greater than that of MgCO3.
In the light of the above statements, choose the most appropriate answer from the options given below

[18 Mar 2021 Shift 1]

Given below are two statements: One is labelled as Assertion A and the other labelled as Reason R.
Assertion A During the boiling of water having temporary hardness, Mg(HCO3)2 is converted to MgCO3 .
Reason R The solubility product of Mg(OH)2 is greater than that of MgCO3.
In the light of the above statements, choose the most appropriate answer from the options given below

[18 Mar 2021 Shift 1]

A

Both A and R are true but R is not the correct explanation of A.

B

A is true but R is fals

C

Both A and R are true and R is the correct explanation of A.

D

A is false but R is true.

Question 76/223

4 / -1

Mark Review

The gas phase reaction
2A(g)⇌A2(g)
at 400K has ∆G∘=+25.2kJmol−1. The equilibrium constant KC for this reaction is .......... ×10−2. (Round off to the nearest integer).
[Use : R=8.3Jmol−1K−1,ln‌10=2.3 ] log1022=0.30,1atm=1bar] [antilog (−0.3)=0.501 ]

[18 Mar 2021 Shift 2]

The gas phase reaction
2A(g)⇌A2(g)
at 400K has ∆G∘=+25.2kJmol−1. The equilibrium constant KC for this reaction is .......... ×10−2. (Round off to the nearest integer).
[Use : R=8.3Jmol−1K−1,ln‌10=2.3 ] log1022=0.30,1atm=1bar] [antilog (−0.3)=0.501 ]

[18 Mar 2021 Shift 2]

Question 77/223

4 / -1

Mark Review

Consider the reaction, N2O4(g)⇌2NO2(g). The temperature at which KC=20.4 and Kp=600.1, is ............ K. (Round off to the nearest integer). [Assume all gases are ideal and R=0.0831L bar, K−1mol−1].

[17 Mar 2021 Shift 2]

Consider the reaction, N2O4(g)⇌2NO2(g). The temperature at which KC=20.4 and Kp=600.1, is ............ K. (Round off to the nearest integer). [Assume all gases are ideal and R=0.0831L bar, K−1mol−1].

[17 Mar 2021 Shift 2]

Question 78/223

4 / -1

Mark Review

For the reaction, A(g)⇌B(g) at 495K, ∆,G∘=−9.478kJmol−1. If we start the reaction in a closed container at 495K with 22 millimoles of A, the amount of B is the equilibrium mixture is ......... millimoles (Round off to the nearest integer). [R=8.314Jmol−1K−1,ln‌10=2.303]

[16 Mar 2021 Shift 1]

For the reaction, A(g)⇌B(g) at 495K, ∆,G∘=−9.478kJmol−1. If we start the reaction in a closed container at 495K with 22 millimoles of A, the amount of B is the equilibrium mixture is ......... millimoles (Round off to the nearest integer). [R=8.314Jmol−1K−1,ln‌10=2.303]

[16 Mar 2021 Shift 1]

Question 79/223

4 / -1

Mark Review

In order to prepare a buffer solution of pH 5.74, sodium acetate is added to acetic acid. If the concentration of acetic acid in the buffer is 1.0M, the concentration of sodium acetate in the buffer is ............ M. (Round off to the nearest integer). [Given : pKa (acetic acid =4.74]

[18 Mar 2021 Shift 1]

In order to prepare a buffer solution of pH 5.74, sodium acetate is added to acetic acid. If the concentration of acetic acid in the buffer is 1.0M, the concentration of sodium acetate in the buffer is ............ M. (Round off to the nearest integer). [Given : pKa (acetic acid =4.74]

[18 Mar 2021 Shift 1]

Question 80/223

4 / -1

Mark Review

Sulphurous acid (H2SO3) has Ka1=1.7×10−2 and Ka2=6.4×10−8. The pH of 0.588M is (Round off to the nearest integer)

[16 Mar 2021 Shift 2]

Sulphurous acid (H2SO3) has Ka1=1.7×10−2 and Ka2=6.4×10−8. The pH of 0.588M is (Round off to the nearest integer)

[16 Mar 2021 Shift 2]

Question 81/223

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Mark Review

Assuming that Ba(OH)2 is completely ionised in aqueous solution under the given conditions the concentration of H3O+ions in 0.005M aqueous solution of Ba(OH)2 at 298K is __________ ×10−12molL−1. (Nearest integer)

[25 Jul 2021 Shift 2]

Assuming that Ba(OH)2 is completely ionised in aqueous solution under the given conditions the concentration of H3O+ions in 0.005M aqueous solution of Ba(OH)2 at 298K is __________ ×10−12molL−1. (Nearest integer)

[25 Jul 2021 Shift 2]

Question 82/223

4 / -1

Mark Review

A solution is 0.1M in Cl−and 0.001M in CrO42−.
Solid AgNO3 is gradually added to it Assuming that the addition does not change in volume and Ksp (AgCl)=1.7×10−10M2 andKsp(Ag2CrO4)=1.9×10−12M3
Select correct statement from the following:

[20 Jul 2021 Shift 2]

A solution is 0.1M in Cl−and 0.001M in CrO42−.
Solid AgNO3 is gradually added to it Assuming that the addition does not change in volume and Ksp (AgCl)=1.7×10−10M2 andKsp(Ag2CrO4)=1.9×10−12M3
Select correct statement from the following:

[20 Jul 2021 Shift 2]

A

AgCl precipitates first because its Ksp is high.

B

Ag2CrO4 precipitates first as its Ksp is low.

C

Ag2CrO4 precipitates first because the amount of Ag+needed is low.

D

AgCl will precipitate first as the amount of Ag+ needed to precipitate is low.

Question 83/223

4 / -1

Mark Review

The equilibrium constant for the reaction
A(s)⇌M(s)+

1

2

O2(g)
is Kp=4. At equilibrium, the partial pressure of O2 is _____ atm. (Round off to the nearest integer)

[27 Jul 2021 Shift 2]

The equilibrium constant for the reaction
A(s)⇌M(s)+

1

2

O2(g)
is Kp=4. At equilibrium, the partial pressure of O2 is _____ atm. (Round off to the nearest integer)

[27 Jul 2021 Shift 2]

Question 84/223

4 / -1

Mark Review

2SO2(g)+O2(g)→2SO3(g)
The above reaction is carried out in a vessel starting with partial pressure PSO2=250m barPO2=750m bar and PSO3=0 bar . When the reaction is complete, the total pressure in the reaction vessel is _____ m bar. (Round off of the nearest integer).

[27 Jul 2021 Shift 2]

2SO2(g)+O2(g)→2SO3(g)
The above reaction is carried out in a vessel starting with partial pressure PSO2=250m barPO2=750m bar and PSO3=0 bar . When the reaction is complete, the total pressure in the reaction vessel is _____ m bar. (Round off of the nearest integer).

[27 Jul 2021 Shift 2]

Question 85/223

4 / -1

Mark Review

PCl5⇌PCl3+Cl3‌‌‌Kc=1.844
3.0 moles of PCl5 is introduced in a 1L closed reaction vessel at 380K. The number of moles ofPCl5 at equilibrium is _______ ×10−3
(Round off to the Nearest Integer)

[27 Jul 2021 Shift 1]

PCl5⇌PCl3+Cl3‌‌‌Kc=1.844
3.0 moles of PCl5 is introduced in a 1L closed reaction vessel at 380K. The number of moles ofPCl5 at equilibrium is _______ ×10−3
(Round off to the Nearest Integer)

[27 Jul 2021 Shift 1]

Question 86/223

4 / -1

Mark Review

Value of Kp for the equilibrium reaction
N2O4⇌2NO2(g) at 288K is 47.9. The KC for this reaction at same temperature is _______. (Nearest integer)
(R=0.083L. bar K−1mol−1)

[22 Jul 2021 Shift 2]

Value of Kp for the equilibrium reaction
N2O4⇌2NO2(g) at 288K is 47.9. The KC for this reaction at same temperature is _______. (Nearest integer)
(R=0.083L. bar K−1mol−1)

[22 Jul 2021 Shift 2]

Question 87/223

4 / -1

Mark Review

2SO2(g)+O2(g)⇌2SO3(g)
In an equilibrium mixture, the partial pressures are
PSO3=43kPa;PO2=530Pa andPSO2=45kPa. The equilibrium constant KP= ______×10−2. (Nearest integer)

[20 Jul 2021 Shift 1]

2SO2(g)+O2(g)⇌2SO3(g)
In an equilibrium mixture, the partial pressures are
PSO3=43kPa;PO2=530Pa andPSO2=45kPa. The equilibrium constant KP= ______×10−2. (Nearest integer)

[20 Jul 2021 Shift 1]

Question 88/223

4 / -1

Mark Review

A3B2 is a sparingly soluble salt of molar mass M(gmol−1) and solubility xgL−1. The solubility product satisfies Ksp=a(

x

M

)5.
The value of a is ......... (Integer answer)

[31 Aug 2021 Shift 1]

A3B2 is a sparingly soluble salt of molar mass M(gmol−1) and solubility xgL−1. The solubility product satisfies Ksp=a(

x

M

)5.
The value of a is ......... (Integer answer)

[31 Aug 2021 Shift 1]

Question 89/223

4 / -1

Mark Review

The pH of a solution obtained by mixing 50‌mL of 1M‌HCl and 30‌mL of 1M‌NaOH is x×10−4. The value of x is ........ (Nearest integer)
[log‌2.5=0.3979]

[31 Aug 2021 Shift 2]

The pH of a solution obtained by mixing 50‌mL of 1M‌HCl and 30‌mL of 1M‌NaOH is x×10−4. The value of x is ........ (Nearest integer)
[log‌2.5=0.3979]

[31 Aug 2021 Shift 2]

Question 90/223

4 / -1

Mark Review

The number of moles of NH3, that must be added to 2L of 0.80MAgNO3 in order to reduce the concentration of Ag+ ions to 5.0×10−8M (Kformation for [Ag(NH3)2]+=1.0×108) is.......... (Nearestinteger)
[Assume no volume change on adding NH3]

[27 Aug 2021 Shift 1]

The number of moles of NH3, that must be added to 2L of 0.80MAgNO3 in order to reduce the concentration of Ag+ ions to 5.0×10−8M (Kformation for [Ag(NH3)2]+=1.0×108) is.......... (Nearestinteger)
[Assume no volume change on adding NH3]

[27 Aug 2021 Shift 1]

Question 91/223

4 / -1

Mark Review

The number of moles of NH3, that must be added to 2L of 0.80MAgNO3 in order to reduce the concentration of Ag+ ions to 5.0×10−8M (Kformation for [Ag(NH3)2]+=1.0×108) is.......... (Nearestinteger)
[Assume no volume change on adding NH3]

[27 Aug 2021 Shift 1]

The number of moles of NH3, that must be added to 2L of 0.80MAgNO3 in order to reduce the concentration of Ag+ ions to 5.0×10−8M (Kformation for [Ag(NH3)2]+=1.0×108) is.......... (Nearestinteger)
[Assume no volume change on adding NH3]

[27 Aug 2021 Shift 1]

Question 92/223

4 / -1

Mark Review

The equilibrium constant Kc at 298K for the reaction A+B⇌C+D is 100 . Starting with an equimolar solution with concentrations of A, B, C and D all equal to 1M, the equilibrium concentration of D is ...........×10−2M. (Nearestinteger)

[26 Aug 2021 Shift 2]

The equilibrium constant Kc at 298K for the reaction A+B⇌C+D is 100 . Starting with an equimolar solution with concentrations of A, B, C and D all equal to 1M, the equilibrium concentration of D is ...........×10−2M. (Nearestinteger)

[26 Aug 2021 Shift 2]

Question 93/223

4 / -1

Mark Review

When 5.1g of solid NH4‌HS is introduced into a two litre evacuated flask at 27°C,20% of the solid decomposes into gaseous ammonia and hydrogen sulphide. The Kp for the reaction at 27°C is x×10−2. The value of x is ........... (Integer answer)
[Given, R=0.082L‌atm‌K−1‌mol−1]

[27 Aug 2021 Shift 2]

When 5.1g of solid NH4‌HS is introduced into a two litre evacuated flask at 27°C,20% of the solid decomposes into gaseous ammonia and hydrogen sulphide. The Kp for the reaction at 27°C is x×10−2. The value of x is ........... (Integer answer)
[Given, R=0.082L‌atm‌K−1‌mol−1]

[27 Aug 2021 Shift 2]

Question 94/223

4 / -1

Mark Review

The molar solubility of Zn(OH)2 in 0.1M NaOH solution is x×10−18M. The value of x is ......... (Nearest integer)
(Given; The solubility product of Zn(OH)2 is 2×10−20 ).

[1 Sep 2021 Shift 2]

The molar solubility of Zn(OH)2 in 0.1M NaOH solution is x×10−18M. The value of x is ......... (Nearest integer)
(Given; The solubility product of Zn(OH)2 is 2×10−20 ).

[1 Sep 2021 Shift 2]

Question 95/223

4 / -1

Mark Review

In the figure shown below reactant A (represented by square) is in equilibrium with product B (represented by circle). The equilibrium constant is:

[Jan. 09, 2020 (II)]

In the figure shown below reactant A (represented by square) is in equilibrium with product B (represented by circle). The equilibrium constant is:

[Jan. 09, 2020 (II)]

A

4

B

8

C

1

D

2

2 Question 96/223

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Mark Review

For the following Assertion and Reason, the correct option is:

Assertion: The pH of water increases with increase in temperature.

Reason: The dissociation of water into H+ and OH− is an exothermic reaction.
[Jan.08,2020(II)]

For the following Assertion and Reason, the correct option is:

Assertion: The pH of water increases with increase in temperature.

Reason: The dissociation of water into H+ and OH− is an exothermic reaction.
[Jan.08,2020(II)]

A

Both assertion and reason are true, and the reason is the correct explanation for the assertion.

B

Both assertion and reason are false.

C

Both assertion and reason are true, but the reason is not the correct explanation for the assertion.

D

Assertion is not true, but reason is true.

Question 97/223

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Mark Review

Two solutions, A and B, each of 100L was made by dissolving 4g of NaOH and 9.8g of H2SO4 in water, respectively. The pH of the resultant solution obtained from mixing 40L of solution A and 10L of solution. B is ________.

[NV, Jan. 07, 2020 (I)]

Two solutions, A and B, each of 100L was made by dissolving 4g of NaOH and 9.8g of H2SO4 in water, respectively. The pH of the resultant solution obtained from mixing 40L of solution A and 10L of solution. B is ________.

[NV, Jan. 07, 2020 (I)]

Question 98/223

4 / -1

Mark Review

3g of acetic acid is added to 250mL of 0.1MHCl and the solution made up to 500mL. To 20mL of this solution ‌

1

2

mL of 5MNaOH is added. The pH of the solution is _________.

[Given: pKa of acetic acid =4.75, molar mass of acetic acid=60g∕mol,log‌3=0.4771]

Neglect any changes in volume.
[NV, Jan. 07, 2020 (II)]

3g of acetic acid is added to 250mL of 0.1MHCl and the solution made up to 500mL. To 20mL of this solution

1

2

mL of 5MNaOH is added. The pH of the solution is _________.

[Given: pKa of acetic acid =4.75, molar mass of acetic acid=60g∕mol,log3=0.4771]

Neglect any changes in volume.
[NV, Jan. 07, 2020 (II)]

Question 99/223

4 / -1

Mark Review

The Ksp for the following dissociation is 1.6×10−5 PbCl2(s)⇌Pb2+(aq)+2Cl−(aq) Which of the following choices is correct for a mixture of
300‌mL‌0.134‌M‌Pb(NO3)2‌ and ‌100‌mL‌0.4‌MNaCl?

[Jan. 09, 2020 (I)]

The Ksp for the following dissociation is 1.6×10−5 PbCl2(s)⇌Pb2+(aq)+2Cl−(aq) Which of the following choices is correct for a mixture of
300‌mL‌0.134‌M‌Pb(NO3)2‌ and ‌100‌mL‌0.4‌MNaCl?

[Jan. 09, 2020 (I)]

A

Not enough data provided

B

Q<Ks

C

Q>Ksp

D

Q=Ksp

Question 100/223

4 / -1

Mark Review

The solubility product of Cr(OH)3 at 298K is 6.0×10−31.
The concentration of hydroxide ions in a saturated solution of Cr(OH)3 will be:

[Jan. 09,2020 (II)]

The solubility product of Cr(OH)3 at 298K is 6.0×10−31.
The concentration of hydroxide ions in a saturated solution of Cr(OH)3 will be:

[Jan. 09,2020 (II)]

A

(2.22×10−31)1∕4

B

(18×10−31)1∕4

C

(18×10−31)1∕2

D

(4.86×10−29)1∕4

Question 101/223

4 / -1

Mark Review

The stoichiometry and solubility product of a salt with the solubility curve given below is, respectively:

[Jan. 08,2020 (I)]

The stoichiometry and solubility product of a salt with the solubility curve given below is, respectively:

[Jan. 08,2020 (I)]

A

X2Y,2×10−9M3

B

XY2,4×10−9M3

C

XY2,1×10−9M3

D

XY,2×10−6M3

Question 102/223

4 / -1

Mark Review

For the reaction
Fe2N(s)+‌

3

2

H2(g)⇌2Fe(s)+NH3(g)

[Sep. 06,2020(I)]

For the reaction
Fe2N(s)+

3

2

H2(g)⇌2Fe(s)+NH3(g)

[Sep. 06,2020(I)]

A

Kc=Kp(RT)

B

Kc=Kp(RT)‌
−1
2

C

Kc=Kp(RT)‌
1
2

D

Kc=Kp(RT)‌
3
2

Question 103/223

4 / -1

Mark Review

The value of Kc is 64 at 800K for the reaction N2(g)+3H2(g)⇌2NH3(g).
The value of Kc for the following reaction is:
NH3(g)⇌‌

1

2

N2(g)+‌

3

2

H2(g)

[Sep. 06, 2020 (II)]

The value of Kc is 64 at 800K for the reaction N2(g)+3H2(g)⇌2NH3(g).
The value of Kc for the following reaction is:
NH3(g)⇌

1

2

N2(g)+

3

2

H2(g)

[Sep. 06, 2020 (II)]

A

1∕64

B

8

C

1∕4

D

1∕8

Question 104/223

4 / -1

Mark Review

For a reaction X+Y⇌2Z,1.0mol of X,1.5mol of Y and 0.5 mol of Z were taken in a 1 L vessel and allowed to react. At equilibrium, the concentration of Z was 1.0molL−1.
The equilibrium constant of the reaction is ‌

x

15

. The value of x is __________.

[NV, Sep. 05, 2020 (II)]

For a reaction X+Y⇌2Z,1.0mol of X,1.5mol of Y and 0.5 mol of Z were taken in a 1 L vessel and allowed to react. At equilibrium, the concentration of Z was 1.0molL−1.
The equilibrium constant of the reaction is ‌

x

15

. The value of x is __________.

[NV, Sep. 05, 2020 (II)]

Question 105/223

4 / -1

Mark Review

For the equilibrium A⇌B, the variation of the rate of the forward (a) and reverse (b) reaction with time is given by:

[Sep. 04,2020(I)]

For the equilibrium A⇌B, the variation of the rate of the forward (a) and reverse (b) reaction with time is given by:

[Sep. 04,2020(I)]

A

B

C

D

Question 106/223

4 / -1

Mark Review

If the equilibrium constant for A⇌B+C is Keq(1) and that of B+C⇌P is Keq(2), the equilibrium constant for A⇌P is:

[Sep. 04,2020(II)]

If the equilibrium constant for A⇌B+C is Keq(1) and that of B+C⇌P is Keq(2), the equilibrium constant for A⇌P is:

[Sep. 04,2020(II)]

A

Keq(1)∕Keq(2)

B

Keq(2)−Keq(t)

C

Keq(1)+Keq(2)

D

K‌eq ‌(1)K‌eq ‌(2)

Question 107/223

4 / -1

Mark Review

The variation of equilibrium constant with temperature is given below:

Temperature Equilibrium Constant

T1=25∘C‌‌K1=10
T2=100‌∘C‌‌K2=100
The values of ∆H∘,∆G∘ at T1 and ∆G∘ at T2 (in kj mol−1 ) respectively, are close to
[ use R=8.314JK−1mol−1]

[Sep. 06, 2020 (I)]

The variation of equilibrium constant with temperature is given below:

Temperature Equilibrium Constant

T1=25∘C‌‌K1=10
T2=100‌∘C‌‌K2=100
The values of ∆H∘,∆G∘ at T1 and ∆G∘ at T2 (in kj mol−1 ) respectively, are close to
[ use R=8.314JK−1mol−1]

[Sep. 06, 2020 (I)]

A

28.4,−7.14 and −5.71

B

0.64,−7.14 and −5.71

C

28.4,−5.71 and −14.29

D

0.64,−5.71 and −14.29

Question 108/223

4 / -1

Mark Review

Consider the following reaction:

N2O4(g)⇌2NO2(g);∆H0=+58kJ

For each of the following cases ((i), (ii)), the direction in which the equilibrium shifts is:
(i) Temperature is decreases
(ii) Pressure is increased by adding N2 at constant T.
[Sep .05,2020(I)]

Consider the following reaction:

N2O4(g)⇌2NO2(g);∆H0=+58kJ

For each of the following cases ((i), (ii)), the direction in which the equilibrium shifts is:
(i) Temperature is decreases
(ii) Pressure is increased by adding N2 at constant T.
[Sep .05,2020(I)]

A

(i) towards product, (ii) towards product

B

(i) towards reactant, (ii) towards product

C

(i) towards reactant, (ii) no change

D

(i) towards product, (ii) no change

Question 109/223

4 / -1

Mark Review

Arrange the following solutions in the decreasing order of pOH:

(A) 0.01MHCl

(B) 0.01MNaOH
(C) 0.01MCH3COONa
(D) 0.01MNaCl
[Sep. 06, 2020 (I)]

Arrange the following solutions in the decreasing order of pOH:

(A) 0.01MHCl

(B) 0.01MNaOH
(C) 0.01MCH3COONa
(D) 0.01MNaCl
[Sep. 06, 2020 (I)]

A

(A)>(C)>(D)>(B)

B

(A)>(D)>(C)>(B)

C

(B)>(C)>(D)>(A)

D

(B)>(D)>(C)>(A)

Question 110/223

4 / -1

Mark Review

A soft drink was bottled with a partial pressure of CO2 of 3 bar over the liquid at room temperature. The partial pressure of CO2 over the solution approaches a value of 30 bar when 44g of CO2 is dissolved in 1kg of water at room temperature. The approximate pH of the soft drink is ______ ×10−1.
(First dissociation constant of H2CO3=4.0×10−7;log‌2= 0.3; density of the soft drink =1gmL−1 )

[NV, Sep. 05, 2020(I)]

A soft drink was bottled with a partial pressure of CO2 of 3 bar over the liquid at room temperature. The partial pressure of CO2 over the solution approaches a value of 30 bar when 44g of CO2 is dissolved in 1kg of water at room temperature. The approximate pH of the soft drink is ______ ×10−1.
(First dissociation constant of H2CO3=4.0×10−7;log‌2= 0.3; density of the soft drink =1gmL−1 )

[NV, Sep. 05, 2020(I)]

Question 111/223

4 / -1

Mark Review

100mL of 0.1MHCl is taken in a beaker and to it 100mL of 0.1MNaOH is added in steps of 2mL and the pH is continuously measured. Which of the following graphs correctly depicts the change in pH?

[Sep. 03, 2020 (II)]

100mL of 0.1MHCl is taken in a beaker and to it 100mL of 0.1MNaOH is added in steps of 2mL and the pH is continuously measured. Which of the following graphs correctly depicts the change in pH?

[Sep. 03, 2020 (II)]

A

B

C

D

Question 112/223

4 / -1

Mark Review

If the solubility product of AB2 is 3.20×10−11M3, then the solubility of AB2 in pure water is _______×10−4molL−1.
[Assuming that neither kind of ion reacts with water]

[NV, Sep.06, 2020 (II)]

If the solubility product of AB2 is 3.20×10−11M3, then the solubility of AB2 in pure water is _______×10−4molL−1.
[Assuming that neither kind of ion reacts with water]

[NV, Sep.06, 2020 (II)]

Question 113/223

4 / -1

Mark Review

An acidic buffer is obtained on mixing :

[Sep. 03,2020 (I)]

An acidic buffer is obtained on mixing :

[Sep. 03,2020 (I)]

A

100mL of 0.1MCH3COOH and 100mL of 0.1MNaOH

B

100mL of 0.1MHCl and 200mL of 0.1MNaCl

C

100mL of 0.1MCH3COOHand200mL of 0.1MNaOH

D

100mL of 0.1MHCl and 200mL of 0.1MCH3COONa

Question 114/223

4 / -1

Mark Review

For the following Assertion and Reason, the correct option is

Assertion (A): When Cu (II) and sulphide ions are mixed, they react together extremely quickly to give a solid.

Reason (R): The equilibrium constant of Cu2+(aq)+S2− (aq) ⇌CuS(s) is high because the solubility product is low.
[Sep. 02,2020(I)]

For the following Assertion and Reason, the correct option is

Assertion (A): When Cu (II) and sulphide ions are mixed, they react together extremely quickly to give a solid.

Reason (R): The equilibrium constant of Cu2+(aq)+S2− (aq) ⇌CuS(s) is high because the solubility product is low.
[Sep. 02,2020(I)]

A

(A) is false and (R) is true

B

Both (A) and (R) are false

C

Both (A) and (R) are true but (R) is not the explanation for (A)

D

Both (A) and (R) are true and (R) is the explanation for (A)

Question 115/223

4 / -1

Mark Review

For the equilibrium
2H2O⇌H3O++OH−; the value of ∆G∘ at 298K is approximately:

[Jan. 11, 2019 (II)]

For the equilibrium
2H2O⇌H3O++OH−; the value of ∆G∘ at 298K is approximately:

[Jan. 11, 2019 (II)]

A

100kJmol−1

B

−80kJmol−1

C

80kJmol−1

D

−100kJmol−1

Question 116/223

4 / -1

Mark Review

Which amongst the following is the strongest acid?

[Jan. 9,2019 (I)]

Which amongst the following is the strongest acid?

[Jan. 9,2019 (I)]

A

CHBr3

B

CHI3

C

CH(CN)3

D

CHCl3

Question 117/223

4 / -1

Mark Review

If K50 of Ag2CO3 is 8×10−12, the molar solubility of Ag2CO3 in 0.1MAgNO3 is:

[Jan. 12,2019(II)]

If K50 of Ag2CO3 is 8×10−12, the molar solubility of Ag2CO3 in 0.1MAgNO3 is:

[Jan. 12,2019(II)]

A

8×10−12M

B

8×10−11M

C

8×10−10M

D

8×10−13M

Question 118/223

4 / -1

Mark Review

20mL of 0.1MH2SO4 solution is added to 30mL of 0.2 MNH4OH solution. The pH of the resultant mixture is:
[pKb of NH4OH=4.7]

[Jan. 9,2019 (I)]

20mL of 0.1MH2SO4 solution is added to 30mL of 0.2 MNH4OH solution. The pH of the resultant mixture is:
[pKb of NH4OH=4.7]

[Jan. 9,2019 (I)]

A

5.2

B

9.0

C

5.0

D

9.4

9.4 Question 119/223

4 / -1

Mark Review

A mixture of 100m mol of Ca(OH)2 and 2g of sodium sulphate was dissolved in water and the volume was made up to 100mL. The mass of calcium sulphate formed and the concentration of OH− in resulting solution, respectively, are: (Molar mass of Ca(OH)2,Na2SO4 and CaSO4 are 74,143 and 136gmol−1, respectively; Ksp of Ca(OH)2 is 5.5×10−6)

[Jan. 10,2019(I)]

A mixture of 100m mol of Ca(OH)2 and 2g of sodium sulphate was dissolved in water and the volume was made up to 100mL. The mass of calcium sulphate formed and the concentration of OH− in resulting solution, respectively, are: (Molar mass of Ca(OH)2,Na2SO4 and CaSO4 are 74,143 and 136gmol−1, respectively; Ksp of Ca(OH)2 is 5.5×10−6)

[Jan. 10,2019(I)]

A

1.9g,0.28molL−1

B

13.6g,0.28molL−1

C

1.9g,0.14molL−1

D

13.6g,0.14molL−1

Question 120/223

4 / -1

Mark Review

Two solids dissociate as follows
A(s)→B(g)+C(g);KP1=xatm2
D(s)→C(g)+E(g);KP2=yatm2
The total pressure when both the solids dissociate simultaneously is:

[Jan. 12, 2019 (I)]

Two solids dissociate as follows
A(s)→B(g)+C(g);KP1=xatm2
D(s)→C(g)+E(g);KP2=yatm2
The total pressure when both the solids dissociate simultaneously is:

[Jan. 12, 2019 (I)]

A

√x+y atm

B

2(√x+y) atm

C

(x+y)atm

D

x2+y2 atm

Question 121/223

4 / -1

Mark Review

In a chemical reaction, A+2B

K

⇌

2C+D, the initial concentration of B was 1.5 times of the concentration of A, but the equilibrium concentrations of A and B were found to be equal. The equilibrium constant (K) for the aforesaid chemical reaction is:

[Jan. 12, 2019 (I)]

In a chemical reaction, A+2B

K

⇌

2C+D, the initial concentration of B was 1.5 times of the concentration of A, but the equilibrium concentrations of A and B were found to be equal. The equilibrium constant (K) for the aforesaid chemical reaction is:

[Jan. 12, 2019 (I)]

A

4

B

16

C

‌
1
4

D

1

1 Question 122/223

4 / -1

Mark Review

Consider the reaction
N2(g)+3H2(g)⇌2NH3(g)
The equilibrium constant of the above reaction is Kp.If pure ammonia is left to dissociate, the partial pressure of ammonia at equilibrium is given by (Assume that PNH3<<P‌total ‌ at equilibrium)

[Jan. 11, 2019 (I)]

Consider the reaction
N2(g)+3H2(g)⇌2NH3(g)
The equilibrium constant of the above reaction is Kp.If pure ammonia is left to dissociate, the partial pressure of ammonia at equilibrium is given by (Assume that PNH3<<P‌total ‌ at equilibrium)

[Jan. 11, 2019 (I)]

A

‌
33∕2KP1∕2P2
16

B

‌
KP1∕2P2
16

C

‌
KP1∕2P2
4

D

‌
33∕2KP1∕2P2
4

Question 123/223

4 / -1

Mark Review

The values of Kp∕Kc for the following reactions at 300K are, respectively: ( At 300K,RT=24.62dm3‌atm‌mol−1)
N2(g)+O2(g)⇌2NO(g)
N2O4(g)⇌2NO2(g)
N2(g)+3H2(g)⇌2NH3(g)
[Jan. 10, 2019 (I)]

The values of Kp∕Kc for the following reactions at 300K are, respectively: ( At 300K,RT=24.62dm3atmmol−1)
N2(g)+O2(g)⇌2NO(g)
N2O4(g)⇌2NO2(g)
N2(g)+3H2(g)⇌2NH3(g)
[Jan. 10, 2019 (I)]

A

1,24.62dm3‌atm‌mol−1,
606.0dm6atm2mol−2

B

1,24.62dm3‌atm‌mol−1,
1.65×10−3dm−6atm−2mol2

C

1,4.1×10−2dm−3atm−1‌mol,
606dm6atm2mol2

D

24.62dm3‌atm‌mol−1,
606.0dm6atm2mol−2
1.65×10−3dm−6atm−2mol2

Question 124/223

4 / -1

Mark Review

5.1 gNH4SH is introduced in 3.0L evacuated flask at 327∘C, 30% of the solid NH4SH decomposed to NH3 and H2S as gases. The Kp of the reaction at 327∘C is (R=0.082L atm mol−1K−1, molar mass of S=32gmol−1, molar mass of N=
14gmol−1)

[Jan. 10, 2019 (II)]

5.1 gNH4SH is introduced in 3.0L evacuated flask at 327∘C, 30% of the solid NH4SH decomposed to NH3 and H2S as gases. The Kp of the reaction at 327∘C is (R=0.082L atm mol−1K−1, molar mass of S=32gmol−1, molar mass of N=
14gmol−1)

[Jan. 10, 2019 (II)]

A

0.242×10−4atm2

B

1×10−4atm2

C

4.9×10−3atm2

D

0.242atm2

Question 125/223

4 / -1

Mark Review

Consider the following reversible chemical reactions:
A2(g)+B2(g)

K1

⟵

2AB(g)......(1)
6AB(g)

K2

⇌

3A2(g)+3B2(g).....(2)
The relation between K1 and K2 is:

[Jan. 9,2019(II)]

Consider the following reversible chemical reactions:
A2(g)+B2(g)

K1

⟵

2AB(g)......(1)
6AB(g)

K2

⇌

3A2(g)+3B2(g).....(2)
The relation between K1 and K2 is:

[Jan. 9,2019(II)]

A

K1K2=‌
1
3

B

K2=K13

C

K2=K1−3

D

K1K2=3

Question 126/223

4 / -1

Mark Review

The INCORRECT match in the following is:

[April 12, 2019 (II)]

The INCORRECT match in the following is:

[April 12, 2019 (II)]

A

∆G0<0,K>1

B

∆G0=0,K=1

C

∆G0>0,K<1

D

∆G0<0,K<1

Question 127/223

4 / -1

Mark Review

In which one of the following equilibria, Kp≠Kc ?

[April 12, 2019 (II)]

In which one of the following equilibria, Kp≠Kc ?

[April 12, 2019 (II)]

A

2C(s)+O2(g)⇌2CO(g)

B

2HI(g)⇌H2(g)+I2(g)

C

NO2(g)+SO2(g)⇌NO(g)+SO3(g)

D

2NO(g)⇌N2(g)+O2(g)

Question 128/223

4 / -1

Mark Review

For the following reactions, equilibrium constants are given:
S(s)+O2(g)⇌SO2(g);K1=1052
2S(s)+3O2(g)⇌2SO3(g);K2=10129
The equilibrium constant for the reaction,
2SO2(g)+O2(g)⇌2SO3(g) is:

[April 8, 2019 (II)]

For the following reactions, equilibrium constants are given:
S(s)+O2(g)⇌SO2(g);K1=1052
2S(s)+3O2(g)⇌2SO3(g);K2=10129
The equilibrium constant for the reaction,
2SO2(g)+O2(g)⇌2SO3(g) is:

[April 8, 2019 (II)]

A

10154

B

10181

C

1025

D

1077

Question 129/223

4 / -1

Mark Review

For the reaction,
2SO2(g)+O2(g)⇌2SO3(g)
∆H=−57.2kJmol−1 and Kc=1.7×1016
Which of the following statement is INCORRECT?

[April 10, 2019 (II)]

For the reaction,
2SO2(g)+O2(g)⇌2SO3(g)
∆H=−57.2kJmol−1 and Kc=1.7×1016
Which of the following statement is INCORRECT?

[April 10, 2019 (II)]

A

The equilibrium constant is large suggestive of reaction going to completion and so no catalyst is required.

B

The equilibrium will shift in forward direction as the pressure increases.

C

The equilibrium constant decreases as the temperature increases.

D

The addition of inert gas at constant volume will not affect the equilibrium constant.

Question 130/223

4 / -1

Mark Review

Consider the following statements

(a) The pH of a mixture containing 400mL of 0.1MH2SO4 and 400mL of 0.1MNaOH will be approximately 1.3.

(b) Ionic product of water is temperature dependent.
(c) A monobasic acid with Ka−10−5 has a pH=5. The degree of dissociation of this acid is 50%.
(d) The Le Chatelier's principle is not applicable to common-ion effect.
The correct statements are :
[April 10, 2019 (I)]

Consider the following statements

(a) The pH of a mixture containing 400mL of 0.1MH2SO4 and 400mL of 0.1MNaOH will be approximately 1.3.

(b) Ionic product of water is temperature dependent.
(c) A monobasic acid with Ka−10−5 has a pH=5. The degree of dissociation of this acid is 50%.
(d) The Le Chatelier's principle is not applicable to common-ion effect.
The correct statements are :
[April 10, 2019 (I)]

A

(a), (b), and (d)

B

(a), (b) and (c)

C

(b) and (c)

D

(a) and (b)

Question 131/223

4 / -1

Mark Review

In an acid base titration, 0.1MHCl solution was added to the NaOH solution of unknown strength. Which of the following correctly shows the change of pH of the titration mixture in this experiment?

[April 9,2019 (II)]

In an acid base titration, 0.1MHCl solution was added to the NaOH solution of unknown strength. Which of the following correctly shows the change of pH of the titration mixture in this experiment?

[April 9,2019 (II)]

A

(B)

B

(A)

C

(C)

D

(D)

Question 132/223

4 / -1

Mark Review

What is the molar solubility of Al(OH)3 in 0.2MNaOH solution ?
Given that, solubility product of Al(OH)3 =2.4×10−24:

[April 12, 2019 (I)]

What is the molar solubility of Al(OH)3 in 0.2MNaOH solution ?
Given that, solubility product of Al(OH)3 =2.4×10−24:

[April 12, 2019 (I)]

A

3×10−19

B

12×10−21

C

3×10−22

D

12×10−23

Question 133/223

4 / -1

Mark Review

The molar solubility of Cd(OH)2 is 1.84×10−5M in water. The expected solubility of Cd(OH)2 in a buffer solution pH=12 is:

[April 12, 2019 (II)]

The molar solubility of Cd(OH)2 is 1.84×10−5M in water. The expected solubility of Cd(OH)2 in a buffer solution pH=12 is:

[April 12, 2019 (II)]

A

1.84×10−9M

B

‌
2.49
1.84
×10−9M

C

6.23×10−11M

D

2.49×10−10M

Question 134/223

4 / -1

Mark Review

The pH of a 0.02MNH4Cl solution will be [given Kb(NH4OH)=10−5 and log‌2=0.301]

[April 10, 2019 (II)]

The pH of a 0.02MNH4Cl solution will be [given Kb(NH4OH)=10−5 and log‌2=0.301]

[April 10, 2019 (II)]

A

2.65

B

4.35

C

4.65

D

5.35

5.35 Question 135/223

4 / -1

Mark Review

If solubility product of Zr3(PO4)4 is denoted by Ksp and its molar solubility is denoted by S, then which of the following relation between S and Ksp is correct?

[April 8, 2019 (I)]

If solubility product of Zr3(PO4)4 is denoted by Ksp and its molar solubility is denoted by S, then which of the following relation between S and Ksp is correct?

[April 8, 2019 (I)]

A

S=(‌
Kgp
144
)1∕6

B

S=(‌
Ksp
6912
)1∕7

C

S=(‌
Kϕ
929
)1∕9

D

S=(‌
Ksp
216
)1∕7

Question 136/223

4 / -1

Mark Review

At a certain temperature in a 5L vessel, 2 moles of carbon monoxide and 3 moles of chlorine were allowed to reach equilibrium according to the reaction, CO+Cl2⇌COCl2 At equilibrium, if one mole of CO is present then equilibrium constant (Kc) for the reaction is:

[Online April 15, 2018 (II)]

At a certain temperature in a 5L vessel, 2 moles of carbon monoxide and 3 moles of chlorine were allowed to reach equilibrium according to the reaction, CO+Cl2⇌COCl2 At equilibrium, if one mole of CO is present then equilibrium constant (Kc) for the reaction is:

[Online April 15, 2018 (II)]

A

2.5

B

4

C

2

D

3

3 Question 137/223

4 / -1

Mark Review

In which of the following reactions, an increase in the volume of the container will favour the formation of products?

[Online April 15,2018(I)]

In which of the following reactions, an increase in the volume of the container will favour the formation of products?

[Online April 15,2018(I)]

A

4NH3(g)+5O2(g)⇌4NO(g)+6H2O(l)

B

2NO2(g)⇌2NO(g)+O2(g)

C

3O2⇌2O3(g)

D

H2(g)+I2(g)⇌2HI(g)

Question 138/223

4 / -1

Mark Review

The gas phase reaction 2NO2(g)⟶N2O4(g) is an exothermic reaction. The decomposition of N2O4, in equilibrium mixutre of NO2(g) and N2O4(g), can be increased by:

[Online April 16, 2018]

The gas phase reaction 2NO2(g)⟶N2O4(g) is an exothermic reaction. The decomposition of N2O4, in equilibrium mixutre of NO2(g) and N2O4(g), can be increased by:

[Online April 16, 2018]

A

addition of an inert gas at constant pressure

B

lowering the temperature

C

increasing the pressure

D

addition of an inert gas at constant volume

Question 139/223

4 / -1

Mark Review

Following four solutions are prepared by mixing different volumes of NaOH and HCl of different concentrations, pH of which one of them will be equal to 1 ?

[Online April 15, 2018 (II)]

Following four solutions are prepared by mixing different volumes of NaOH and HCl of different concentrations, pH of which one of them will be equal to 1 ?

[Online April 15, 2018 (II)]

A

55mL‌
M
10
HCl+45mL‌
M
10
NaOH

B

75mL‌
M
5
HCl+25mL‌
M
5
NaOH

C

100mL‌
M
10
HCl+100mL‌
M
10
NaOH

D

60mL‌
M
10
HCl+40mL‌
M
10
NaOH

Question 140/223

4 / -1

Mark Review

Which of the following is a Lewis acid?

[Online April 15, 2018 (I)]

Which of the following is a Lewis acid?

[Online April 15, 2018 (I)]

A

PH3

B

NF3

C

NaH

D

B(CH3)3

Question 141/223

4 / -1

Mark Review

Which of the following salts is the most basic in aqueous solution?

[2018]

Which of the following salts is the most basic in aqueous solution?

[2018]

A

Al(CN)3

B

CH3COOK

C

FeCl3

D

Pb(CH3COO)2

Question 142/223

4 / -1

Mark Review

An aqueous solution contains 0.10MH2S and 0.20M HCl. If the equilibrium constants for the formation of HS from H2S is 1.0×10−7 and that of S2− from HS -ions is 1.2 ×10−13 then the concentration of S2− ions in aqueous solution is :

[2018]

An aqueous solution contains 0.10MH2S and 0.20M HCl. If the equilibrium constants for the formation of HS from H2S is 1.0×10−7 and that of S2− from HS -ions is 1.2 ×10−13 then the concentration of S2− ions in aqueous solution is :

[2018]

A

5×108

B

3×10−20

C

6×10−21

D

5×10−19

Question 143/223

4 / -1

Mark Review

An aqueous solution contains an unknown concentration of Ba2+. When 50mL of a 1M solution of Na2SO4 is added, BaSO4 just begins to precipitate. The final volume is 500 mL. The solubility product of BaSO4 is 1×10−10. What is the original concentration of Ba2+?

[2018]

An aqueous solution contains an unknown concentration of Ba2+. When 50mL of a 1M solution of Na2SO4 is added, BaSO4 just begins to precipitate. The final volume is 500 mL. The solubility product of BaSO4 is 1×10−10. What is the original concentration of Ba2+?

[2018]

A

5×10−9M

B

2×10−9M

C

1.1×10−9M

D

1.0×10−10M

Question 144/223

4 / -1

Mark Review

The minimum volume of water required to dissolve 0.1g lead (II) chloride to get a saturated solution (KsP of PbCl2= 3.2×10−8; atomic mass of Pb=207u ) is:

[Online April 15, 2018 (I)]

The minimum volume of water required to dissolve 0.1g lead (II) chloride to get a saturated solution (KsP of PbCl2= 3.2×10−8; atomic mass of Pb=207u ) is:

[Online April 15, 2018 (I)]

A

1.798L

B

0.36L

C

17.95L

D

0.18L

Question 145/223

4 / -1

Mark Review

The following reaction occurs in the Blast Furnace where iron ore is reduced to iron metal :

Fe2O3(s)+3CO(g)⇌2Fe(l)+3CO2(g)

Using the Le Chatelier's principle, predict which one of the following will not disturb the equilibrium?
[Online April 9, 2017]

The following reaction occurs in the Blast Furnace where iron ore is reduced to iron metal :

Fe2O3(s)+3CO(g)⇌2Fe(l)+3CO2(g)

Using the Le Chatelier's principle, predict which one of the following will not disturb the equilibrium?
[Online April 9, 2017]

A

Removal of CO

B

Removal of CO2

C

Addition of CO2

D

Addition of Fe2O3

Question 146/223

4 / -1

Mark Review

50mL of 0.2M ammonia solution is treated with 25mL of 0.2MHCl. If pKb of ammonia solution is 4.75, the pH of the mixture will be:

[Online April 9, 2017]

50mL of 0.2M ammonia solution is treated with 25mL of 0.2MHCl. If pKb of ammonia solution is 4.75, the pH of the mixture will be:

[Online April 9, 2017]

A

3.75

B

4.75

C

8.25

D

9.25

9.25 Question 147/223

4 / -1

Mark Review

pKa of a weak acid (HA) and pKb of a weak base (BOH) are 3.2 and 3.4, respectively. The pH of their salt (AB) solution is

[2017]

pKa of a weak acid (HA) and pKb of a weak base (BOH) are 3.2 and 3.4, respectively. The pH of their salt (AB) solution is

[2017]

A

7.2

B

6.9

C

7.0

D

1.0

1.0 Question 148/223

4 / -1

Mark Review

Addition of sodium hydroxide solution to a weak acid (HA) results in a buffer of pH. . If ionisation constant of HA is 10−5, the ratio of salt to acid concentration in the buffer solution will be:

[Online April 8, 2017]

Addition of sodium hydroxide solution to a weak acid (HA) results in a buffer of pH. . If ionisation constant of HA is 10−5, the ratio of salt to acid concentration in the buffer solution will be:

[Online April 8, 2017]

A

4:5

B

1:10

C

10:1

D

5:4

Question 149/223

4 / -1

Mark Review

The equilibrium constant at 298K for a reaction A+B⇌C+D is 100 . If the initial concentration of all the four species were 1 M each, then equilibrium concentration of D (in mol L−1 ) will be:

[2016]

The equilibrium constant at 298K for a reaction A+B⇌C+D is 100 . If the initial concentration of all the four species were 1 M each, then equilibrium concentration of D (in mol L−1 ) will be:

[2016]

A

1.818

B

1.182

C

0.182

D

0.818

0.818 Question 150/223

4 / -1

Mark Review

A solid XY kept in an evacuated sealed container undergoes decomposition to form a mixture of gases X and Y at temperature T. The equilibrium pressure is 10 bar in the vessel. Kp for this reaction is:

[Online April 10,2016]

A solid XY kept in an evacuated sealed container undergoes decomposition to form a mixture of gases X and Y at temperature T. The equilibrium pressure is 10 bar in the vessel. Kp for this reaction is:

[Online April 10,2016]

A

25

B

100

C

10

D

5

5 Question 151/223

4 / -1

Mark Review

The plot shows the variation of −ln‌Kp versus temperature for the two reactions.
M(s)+‌

1

2

O2(g)→MO(s) and
C(s)+‌

1

2

O2(g)→CO(s)

Identify the correct statement:
[Online April 9,2016]

The plot shows the variation of −lnKp versus temperature for the two reactions.
M(s)+

1

2

O2(g)→MO(s) and
C(s)+

1

2

O2(g)→CO(s)

Identify the correct statement:
[Online April 9,2016]

A

At T<1200K, oxidation of carbon is unfavourable.

B

Oxidation of carbon is favourable at all temperatures.

C

At T<1200K, the reaction MO(s)+C(s)→M(s)+CO(g) is spontaneous.

D

At T>1200K, carbon will reduce MO(s) to M(s).

Question 152/223

4 / -1

Mark Review

For the reaction,
A(g)+B(g)→C(g)+D(g),∆H∘ and ∆S∘ are, respectively,
−29.8kJmol−1 and −0.100kJK−1mol−1 at 298K.
The equilibrium constant for the reaction at 298K is :
[Online April 9, 2016]

A

1.0×10−10

B

10

C

1

D

1.0×1010

Question 153/223

4 / -1

Mark Review

Gaseous N2O4 dissociates into gaseous NO2 according to the reaction
[N2O4(g)⇌2NO2(g)]
At 300K and 1 atm pressure, the degree of dissociation of N2O4 is 0.2. If one mole of N2O4 gas is contained in a vessel, then the density of the equilibrium mixture is :

[Online April 10, 2015]

Gaseous N2O4 dissociates into gaseous NO2 according to the reaction
[N2O4(g)⇌2NO2(g)]
At 300K and 1 atm pressure, the degree of dissociation of N2O4 is 0.2. If one mole of N2O4 gas is contained in a vessel, then the density of the equilibrium mixture is :

[Online April 10, 2015]

A

1.56g∕L

B

6.22g∕L

C

3.11gL

D

4.56g∕L

Question 154/223

4 / -1

Mark Review

The standard Gibbs energy change at 300K for the reaction 2A⇌B+C is 2494.2J. At a given time, the composition of the reaction mixture is [A]=‌

1

2

,[B]=2 and [C]=‌

1

2

. The reaction proceeds in the : [R=8.314J∕K∕mol,e=2.718]

[2015]

The standard Gibbs energy change at 300K for the reaction 2A⇌B+C is 2494.2J. At a given time, the composition of the reaction mixture is [A]=‌

1

2

,[B]=2 and [C]=‌

1

2

. The reaction proceeds in the : [R=8.314J∕K∕mol,e=2.718]

[2015]

A

forward direction because Q<Kc

B

reverse direction because Q<Kc

C

forward direction because Q>Kc

D

reverse direction because Q>Kc

Question 155/223

4 / -1

Mark Review

The following reaction is performed at 298K.
2NO(g)+O2(g)⇌2NO2(g)
The standard free energy of formation of NO(g) is 86.6 KJ∕mol at 298K.
What is the standard free energy of formation of NO2(g) at 298K?(Kp=1.6×1012)
[2015]

A

86600−‌
ln(1.6×1012)
R(298)

B

0.5[2×86,600−R(298)‌ln(1.6×1012)]

C

R(298)‌ln(1.6×1012)−86600

D

86600+R(298)‌ln(1.6×1012)

Question 156/223

4 / -1

Mark Review

The increase of pressure on ice ⇌ water system at constant temperature will lead to

[Online April 11, 2015]

The increase of pressure on ice ⇌ water system at constant temperature will lead to

[Online April 11, 2015]

A

a decrease in the entropy of the system

B

an increase in the Gibb's energy of the system

C

no effect on the equilibrium

D

a shift of the equilibrium in the forward direction

Question 157/223

4 / -1

Mark Review

For the reaction SO2(g)+‌

1

2

O2(g)⇌SO3(g), if Kp=Kc(RT)x where the symbols have usual meaning then the value of x is (assuming ideality):

[2014]

For the reaction SO2(g)+‌

1

2

O2(g)⇌SO3(g), if Kp=Kc(RT)x where the symbols have usual meaning then the value of x is (assuming ideality):

[2014]

A

−1

B

−‌
1
2

C

‌
1
2

D

1

1 Question 158/223

4 / -1

Mark Review

At a certain temperature, only 50%HI is dissociated into H2 and I2 at equilibrium. The equilibrium constant is:

[Online April 9, 2014]

At a certain temperature, only 50%HI is dissociated into H2 and I2 at equilibrium. The equilibrium constant is:

[Online April 9, 2014]

A

1.0

B

3.0

C

0.5

D

0.25

0.25 Question 159/223

4 / -1

Mark Review

For the decomposition of the compound, represented as
NH2COONH4(s)⇌2NH3(g)+CO2(g) the Kp=2.9×10−5atm3.
If the reaction is started with 1mol of the compound, the total pressure at equilibrium would be:

[Online April 19, 2014]

For the decomposition of the compound, represented as
NH2COONH4(s)⇌2NH3(g)+CO2(g) the Kp=2.9×10−5atm3.
If the reaction is started with 1mol of the compound, the total pressure at equilibrium would be:

[Online April 19, 2014]

A

1.94×10−2 atm

B

5.82×10−2atm

C

7.66×10−2atm

D

38.8×10−2atm

Question 160/223

4 / -1

Mark Review

What happens when an inert gas is added to an equilibrium keeping volume unchanged?

[Online April 12, 2014]

What happens when an inert gas is added to an equilibrium keeping volume unchanged?

[Online April 12, 2014]

A

More product will form

B

Less product will form

C

More reactant will form

D

Equilibrium will remain unchanged

Question 161/223

4 / -1

Mark Review

The conjugate base of hydrazoic acid is:

[Online April 12, 2014]

The conjugate base of hydrazoic acid is:

[Online April 12, 2014]

A

N−3

B

N3−

C

N2−

D

HN3−

Question 162/223

4 / -1

Mark Review

Assuming that the degree of hydrolysis is small, the pH of 0.1M solution of sodium acetate (Ka=1.0×10−5) will be:

[Online April 11, 2014]

Assuming that the degree of hydrolysis is small, the pH of 0.1M solution of sodium acetate (Ka=1.0×10−5) will be:

[Online April 11, 2014]

A

5.0

B

6.0

C

8.0

D

9.0

9.0 Question 163/223

4 / -1

Mark Review

In some solutions, the concentration of H3O+ remains constant even when small amounts of strong acid or strong base are added to them. These solutions are known as:

[Online April 11, 2014]

In some solutions, the concentration of H3O+ remains constant even when small amounts of strong acid or strong base are added to them. These solutions are known as:

[Online April 11, 2014]

A

Ideal solutions

B

Colloidal solutions

C

True solutions

D

Buffer solutions

Question 164/223

4 / -1

Mark Review

Consider the following equilibrium
AgCl↓+2NH3⇌[Ag(NH3)2]++Cl−
White precipitate of AgCl appears on adding which of the following?

[Online April 11,2014]

Consider the following equilibrium
AgCl↓+2NH3⇌[Ag(NH3)2]++Cl−
White precipitate of AgCl appears on adding which of the following?

[Online April 11,2014]

A

NH3

B

aqueous NaCl

C

aqueous HNO3

D

aqueous NH4Cl

Question 165/223

4 / -1

Mark Review

Zirconium phosphate [Zr3(PO4)4] dissociates into three zirconium cations of charge +4 and four phosphate anions of charge −3. If molar solubility of zirconium phosphate is denoted by S and its solubility product by Ksp then which of the following relationship between S and Ksp is correct?

[Online April 19,2014]

Zirconium phosphate [Zr3(PO4)4] dissociates into three zirconium cations of charge +4 and four phosphate anions of charge −3. If molar solubility of zirconium phosphate is denoted by S and its solubility product by Ksp then which of the following relationship between S and Ksp is correct?

[Online April 19,2014]

A

S={Ksp∕(6912)1∕7}

B

S={Ksp∕144}1∕7

C

S={Ksp∕6912}1∕7

D

S={K‌sp ‌∕6912}7

Question 166/223

4 / -1

Mark Review

In reaction A+2B⇌2C+D, initial concentration of B was 1.5 times of [A], but at equilibrium the concentrations of A and B became equal. The equilibrium constant for the reaction is :

[Online April 9, 2013]

In reaction A+2B⇌2C+D, initial concentration of B was 1.5 times of [A], but at equilibrium the concentrations of A and B became equal. The equilibrium constant for the reaction is :

[Online April 9, 2013]

A

8

B

4

C

12

D

6

6 Question 167/223

4 / -1

Mark Review

(1) N2(g)+3H2(g)⇌2NH3(g),K1
(2) N2(g)+O2(g)⇌2NO(g),K2
(3) H2(g)+‌

1

2

O2(g)⇌H2O(g),K3
The equation for the equilibrium constant of the reaction
2NH3(g)+‌

5

2

O2(g)⇌2NO(g)+3H2O(g),(K4) in ter of K1,K2 and K3 is :

[Online April 23, 2013]

(1) N2(g)+3H2(g)⇌2NH3(g),K1
(2) N2(g)+O2(g)⇌2NO(g),K2
(3) H2(g)+‌

1

2

O2(g)⇌H2O(g),K3
The equation for the equilibrium constant of the reaction
2NH3(g)+‌

5

2

O2(g)⇌2NO(g)+3H2O(g),(K4) in ter of K1,K2 and K3 is :

[Online April 23, 2013]

A

‌
K1⋅K2
K3

B

‌
K1⋅K32
K2

C

K1K2K3

D

‌
K2⋅K33
K1

Question 168/223

4 / -1

Mark Review

The ratio ‌

Kp

Kc

for the reaction is:

[Online April 25, 2013]

The ratio ‌

Kp

Kc

for the reaction is:

[Online April 25, 2013]

A

‌
1
√RT

B

(RT)1∕2

C

RT

D

1

1 Question 169/223

4 / -1

Mark Review

How many litres of water must be added to 1 litre an aqueous solution of HCl with a pH of 1 to create an aqueous solution with pH of 2 ?

[2013]

How many litres of water must be added to 1 litre an aqueous solution of HCl with a pH of 1 to create an aqueous solution with pH of 2 ?

[2013]

A

0.1L

B

0.9L

C

2.0L

D

9.0L

Question 170/223

4 / -1

Mark Review

NaOH is a strong base. What will be pH of 5.0×10−2MNaOH solution ? (log‌2=0.3)

[Online April 22, 2013]

NaOH is a strong base. What will be pH of 5.0×10−2MNaOH solution ? (log‌2=0.3)

[Online April 22, 2013]

A

14.00

B

13.70

C

13.00

D

12.70

12.70 Question 171/223

4 / -1

Mark Review

Equimolar solutions of the following compounds are prepared separately in water. Which will have the lowest pH value?

[Online April 23, 2013]

Equimolar solutions of the following compounds are prepared separately in water. Which will have the lowest pH value?

[Online April 23, 2013]

A

BeCl2

B

SrCl2

C

CaCl2

D

MgCl2

Question 172/223

4 / -1

Mark Review

What is the pH of a 10−4MOH− solution at 330K, if Kw at 330K is 10−13.6?

[Online April 23, 2013]

What is the pH of a 10−4MOH− solution at 330K, if Kw at 330K is 10−13.6?

[Online April 23, 2013]

A

4

B

9.0

C

10

D

9.6

9.6 Question 173/223

4 / -1

Mark Review

Which one of the following arrangements represents the correct order of the proton affinity of the given species:

[Online April 25, 2013]

Which one of the following arrangements represents the correct order of the proton affinity of the given species:

[Online April 25, 2013]

A

I−<F−<HS−<NH2−

B

HS−<NH2−<F−<I−

C

F−<I−<NH2−<HS

D

NH2−<HS−<I−<F−

Question 174/223

4 / -1

Mark Review

Values of dissociation constant, K0 are given as follows:

Correct order of increasing base strength of the base CN− F− and NO2− will be:

[Online April 22, 2013]

Values of dissociation constant, K0 are given as follows:

Correct order of increasing base strength of the base CN− F− and NO2− will be:

[Online April 22, 2013]

A

F<CN−<NO2−

B

NO2−<CN−<F−

C

F<NO2−<CN−

D

NO2−<F−<CN−

Question 175/223

4 / -1

Mark Review

What would be the pH of a solution obtained by mixing 5g of acetic acid and 7.5g of sodium acetate and making the volume equal to 500mL ? (Ka=1.75×10−5,pKa=4.76)

[Online April 25, 2013]

What would be the pH of a solution obtained by mixing 5g of acetic acid and 7.5g of sodium acetate and making the volume equal to 500mL ? (Ka=1.75×10−5,pKa=4.76)

[Online April 25, 2013]

A

pH=4.70

B

pH<4.70

C

pH of solution will be equal to pH of acetic acid

D

4.76<pH<5.0

Question 176/223

4 / -1

Mark Review

Solid Ba(NO3)2 is gradually dissolved in a 1.0×10−4MNa2CO3 solution. At which concentration of Ba2+, precipitate of BaCO3 begins to form ?(Ksp for BaCO3 =5.1×10−9)

[Online April 9, 2013]

Solid Ba(NO3)2 is gradually dissolved in a 1.0×10−4MNa2CO3 solution. At which concentration of Ba2+, precipitate of BaCO3 begins to form ?(Ksp for BaCO3 =5.1×10−9)

[Online April 9, 2013]

A

5.1×10−5M

B

7.1×10−8M

C

4.1×10−5M

D

8.1×10−7M

Question 177/223

4 / -1

Mark Review

Which one of the following arrangements represents the correct order of solubilities of sparingly soluble salts Hg2Cl2,Cr2(SO4)3,BaSO4 and CrCl3 respectively?

[Online April 22, 2013]

Which one of the following arrangements represents the correct order of solubilities of sparingly soluble salts Hg2Cl2,Cr2(SO4)3,BaSO4 and CrCl3 respectively?

[Online April 22, 2013]

A

BaSO4>Hg2Cl2>Cr2(SO4)3>CrCl3

B

BaSO4>Hg2Cl2>CrCl3>Cr2(SO4)3

C

BaSO4>CrCl3>Hg2Cl2>Cr2(SO4)3

D

Hg2Cl2>BaSO4>CrCl3>Cr2(SO4)3

Question 178/223

4 / -1

Mark Review

K1,K2 and K3 are the equilibrium constants of the following reactions (I), (II) and (III) respectively:

(I) N2+2O2⇌2NO2

(II) 2NO2⇌N2+2O2
(III) NO2⇌‌

1

2

N2+O2
The correct relation from the following is
[Online May 7, 2012]

K1,K2 and K3 are the equilibrium constants of the following reactions (I), (II) and (III) respectively:

(I) N2+2O2⇌2NO2

(II) 2NO2⇌N2+2O2
(III) NO2⇌

1

2

N2+O2
The correct relation from the following is
[Online May 7, 2012]

A

K1=‌
1
K2
=‌
1
K3

B

K1=‌
1
K2
=‌
1
(K3)2

C

K1=√K2=K3

D

K1=‌
1
K2
=K3

Question 179/223

4 / -1

Mark Review

8 mol of AB3(g) are introduced into a 1.0dm3 vessel. If it dissociates as 2AB3(g)⇌A2(g)+3B2(g). At equilibrium, 2 mol of A2 are found to be present. The equilibrium constant of this reaction is

[Online May 12, 2012]

8 mol of AB3(g) are introduced into a 1.0dm3 vessel. If it dissociates as 2AB3(g)⇌A2(g)+3B2(g). At equilibrium, 2 mol of A2 are found to be present. The equilibrium constant of this reaction is

[Online May 12, 2012]

A

2

B

3

C

27

D

36

36 Question 180/223

4 / -1

Mark Review

The value of Kp for the equilibrium reaction N2O4(g)⇌2NO2(g) is 2 .
The percentage dissociation of N2O4(g) at a pressure of 0.5 atm is

[Online May 19, 2012]

The value of Kp for the equilibrium reaction N2O4(g)⇌2NO2(g) is 2 .
The percentage dissociation of N2O4(g) at a pressure of 0.5 atm is

[Online May 19, 2012]

A

25

B

88

C

50

D

71

71 Question 181/223

4 / -1

Mark Review

One mole of O2(g) and two moles of SO2(g) were heated in a closed vessel of one-litre capacity at 1098K. At equilibrium 1.6 moles of SO3(g) were found. The equilibrium constant Kc of the reaction would be

[Online May 26, 2012]

One mole of O2(g) and two moles of SO2(g) were heated in a closed vessel of one-litre capacity at 1098K. At equilibrium 1.6 moles of SO3(g) were found. The equilibrium constant Kc of the reaction would be

[Online May 26, 2012]

A

30

B

40

C

80

D

60

60 Question 182/223

4 / -1

Mark Review

The pH of a 0.1 molar solution of the acid HQ is 3. The value of the ionization constant, Ka of the acid is :

[2012]

The pH of a 0.1 molar solution of the acid HQ is 3. The value of the ionization constant, Ka of the acid is :

[2012]

A

3×10−1

B

1×10−3

C

1×10−5

D

1×10−7

Question 183/223

4 / -1

Mark Review

Given
(i) HCN(aq)+H2O(I)⇌H3O+(aq)+CN−(aq)
Ka=6.2×10−10
(ii) CN−(aq)+H2O(I)⇌HCN(aq)+OH−(aq)
Kb=1.6×10−5
These equilibria show the following order of the relative base strength,
[Online May 12, 2012]

A

OH−>H2O>CN−

B

OH−>CN−>H2O

C

H2O>CN−>OH−

D

CN−>H2O>OH−

Question 184/223

4 / -1

Mark Review

The solubility (in molL−1 ) of AgCl(Ksp=1.0×10−10) in a 0.1 M KCl solution will be

[Online May 7, 2012]

The solubility (in molL−1 ) of AgCl(Ksp=1.0×10−10) in a 0.1 M KCl solution will be

[Online May 7, 2012]

A

1.0×10−9

B

1.0×10−10

C

1.0×10−5

D

1.0×10−11

Question 185/223

4 / -1

Mark Review

If Ksp of CaF2 at 25∘C is 1.7×10−10, the combination amongst the following which gives a precipitate of CaF2 is

[Online May 19, 2012]

If Ksp of CaF2 at 25∘C is 1.7×10−10, the combination amongst the following which gives a precipitate of CaF2 is

[Online May 19, 2012]

A

1×10−2MCa2+ and 1×10−3MF−

B

1×10−4MCa2+ and 1×10−4MF−

C

1×10−2MCa2+ and 1×10−5MF

D

1×10−3MCa2+ and 1×10−5MF−

Question 186/223

4 / -1

Mark Review

The solubility of PbI2 at 25∘C is 0.7gL−1. The solubility product of PbI2 at this temperature is (molar mass of PbI2=461.2gmol−1)

[Online May 26, 2012]

The solubility of PbI2 at 25∘C is 0.7gL−1. The solubility product of PbI2 at this temperature is (molar mass of PbI2=461.2gmol−1)

[Online May 26, 2012]

A

1.40×10−9

B

0.14×10−9

C

140×10−9

D

14.0×10−9

Question 187/223

4 / -1

Mark Review

An acid HA ionises as
HA⇌H++A−
The pH of 1.0M solution is 5. Its dissociation constant would be :

[2011RS]

An acid HA ionises as
HA⇌H++A−
The pH of 1.0M solution is 5. Its dissociation constant would be :

[2011RS]

A

5

B

5×10−8

C

1×10−5

D

1×10−10

Question 188/223

4 / -1

Mark Review

The Ksp for Cr(OH)3 is 1.6×10−30. The solubility of this compound in water is :

[2011 RS]

The Ksp for Cr(OH)3 is 1.6×10−30. The solubility of this compound in water is :

[2011 RS]

A

4√1.6×10−30

B

4√1.6×10−30∕27

C

1.6×10−30∕27

D

2√1.6×10−30

Question 189/223

4 / -1

Mark Review

In aqueous solution the ionization constants for carbonic acid are
KL=4.2×10−7 and K2=4.8×10−11
Select the correct statement for a saturated 0.034M solution of the carbonic acid.

[2010]

In aqueous solution the ionization constants for carbonic acid are
KL=4.2×10−7 and K2=4.8×10−11
Select the correct statement for a saturated 0.034M solution of the carbonic acid.

[2010]

A

The concentration of CO32− is 0.034M.

B

The concentration of CO32− is greater than that of HCO3−

C

The concentrations of H+ and HCO3− are approximately equal.

D

The concentration of H+ is double that of CO32−.

Question 190/223

4 / -1

Mark Review

Solubility product of silver bromide is 5.0×10−13. The quantity of potassium bromide (molar mass taken as 120g mol−1 ) to be added to 1 litre of 0.05M solution of silver nitrate to start the precipitation of AgBr is

[2010]

Solubility product of silver bromide is 5.0×10−13. The quantity of potassium bromide (molar mass taken as 120g mol−1 ) to be added to 1 litre of 0.05M solution of silver nitrate to start the precipitation of AgBr is

[2010]

A

1.2×10−10g

B

1.2×10−9g

C

6.2×10−5g

D

5.0×108g

Question 191/223

4 / -1

Mark Review

At 25∘C, the solubility product of Mg(OH)2 is 1.0×10−11. At which pH, will Mg2+ ions start precipitating in the form of Mg(OH)2 from a solution of 0.001MMg2+ ions?

[2010]

At 25∘C, the solubility product of Mg(OH)2 is 1.0×10−11. At which pH, will Mg2+ ions start precipitating in the form of Mg(OH)2 from a solution of 0.001MMg2+ ions?

[2010]

A

9

B

10

C

11

D

8

8 Question 192/223

4 / -1

Mark Review

Three reactions involving H2PO4− are given below:
(i) H3PO4+H2O→H3O++H2PO4− [2010]
(ii) H2PO4−+H2O→HPO42−+H3O+
(iii) H22PO4−+OH−→H3PO4+O2
In which of the above does H2PO4− act as an acid ?

[2010]

Three reactions involving H2PO4− are given below:
(i) H3PO4+H2O→H3O++H2PO4− [2010]
(ii) H2PO4−+H2O→HPO42−+H3O+
(iii) H22PO4−+OH−→H3PO4+O2
In which of the above does H2PO4− act as an acid ?

[2010]

A

(ii) only

B

(i) and (ii)

C

(iii) only

D

(i) only

Question 193/223

4 / -1

Mark Review

Solid Ba(NO3)2 is gradually dissolved in a 1.0×10−4M Na2CO3 solution. At what concentration of Ba2+ will a precipitate begin to form? (Kxp for for BaCO3=5.1×10−9)

[2009]

Solid Ba(NO3)2 is gradually dissolved in a 1.0×10−4M Na2CO3 solution. At what concentration of Ba2+ will a precipitate begin to form? (Kxp for for BaCO3=5.1×10−9)

[2009]

A

5.1×10−5M

B

8.1×10−8M

C

8.1×10−7M

D

4.1×10−5M

Question 194/223

4 / -1

Mark Review

The equilibrium constants Kp1 and Kp2 for the reactions X⇌2Y and Z⇌P+Q, respectively are in the ratio of 1:9. If the degree of dissociation of X and Z be equal, then the ratio of total pressures at these equilibria is

[2008]

The equilibrium constants Kp1 and Kp2 for the reactions X⇌2Y and Z⇌P+Q, respectively are in the ratio of 1:9. If the degree of dissociation of X and Z be equal, then the ratio of total pressures at these equilibria is

[2008]

A

1:36

B

1:1

C

1:3

D

1:9

Question 195/223

4 / -1

Mark Review

For the following threereactions (i), (ii) and (iii), equilibrium constants are given:
(i) CO(g)+H2O(g)⇌CO2(g)+H2(g);Kl
(ii) CH4(g)+H2O(g)⇌CO(g)+3H2(g);K2
(iii) CH4(g)+2H2O(g)⇌CO2(g)+4H2(g);K3
Which of the following is correct?

[2008]

For the following threereactions (i), (ii) and (iii), equilibrium constants are given:
(i) CO(g)+H2O(g)⇌CO2(g)+H2(g);Kl
(ii) CH4(g)+H2O(g)⇌CO(g)+3H2(g);K2
(iii) CH4(g)+2H2O(g)⇌CO2(g)+4H2(g);K3
Which of the following is correct?

[2008]

A

K1√K2=K3

B

K2K3=K1

C

K3=K1K2

D

K3⋅K23=K12

Question 196/223

4 / -1

Mark Review

Four species are listed below:
i. HCO3−
ii. H3O+
iii. HSO4−
iv. HSO3F
Which one of the following is the correct sequence of their acid strength?
[2008]

A

iv<ii<iii<i

B

ii<iii<i<iv

C

i<iii<ii<iv

D

iii<1<iv<ii

Question 197/223

4 / -1

Mark Review

The pKa of a weak acid, HA, is 4.80. The pKb of a weak base, BOH, is 4.78. The pH of an aqueous solution of the corresponding salt, BA, will be

[2008]

The pKa of a weak acid, HA, is 4.80. The pKb of a weak base, BOH, is 4.78. The pH of an aqueous solution of the corresponding salt, BA, will be

[2008]

A

9.58

B

4.79

C

7.01

D

9.22

9.22 Question 198/223

4 / -1

Mark Review

The first and second dissociation constants of an acid H2 A are 1.0×10−5 and 5.0×10−10 respectively. The overall dissociation constant of the acid will be

[2007]

The first and second dissociation constants of an acid H2 A are 1.0×10−5 and 5.0×10−10 respectively. The overall dissociation constant of the acid will be

[2007]

A

0.2×105

B

5.0×10−5

C

5.0×1015

D

5.0×10−15.

Question 199/223

4 / -1

Mark Review

The pKa of a weak acid (HA) is 4.5. The pOH of an aqueous buffer solution of HA in which 50% of the acid is ionized is

[2007]

The pKa of a weak acid (HA) is 4.5. The pOH of an aqueous buffer solution of HA in which 50% of the acid is ionized is

[2007]

A

7.0

B

4.5

C

2.5

D

9.5

9.5 Question 200/223

4 / -1

Mark Review

In a saturated solution of the sparingly soluble strong electrolyte AgIO3 (molecular mass =283 ) the equilibrium which sets in is AgIO3(s)⇌Ag+(aq)+IO3−(aq). If the solubility product constant Ksp of AgIO3 at a given temperature is 1.0×10−8, what is the mass of AgIO3 contained in 100mL of its saturated solution?

[2007]

In a saturated solution of the sparingly soluble strong electrolyte AgIO3 (molecular mass =283 ) the equilibrium which sets in is AgIO3(s)⇌Ag+(aq)+IO3−(aq). If the solubility product constant Ksp of AgIO3 at a given temperature is 1.0×10−8, what is the mass of AgIO3 contained in 100mL of its saturated solution?

[2007]

A

1.0×10−4g

B

28.3×10−2g

C

2.83×10−3g

D

1.0×10−7g.

Question 201/223

4 / -1

Mark Review

Phosphorus pentachloride dissociates as follows, in a closed reaction vessel
PCl5(g)⇌PCl3(g)+Cl2(g)
If total pressure at equilibrium of the reaction mixture is P and degree of dissociation of PCl5 is x, the partial pressure of PCl3 will be

[2006]

Phosphorus pentachloride dissociates as follows, in a closed reaction vessel
PCl5(g)⇌PCl3(g)+Cl2(g)
If total pressure at equilibrium of the reaction mixture is P and degree of dissociation of PCl5 is x, the partial pressure of PCl3 will be

[2006]

A

(‌
x
x−1
)P

B

(‌
x
1−x
)P

C

(‌
x
x+1
)P

D

(‌
2x
1−x
)P

Question 202/223

4 / -1

Mark Review

The equilibrium constant for the reaction
SO3(g)⇌SO2(g)+‌

1

2

O2(g)
is Kc=4.9×10−2.
The value of Kc for the reaction 2SO2(g)+O2(g)⇌2SO3(g)
will be

[2006]

The equilibrium constant for the reaction
SO3(g)⇌SO2(g)+‌

1

2

O2(g)
is Kc=4.9×10−2.
The value of Kc for the reaction 2SO2(g)+O2(g)⇌2SO3(g)
will be

[2006]

A

9.8×10−2

B

4.9×10−2

C

416

D

2.40×10−3

Question 203/223

4 / -1

Mark Review

For the reaction :
2NO2(g)⇌2NO(g)+O2(g)
(Kc=1.8×10−6 at 184∘C)(R=0.0831kJ∕(mol.K))
When Kp and Kc are compared at 184∘C, it is found that
[2005]

A

Whether Kp is greater than, less than or equal to Kc depends upon the total gas pressure

B

Kp=Kc

C

Kp is less than Kc

D

Kp is greater than Kc

Question 204/223

4 / -1

Mark Review

An amount of solid NH4HS is placed in a flask already containing ammonia gas at a certain temperature and 0.50 atm pressure. Ammonium hydrogen sulphide decomposes to yield NH3 and N2S gases in the flask. When the decomposition reaction reaches equilibrium, the total pressure in the flask rises to 0.84 atm? The equilibrium constant for NH4HS decomposition at this temperature is

[2005]

An amount of solid NH4HS is placed in a flask already containing ammonia gas at a certain temperature and 0.50 atm pressure. Ammonium hydrogen sulphide decomposes to yield NH3 and N2S gases in the flask. When the decomposition reaction reaches equilibrium, the total pressure in the flask rises to 0.84 atm? The equilibrium constant for NH4HS decomposition at this temperature is

[2005]

A

0.11

B

0.17

C

0.18

D

0.30

0.30 Question 205/223

4 / -1

Mark Review

The exothermic formation of CIF3 is represented by the equation:
Cl2(g)+3F2(g)⇌2ClF3(g);‌‌∆H=−329kJ
Which of the following will increase the quantity of CIF3 in an equilibrium mixture of Cl2,F2 and ClF3 ?

[2005]

The exothermic formation of CIF3 is represented by the equation:
Cl2(g)+3F2(g)⇌2ClF3(g);‌‌∆H=−329kJ
Which of the following will increase the quantity of CIF3 in an equilibrium mixture of Cl2,F2 and ClF3 ?

[2005]

A

Adding F2

B

Increasing the volume of the container

C

Removing Cl2

D

Increasing the temperature

Question 206/223

4 / -1

Mark Review

Hydrogen ion concentration in mol∕L in a solution of pH=5.4 will be:

[2005]

Hydrogen ion concentration in mol∕L in a solution of pH=5.4 will be:

[2005]

A

3.98×10−6

B

3.68×10−6

C

3.88×106

D

3.98×108

Question 207/223

4 / -1

Mark Review

What is the conjugate base of OH− ?

[2005]

What is the conjugate base of OH− ?

[2005]

A

O2−

B

O−

C

H2O

D

O2

Question 208/223

4 / -1

Mark Review

The solubility product of a salt having general formula MX2, in water, is :4×10−12. The concentration of M2+ ions in the aqueous solution of the salt is

[2005]

The solubility product of a salt having general formula MX2, in water, is :4×10−12. The concentration of M2+ ions in the aqueous solution of the salt is

[2005]

A

4.0×10−10M

B

1.6×10−4M

C

1.0×10−4M

D

2.0×10−6M

Question 209/223

4 / -1

Mark Review

The equilibrium constant (Kc) for the reaction N2(g)+O2(g) →2NO(g) at temperature T is 4×10−4. The value of Kc for the reaction
NO(g)→‌

1

2

N2(g)+‌

1

2

O2(g) at the same temperature is:

[2004, 2012]

The equilibrium constant (Kc) for the reaction N2(g)+O2(g) →2NO(g) at temperature T is 4×10−4. The value of Kc for the reaction
NO(g)→‌

1

2

N2(g)+‌

1

2

O2(g) at the same temperature is:

[2004, 2012]

A

0.02

B

2.5×102

C

4×10−4

D

50.0

50.0 Question 210/223

4 / -1

Mark Review

What is the equilibrium expression for the reaction
P4(s)+5O2(g)⇌P4O10(s)?

[2004]

What is the equilibrium expression for the reaction
P4(s)+5O2(g)⇌P4O10(s)?

[2004]

A

Kc=[O2]5

B

Kc=[P4O10]∕5[P4][O2]

C

Kc=[P4O10]∕[P4][O2]5

D

Kc=1∕[O2]5

Question 211/223

4 / -1

Mark Review

For the reaction, CO(g)+Cl2(g)⇌COCl2(g) the Kp∕Kc is equal to

[2004]

For the reaction, CO(g)+Cl2(g)⇌COCl2(g) the Kp∕Kc is equal to

[2004]

A

√RT

B

RT

C

1∕RT

D

1.0

1.0 Question 212/223

4 / -1

Mark Review

The conjugate base of H2PO4− is

[2004]

The conjugate base of H2PO4− is

[2004]

A

H3PO4

B

P2O5

C

PO43−

D

HPO42−

Question 213/223

4 / -1

Mark Review

The molar solubility (in molL−1 ) of a sparingly soluble salt MX4 is 's'. The corresponding solubility product is Ksp∘ 's' is given in term of Ksp by the relation:

[2004]

The molar solubility (in molL−1 ) of a sparingly soluble salt MX4 is 's'. The corresponding solubility product is Ksp∘ 's' is given in term of Ksp by the relation:

[2004]

A

s=(256Ksp)1∕5

B

s=(128Ksp)1∕4

C

s=(Ksp∕128)1∕4

D

s=(Ksp∕256)1∕5

Question 214/223

4 / -1

Mark Review

For the reaction equilibrium
N2O4(g)⇌2NO2(g)
the concentrations of N2O4 and NO2 at equilibrium are 4.8×10−2 and 1.2×10−2molL−1 respectively. The value of Kc for the reaction is

[2003]

For the reaction equilibrium
N2O4(g)⇌2NO2(g)
the concentrations of N2O4 and NO2 at equilibrium are 4.8×10−2 and 1.2×10−2molL−1 respectively. The value of Kc for the reaction is

[2003]

A

3×10−1molL−1

B

3×10−3molL−1

C

3×103molL−1

D

3.3×102molL−1

Question 215/223

4 / -1

Mark Review

Consider the reaction equilibrium

2SO2(g)+O2(g)⇌2SO3(g);∆H∘=−198kJ

On the basis of Le Chatelier's principle, the condition favourable for the forward reaction is
[2003]

Consider the reaction equilibrium

2SO2(g)+O2(g)⇌2SO3(g);∆H∘=−198kJ

On the basis of Le Chatelier's principle, the condition favourable for the forward reaction is
[2003]

A

increasing temperature as well as pressure

B

lowering the temperature and increasing the pressure

C

any value of temperature and pressure

D

lowering of temperature as well as pressure

Question 216/223

4 / -1

Mark Review

Which one of the following statements is not true?

[2003]

Which one of the following statements is not true?

[2003]

A

pH+pOH=14 for all aqueous solutions

B

The pH of 1×108MHCl is 8

C

96,500 coulombs of electricity when passed through a CuSO4 solution deposits 1 gram equivalent of copper at the cathode

D

The conjugate base of H2PO4− is HPO42−

Question 217/223

4 / -1

Mark Review

When rain is accompanied by a thunderstorm, the collected rain water will have a pH value

[2003]

When rain is accompanied by a thunderstorm, the collected rain water will have a pH value

[2003]

A

slightly higher than that when the thunderstorm is not there

B

uninfluenced by occurrence of thunderstorm

C

that depends on the amount of dust in air

D

slightly lower than that of rain water without thunderstorm.

Question 218/223

4 / -1

Mark Review

The solubility in water of a sparingly soluble salt AB2 is 1.0×10−5molL−1. Its solubility product will be

[2003]

The solubility in water of a sparingly soluble salt AB2 is 1.0×10−5molL−1. Its solubility product will be

[2003]

A

4×10−10

B

1×10−15

C

1×10−10

D

4×10−15

Question 219/223

4 / -1

Mark Review

For the reaction CO(g)+(1∕2)O2(g)⇌CO2(g),Kp∕Kc is

[2002]

For the reaction CO(g)+(1∕2)O2(g)⇌CO2(g),Kp∕Kc is

[2002]

A

RT

B

(RT)−1

C

(RT)−1∕2

D

(RT)1∕2

Question 220/223

4 / -1

Mark Review

Change in volume of the system does not alter which of the following equilibria?

[2002]

Change in volume of the system does not alter which of the following equilibria?

[2002]

A

N2(g)+O2(g)⇌2NO(g)

B

PCl5(g)⇌PCl3(g)+Cl2(g)

C

N2(g)+3H2(g)⇌2NH3(g)

D

SO2Cl2(g)⇌SO2(g)+Cl2(g)

Question 221/223

4 / -1

Mark Review

Species acting as both Bronsted acid and base is

[2002]

Species acting as both Bronsted acid and base is

[2002]

A

HSO4−

B

Na2CO3

C

NH3

D

OH

Question 222/223

4 / -1

Mark Review

Let the solubility of an aqueous solution of Mg(OH)2, be x, then its Ksp is

[2002]

Let the solubility of an aqueous solution of Mg(OH)2, be x, then its Ksp is

[2002]

A

4x3

B

108x5

C

27x4

D

9x.

Question 223/223

4 / -1

Mark Review

1M‌NaCl and 1M‌HCl are present in an aqueous solution. The solution is

[2002]

1MNaCl and 1MHCl are present in an aqueous solution. The solution is

[2002]

A

not a buffer solution with pH<7

B

not a buffer solution with pH>7

C

a buffer solution with pH<7

D

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Both Statement I and Statement II are correct

Both Statement I and Statement II are correct

Statement I is correct but Statement II is incorrect

Statement I is correct but Statement II is incorrect

Both Statement I and Statement II are incorrect

Both Statement I and Statement II are incorrect

Statement I is incorrect but Statement II is correct

Statement I is incorrect but Statement II is correct

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