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Ionic Equilibrium

229351 The activation energy for a simple chemical reaction $A \to B$ is $E_{a}$ in forward direction. They activation energy for reverse reaction

1 is negative of

E_{a}

2 is always less than

E_{a}

3 can be less than or more than

E_{a}

4 is always double of

E_{a}

Explanation:

The activation energy of reverse reaction is less than or more than activation energy $(E_{a})$ of forward reaction.
$∵ Δ H = {(E_{a})}_{F} - {(E_{a})}_{R}$
Because it depends. upon the nature of reaction.
If ${(E_{a})}_{F} < {(E_{a})}_{R}$ reaction is exothermic
or ${(E_{a})}_{F} > {(E_{a})}_{R}$ reaction is endothermic

UPTU/UPSEE-2018]**

Ionic Equilibrium

229344 Find the correct statement about catalyst.

1 It changes the value of equilibrium constant

K_{c}

or

K_{p}

.

2 It decreases the activation energy of a reaction.

3 It changes the enthalpy of a reaction.

4 It is not specific in its function.

Explanation:

A catalyst is a substance which increase the rate of reaction without itself undergoing any permanent chemical change. Catalyst provides an alternate reaction mechanism by reducing the activation energy between reactants and product. A catalyst does not alter Gibbs energy $(Δ G)$ .

SRM JEEE-2013

Ionic Equilibrium

229345 $20 ml$ of $0.1 M$ acetic acid is mixed with $50 mL$ of potassium acetate. $K_{a}$ of acetic acid $= 1.8 \times$ $10^{- 5}$ at $27^{\circ} C$ . Calculate concentration of potassium acetate if $pH$ of the mixture is 4.8 .

1

0.1 M

2

0.04 M

3

0.4 M

4

0.02 M

Explanation:

Given that, $pH = 4.8, {pK}_{a} = 1.8 \times 10^{- 5}$ Let the concentration of potassium acetate is $x$ . According to Henderson's equation $pH = {pK}_{a} + \log \frac{[salt]}{[acid]}$ or $4.8 = - \log (1.8 \times 10^{- 5}) + \log \frac{x \times 50}{20 \times 0.1 M}$ or $4.8 = 4.74 + \log 25 x$ $\log 25 x = 0.06$ $25 x = 1.148$ $∴ x = 0.045 M$

VITEEE-2009

Ionic Equilibrium

229355 Aqueous solution of which of the following compound is the best conductor of electric current?

1 Hydrochloric acid,

HCl

2 Ammonia

{NH}_{3}

3 Fructose

C_{6} H_{12} O_{6}

4 Acetic acid,

C_{2} H_{4} O_{2}

Explanation:

The aqueous solution of hydrochloric acid $(HCl)$ is the best conductor of electric current as it is a strong electrolyte and its completely dissociated into ions.

NEET-2015

Ionic Equilibrium

229351 The activation energy for a simple chemical reaction $A \to B$ is $E_{a}$ in forward direction. They activation energy for reverse reaction

1 is negative of

E_{a}

2 is always less than

E_{a}

3 can be less than or more than

E_{a}

4 is always double of

E_{a}

Explanation:

The activation energy of reverse reaction is less than or more than activation energy $(E_{a})$ of forward reaction.
$∵ Δ H = {(E_{a})}_{F} - {(E_{a})}_{R}$
Because it depends. upon the nature of reaction.
If ${(E_{a})}_{F} < {(E_{a})}_{R}$ reaction is exothermic
or ${(E_{a})}_{F} > {(E_{a})}_{R}$ reaction is endothermic

UPTU/UPSEE-2018]**

Ionic Equilibrium

229344 Find the correct statement about catalyst.

1 It changes the value of equilibrium constant

K_{c}

or

K_{p}

.

2 It decreases the activation energy of a reaction.

3 It changes the enthalpy of a reaction.

4 It is not specific in its function.

Explanation:

A catalyst is a substance which increase the rate of reaction without itself undergoing any permanent chemical change. Catalyst provides an alternate reaction mechanism by reducing the activation energy between reactants and product. A catalyst does not alter Gibbs energy $(Δ G)$ .

SRM JEEE-2013

Ionic Equilibrium

229345 $20 ml$ of $0.1 M$ acetic acid is mixed with $50 mL$ of potassium acetate. $K_{a}$ of acetic acid $= 1.8 \times$ $10^{- 5}$ at $27^{\circ} C$ . Calculate concentration of potassium acetate if $pH$ of the mixture is 4.8 .

1

0.1 M

2

0.04 M

3

0.4 M

4

0.02 M

Explanation:

Given that, $pH = 4.8, {pK}_{a} = 1.8 \times 10^{- 5}$ Let the concentration of potassium acetate is $x$ . According to Henderson's equation $pH = {pK}_{a} + \log \frac{[salt]}{[acid]}$ or $4.8 = - \log (1.8 \times 10^{- 5}) + \log \frac{x \times 50}{20 \times 0.1 M}$ or $4.8 = 4.74 + \log 25 x$ $\log 25 x = 0.06$ $25 x = 1.148$ $∴ x = 0.045 M$

VITEEE-2009

Ionic Equilibrium

229355 Aqueous solution of which of the following compound is the best conductor of electric current?

1 Hydrochloric acid,

HCl

2 Ammonia

{NH}_{3}

3 Fructose

C_{6} H_{12} O_{6}

4 Acetic acid,

C_{2} H_{4} O_{2}

Explanation:

The aqueous solution of hydrochloric acid $(HCl)$ is the best conductor of electric current as it is a strong electrolyte and its completely dissociated into ions.

NEET-2015

Ionic Equilibrium

229351 The activation energy for a simple chemical reaction $A \to B$ is $E_{a}$ in forward direction. They activation energy for reverse reaction

1 is negative of

E_{a}

2 is always less than

E_{a}

3 can be less than or more than

E_{a}

4 is always double of

E_{a}

Explanation:

The activation energy of reverse reaction is less than or more than activation energy $(E_{a})$ of forward reaction.
$∵ Δ H = {(E_{a})}_{F} - {(E_{a})}_{R}$
Because it depends. upon the nature of reaction.
If ${(E_{a})}_{F} < {(E_{a})}_{R}$ reaction is exothermic
or ${(E_{a})}_{F} > {(E_{a})}_{R}$ reaction is endothermic

UPTU/UPSEE-2018]**

Ionic Equilibrium

229344 Find the correct statement about catalyst.

1 It changes the value of equilibrium constant

K_{c}

or

K_{p}

.

2 It decreases the activation energy of a reaction.

3 It changes the enthalpy of a reaction.

4 It is not specific in its function.

Explanation:

A catalyst is a substance which increase the rate of reaction without itself undergoing any permanent chemical change. Catalyst provides an alternate reaction mechanism by reducing the activation energy between reactants and product. A catalyst does not alter Gibbs energy $(Δ G)$ .

SRM JEEE-2013

Ionic Equilibrium

229345 $20 ml$ of $0.1 M$ acetic acid is mixed with $50 mL$ of potassium acetate. $K_{a}$ of acetic acid $= 1.8 \times$ $10^{- 5}$ at $27^{\circ} C$ . Calculate concentration of potassium acetate if $pH$ of the mixture is 4.8 .

1

0.1 M

2

0.04 M

3

0.4 M

4

0.02 M

Explanation:

Given that, $pH = 4.8, {pK}_{a} = 1.8 \times 10^{- 5}$ Let the concentration of potassium acetate is $x$ . According to Henderson's equation $pH = {pK}_{a} + \log \frac{[salt]}{[acid]}$ or $4.8 = - \log (1.8 \times 10^{- 5}) + \log \frac{x \times 50}{20 \times 0.1 M}$ or $4.8 = 4.74 + \log 25 x$ $\log 25 x = 0.06$ $25 x = 1.148$ $∴ x = 0.045 M$

VITEEE-2009

Ionic Equilibrium

229355 Aqueous solution of which of the following compound is the best conductor of electric current?

1 Hydrochloric acid,

HCl

2 Ammonia

{NH}_{3}

3 Fructose

C_{6} H_{12} O_{6}

4 Acetic acid,

C_{2} H_{4} O_{2}

Explanation:

The aqueous solution of hydrochloric acid $(HCl)$ is the best conductor of electric current as it is a strong electrolyte and its completely dissociated into ions.

NEET-2015

Ionic Equilibrium

229351 The activation energy for a simple chemical reaction $A \to B$ is $E_{a}$ in forward direction. They activation energy for reverse reaction

1 is negative of

E_{a}

2 is always less than

E_{a}

3 can be less than or more than

E_{a}

4 is always double of

E_{a}

Explanation:

The activation energy of reverse reaction is less than or more than activation energy $(E_{a})$ of forward reaction.
$∵ Δ H = {(E_{a})}_{F} - {(E_{a})}_{R}$
Because it depends. upon the nature of reaction.
If ${(E_{a})}_{F} < {(E_{a})}_{R}$ reaction is exothermic
or ${(E_{a})}_{F} > {(E_{a})}_{R}$ reaction is endothermic

UPTU/UPSEE-2018]**

Ionic Equilibrium

229344 Find the correct statement about catalyst.

1 It changes the value of equilibrium constant

K_{c}

or

K_{p}

.

2 It decreases the activation energy of a reaction.

3 It changes the enthalpy of a reaction.

4 It is not specific in its function.

Explanation:

A catalyst is a substance which increase the rate of reaction without itself undergoing any permanent chemical change. Catalyst provides an alternate reaction mechanism by reducing the activation energy between reactants and product. A catalyst does not alter Gibbs energy $(Δ G)$ .

SRM JEEE-2013

Ionic Equilibrium

229345 $20 ml$ of $0.1 M$ acetic acid is mixed with $50 mL$ of potassium acetate. $K_{a}$ of acetic acid $= 1.8 \times$ $10^{- 5}$ at $27^{\circ} C$ . Calculate concentration of potassium acetate if $pH$ of the mixture is 4.8 .

1

0.1 M

2

0.04 M

3

0.4 M

4

0.02 M

Explanation:

Given that, $pH = 4.8, {pK}_{a} = 1.8 \times 10^{- 5}$ Let the concentration of potassium acetate is $x$ . According to Henderson's equation $pH = {pK}_{a} + \log \frac{[salt]}{[acid]}$ or $4.8 = - \log (1.8 \times 10^{- 5}) + \log \frac{x \times 50}{20 \times 0.1 M}$ or $4.8 = 4.74 + \log 25 x$ $\log 25 x = 0.06$ $25 x = 1.148$ $∴ x = 0.045 M$

VITEEE-2009

Ionic Equilibrium

229355 Aqueous solution of which of the following compound is the best conductor of electric current?

1 Hydrochloric acid,

HCl

2 Ammonia

{NH}_{3}

3 Fructose

C_{6} H_{12} O_{6}

4 Acetic acid,

C_{2} H_{4} O_{2}

Explanation:

The aqueous solution of hydrochloric acid $(HCl)$ is the best conductor of electric current as it is a strong electrolyte and its completely dissociated into ions.

NEET-2015

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