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Ionic Equilibrium

32437 An example for a strong electrolyte is

1 Urea

2 Ammonium hydroxide

3 Sugar

4 Sodium acetate

Explanation:

(d) $C H_{3} C O O N a$ $⇌$ $C H_{3} C O O^{-} + N a^{+}$
$H_{2} O$ $⇌$ $H^{+} + O H^{-}$
$C H_{3} C O O H + N a O H$

Ionic Equilibrium

32438 Which one is strongest electrolyte in the following

1

N a C l

2

C H_{3} C O O H

3

N H_{4} O H

4

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

Explanation:

(a) $N a C l$ , being a salt, is a strong electrolyte.

Ionic Equilibrium

32439 If $α$ is the degree of ionization, $C$ the concentration of a weak electrolyte and $K_{a}$ the acid ionization constant, then the correct relationship between $α, C$ and $K_{a}$ is

1

α^{2} = \sqrt{\frac{K_{a}}{C}}

2

α^{2} = \sqrt{\frac{C}{K_{a}}}

3

α = \sqrt{\frac{K_{a}}{C}}

4

α = \sqrt{\frac{C}{K_{a}}}

Explanation:

(c) According to the Ostwald’s dilution formula $α^{2} = \frac{K (1 - α)}{C}$ . But for weak electrolytes $α$ is very small. So that $(1 - α)$ can be neglected. So that $α = \sqrt{\frac{K_{a}}{C}}$ .

Ionic Equilibrium

32440 Theory of ionization was given by

1 Rutherford

2 Graham

3 Faraday

4 Arrhenius

Ionic Equilibrium

32437 An example for a strong electrolyte is

1 Urea

2 Ammonium hydroxide

3 Sugar

4 Sodium acetate

Explanation:

(d) $C H_{3} C O O N a$ $⇌$ $C H_{3} C O O^{-} + N a^{+}$
$H_{2} O$ $⇌$ $H^{+} + O H^{-}$
$C H_{3} C O O H + N a O H$

Ionic Equilibrium

32438 Which one is strongest electrolyte in the following

1

N a C l

2

C H_{3} C O O H

3

N H_{4} O H

4

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

Explanation:

(a) $N a C l$ , being a salt, is a strong electrolyte.

Ionic Equilibrium

32439 If $α$ is the degree of ionization, $C$ the concentration of a weak electrolyte and $K_{a}$ the acid ionization constant, then the correct relationship between $α, C$ and $K_{a}$ is

1

α^{2} = \sqrt{\frac{K_{a}}{C}}

2

α^{2} = \sqrt{\frac{C}{K_{a}}}

3

α = \sqrt{\frac{K_{a}}{C}}

4

α = \sqrt{\frac{C}{K_{a}}}

Explanation:

(c) According to the Ostwald’s dilution formula $α^{2} = \frac{K (1 - α)}{C}$ . But for weak electrolytes $α$ is very small. So that $(1 - α)$ can be neglected. So that $α = \sqrt{\frac{K_{a}}{C}}$ .

Ionic Equilibrium

32440 Theory of ionization was given by

1 Rutherford

2 Graham

3 Faraday

4 Arrhenius

Ionic Equilibrium

32437 An example for a strong electrolyte is

1 Urea

2 Ammonium hydroxide

3 Sugar

4 Sodium acetate

Explanation:

(d) $C H_{3} C O O N a$ $⇌$ $C H_{3} C O O^{-} + N a^{+}$
$H_{2} O$ $⇌$ $H^{+} + O H^{-}$
$C H_{3} C O O H + N a O H$

Ionic Equilibrium

32438 Which one is strongest electrolyte in the following

1

N a C l

2

C H_{3} C O O H

3

N H_{4} O H

4

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

Explanation:

(a) $N a C l$ , being a salt, is a strong electrolyte.

Ionic Equilibrium

32439 If $α$ is the degree of ionization, $C$ the concentration of a weak electrolyte and $K_{a}$ the acid ionization constant, then the correct relationship between $α, C$ and $K_{a}$ is

1

α^{2} = \sqrt{\frac{K_{a}}{C}}

2

α^{2} = \sqrt{\frac{C}{K_{a}}}

3

α = \sqrt{\frac{K_{a}}{C}}

4

α = \sqrt{\frac{C}{K_{a}}}

Explanation:

(c) According to the Ostwald’s dilution formula $α^{2} = \frac{K (1 - α)}{C}$ . But for weak electrolytes $α$ is very small. So that $(1 - α)$ can be neglected. So that $α = \sqrt{\frac{K_{a}}{C}}$ .

Ionic Equilibrium

32440 Theory of ionization was given by

1 Rutherford

2 Graham

3 Faraday

4 Arrhenius

Ionic Equilibrium

32437 An example for a strong electrolyte is

1 Urea

2 Ammonium hydroxide

3 Sugar

4 Sodium acetate

Explanation:

(d) $C H_{3} C O O N a$ $⇌$ $C H_{3} C O O^{-} + N a^{+}$
$H_{2} O$ $⇌$ $H^{+} + O H^{-}$
$C H_{3} C O O H + N a O H$

Ionic Equilibrium

32438 Which one is strongest electrolyte in the following

1

N a C l

2

C H_{3} C O O H

3

N H_{4} O H

4

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

Explanation:

(a) $N a C l$ , being a salt, is a strong electrolyte.

Ionic Equilibrium

32439 If $α$ is the degree of ionization, $C$ the concentration of a weak electrolyte and $K_{a}$ the acid ionization constant, then the correct relationship between $α, C$ and $K_{a}$ is

1

α^{2} = \sqrt{\frac{K_{a}}{C}}

2

α^{2} = \sqrt{\frac{C}{K_{a}}}

3

α = \sqrt{\frac{K_{a}}{C}}

4

α = \sqrt{\frac{C}{K_{a}}}

Explanation:

(c) According to the Ostwald’s dilution formula $α^{2} = \frac{K (1 - α)}{C}$ . But for weak electrolytes $α$ is very small. So that $(1 - α)$ can be neglected. So that $α = \sqrt{\frac{K_{a}}{C}}$ .

Ionic Equilibrium

32440 Theory of ionization was given by

1 Rutherford

2 Graham

3 Faraday

4 Arrhenius

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Question Bank Series

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