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Byju's Answer

Standard XII

Chemistry

Dissolution of Solids and Gases in Liquid

If α is the...

Question

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:

α^{2} = \sqrt{\frac{K_{a}}{C}}

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α^{2} = \sqrt{\frac{C}{K_{a}}}

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α = \sqrt{\frac{K_{a}}{C}}

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α = \sqrt{\frac{C}{K_{a}}}

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Solution

The correct option is C $α = \sqrt{\frac{K_{a}}{C}}$
According to Ostwald's dilution law, the degree of dissociation of a weak electrolyte is given by the formula $α = \sqrt{\frac{K_{a}}{C}}$

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Similar questions

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 $α$ , Cand $K_{a}$ is

Q. Consider a weak monobasic acid

H A

having a concentration C with degree of dissociation,

α << 1.

. The pH of this weak acid in terms of acid dissociation constant

K_{a}

and concentration

C

is :

The degree of dissociation of weak electrolyte is inversely proportional to the square root of concentration. It is called Ostwald's dilution law.

α = \sqrt{\frac{K_{a}}{c}}

, as the temperature increases, degree of dissociation will increase

\frac{α_{1}}{α_{2}} = \sqrt{\frac{K_{a_{1}}}{K_{a_{2}}}}

, if concentration is same

\frac{α_{1}}{α_{2}} = \sqrt{\frac{c_{2}}{c_{1}}}

, if acid is same

a_{1}

and

a_{2}

are in ratio of

1 : 2, K_{a_{1}} = 2 \times 10^{- 4}

. What will be

K_{a_{2}}

Q. What is the percent ionization

(α)

of a

0.01 M

H A

solution?
(Given that

K_{a} = 10^{- 4}

)

Q. Which of the following describes the correct relation for hydrolysis constant

(K_{h})

for a salt of weak acid and weak base at

25^{\circ} C ?

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If α is the degree of ionization, C the concentration of a weak electrolyte and Ka, the acid ionization constant, then the correct relationship between α,C and Ka is:

The correct option is C α=√KaCAccording to Ostwald's dilution law, the degree of dissociation of a weak electrolyte is given by the formula α=√KaC

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:

The correct option is C $α = \sqrt{\frac{K_{a}}{C}}$
According to Ostwald's dilution law, the degree of dissociation of a weak electrolyte is given by the formula $α = \sqrt{\frac{K_{a}}{C}}$