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

$α^{2} = \sqrt{K_{a} \times C}$ .

No worries! We‘ve got your back. Try BYJU‘S free classes today!

$α^{2} = \sqrt{\frac{C}{K_{a}}}$

No worries! We‘ve got your back. Try BYJU‘S free classes today!

$α = \sqrt{\frac{K_{a}}{C}}$

Right on! Give the BNAT exam to get a 100% scholarship for BYJUS courses

$α = \sqrt{\frac{C}{K_{a}}}$

No worries! We‘ve got your back. Try BYJU‘S free classes today!

Open in App

Solution

The correct option is C
$α = \sqrt{\frac{K_{a}}{C}}$

According to the Ostwald's dilution formula $α^{2} - \frac{K_{a} (1 - α)}{C}$ . But for weak

electrolytes $α$ is very small. So that $(1 - α$ ) can be taken as 1. So that $α = \sqrt{\frac{K_{a}}{C}}$ .

Suggest Corrections

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. If the degree of ionization

(α)

of a weak electrolyte

A B

is very less, then

α

Q. If degree of ionization

(α)

of a weak electrolyte

A B

is very less, then

α

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 :

Q. If concentration of two weak acids are different and degree of ionization

(α)

is very less, then their relative strength can be compared by:

Join BYJU'S Learning Program

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 = √KaC According to the Ostwald's dilution formula α2 − Ka(1 − α)C. But for weak electrolytes α is very small. So that (1 − α) can be taken as 1. So that 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 the Ostwald's dilution formula $α^{2} - \frac{K_{a} (1 - α)}{C}$ . But for weak

electrolytes $α$ is very small. So that $(1 - α$ ) can be taken as 1. So that $α = \sqrt{\frac{K_{a}}{C}}$ .