The degree of dissociation of weak electrolyte is inversely proportional to the square root of concentration. It is called Ostwald's dilution law α=√(Ka/c) As the temperature increases, degree of dissociation will increase (α1/α2)=√(Ka1/Ka2) if concentration is same (α1/α2)=√(c2/c1) if acid is same 0.01 M CH 3 COOOH has 4.24 % degree of dissociation, the degree of dissociation of 0.1 M CH 3 COOH 2 will be

Question

The degree of dissociation of weak electrolyte is inversely proportional to the square root of concentration. It is called Ostwald's dilution law α=√(Ka/c) As the temperature increases, degree of dissociation will increase (α1/α2)=√(Ka1/Ka2) if concentration is same (α1/α2)=√(c2/c1) if acid is same 0.01 M CH 3 COOOH has 4.24 % degree of dissociation, the degree of dissociation of 0.1 M CH 3 COOH 2 will be (A) 1.33 % (B) 4.24 % (C) 5.24 % (D) 0.33 %

Tardigrade Admin · Accepted Answer

Use: (α1/α2)=√(C2/C1) ⇒ (4.24/α2)=√(0.1/0.01) ⇒ α2=(4.24/√10) %=1.33 %

$1.33%$

$4.24%$

$5.24%$

$0.33%$

Use: $\frac{α _{1}}{α _{2}} = \frac{C _{2}}{C _{1}} \Rightarrow \frac{4.24}{α _{2}} = \frac{0.1}{0.01}$
$\Rightarrow α_{2} = \frac{4.24}{10} % = 1.33%$

1.33%

4.24%

5.24%

0.33%

Use: α2​α1​​=C1​C2​​​⇒α2​4.24​=0.010.1​​ ⇒α2​=10​4.24​%=1.33%

$1.33%$

$4.24%$

$5.24%$

$0.33%$

Use: $\frac{α _{1}}{α _{2}} = \frac{C _{2}}{C _{1}} \Rightarrow \frac{4.24}{α _{2}} = \frac{0.1}{0.01}$
$\Rightarrow α_{2} = \frac{4.24}{10} % = 1.33%$