The hydrogen ion concentration of a 0.006,M b | vedclass

Name: PDF Generator App | JEE NEET Paper Generator | Vedclass
Brand: Vedclass
Rating: 5 (35 reviews)

Question

(b) Initial concentration $= 0.006\, M$ $==>$ ${K_a} = 6 	imes {10^{ - 5}}$
equilibrium reaction.

$\mathop {\mathop {{C_6}{H_5}COOH}\limits_C

Vedclass · Accepted Answer

$6 	imes {10^{ - 4}}$

Vedclass · Answer

(b) Initial concentration $= 0.006\, M$ $==>$ ${K_a} = 6 	imes {10^{ - 5}}$
equilibrium reaction.

$\mathop {\mathop {{C_6}{H_5}COOH}\limits_C }\limits_{C(1 - a)\,\,\,} $$ ightleftharpoons $$\mathop {\mathop {{C_6}{H_5}CO{O^ - }}\limits_O }\limits_{Ca} + \mathop {\mathop {{H^ + }\,\,\,\,\,\,\,}\limits_{O\,\,{m{initial}}} }\limits_{Ca\,\,\,\,\,\,\,\,\,\,\,\,\,\,} $

${K_a} = C{\alpha ^2}$ for weak electrolyte

$\alpha = \sqrt {\frac{{{K_a}}}{C}} $; $\alpha = \sqrt {\frac{{6 	imes {{10}^{ - 5}}}}{{0.006}}} $; $\alpha = {10^{ - 1}}$

$ = 0.006 	imes {10^{ - 1}}$$ = 6 	imes {10^{ - 4}}\,M$.

The hydrogen ion concentration of a $0.006\,M$ benzoic acid solution is $({K_a} = 6 \times {10^{ - 5}})$

Similar Questions

A monoprotic acid in a $0.1\,\,M$ solution ionizes to $0.001\%$. Its ionisation constant is

$5.0$ $pH$ containing solution is dilute $100$ times. Calculate $pH$ of dilute solution.

${K_a}$ of $C{H_3}COOH$ is $1.76 \times {10^{ - 5}}$ at $298$ $K$ temperature. Calculate dissociation constant of its conjugate base.

The degree of dissociation $(\alpha )$ of $PCl_5$ obeying the equilibrium; is $PC{l_5}\, \rightleftharpoons \,PC{l_3}\, + \,C{l_2}$ related to the pressure at equlibrium by

Derive the equation of ionization constant $({K_b})$ of weak base.