For a weak acid HA with dissociation constant | vedclass

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

Question

(d) Dissociation constant of $HA = {10^{ - 9}}$

$HA⇌{H^ + } + {A^ - }$

$[{H^ + }] = \sqrt {\frac{{{K_a}}}{C}} $ $ = \sqrt {\frac{{{{10}^{ - 9}}}

Vedclass · Accepted Answer

$9$

Vedclass · Answer

(d) Dissociation constant of $HA = {10^{ - 9}}$

$HA⇌{H^ + } + {A^ - }$

$[{H^ + }] = \sqrt {\frac{{{K_a}}}{C}} $ $ = \sqrt {\frac{{{{10}^{ - 9}}}}{{0.1}}} $ ; $[{H^ + }] = {10^{ - 5}}$

$	herefore \,pH = 5$

$pH+pOH = 14$

$pOH = 14 - pH$$ = 14 - 5$ ; $pOH = 9$

For a weak acid $HA$ with dissociation constant ${10^{ - 9}},\,\,pOH$ of its $0.1 \,M$ solution is

Similar Questions

It has been found that the $pH$ of a $0.01$ $M$ solution of an organic acid is $4.15 .$ Calculate the concentration of the anion, the ionization constant of the acid and its $p{K_a}$

Write examples of weak acids and weak bases and give ionic equilibrium in its aqueous solution.

$25$ $mL$ $0.1$ $M$ $HCl$ solution is diluted till $500$ $mL$. Calculate $pH$ of dilute solution.

$0.01\, M \,HA(aq.)$ is $2\%$ ionized, $[OH^-]$ of solution is :-

The ionization constant of $0.1$ $M$ weak acid is $1.74 \times {10^{ - 5}}$ at $298$ $K$ temperature. Calculate $pH$ of its $0.1$ $M$ solution.