Calculate $pH$ of solution of $6.0$ $gm$ acetic acid in $250$ $mL$. ( ${K_a} = 1.8 \times {10^{ – 5}}$ at $298$ $K$ ) ( $C = 12, H = 1, O = 16$ )

${K_{C{H_3}COOH}} = 1.9 \times {10^{ – 5}}$. Calculate $pH$ at end point in titration of $0.1$ $M$ $C{H_3}COOH$ and $0.1$ $M$ $NaOH$.

The $pH$ of a $0.1\  M$ aqueous solution of a very weak acid $(HA)$ is $3$. What is its degree of dissociation ?……$\%$

$0.1$ $mol$ of $H_2S(g)$ is kept in a $0.4$ litre vessel at $1000\,K$. For the reaction –
$2{H_2}S(g)\,\rightleftharpoons\,2{H_2}(g)\, + \,{S_2}(g)\,;\,{K_c} = {10^{ – 6}}\% $ dissociation of $H_2S$ is…….$\%$

${K_b}$ of $N{H_4}OH = 1.8 \times {10^{ – 5}}$ calculate $pH$ of $0.15$ $mol$ $N{H_4}OH$ and $0.25$ $mol$ $N{H_4}OH$ containing solution.