At $298\,K$ a $0.1 \,M $ $C{H_3}COOH$ solution is $ 1.34\%$ ionized. The ionization constant ${K_a}$ for acetic acid will be
$1.82 \times {10^{ - 5}}$
$18.2 \times {10^{ - 5}}$
$0.182 \times {10^{ - 5}}$
None of these
A weak acid, $HA,$ has a $K_a$ of $1.00 \times 10^{-5}.$ If $0.100 \,mol$ of this acid is dissolved in one litreof water, the percentage of acid dissociated at equilibrium is closest to.....$\%$
The $pH$ of $0.004 \,M$ hydrazine solution is $9.7 .$ Calculate its ionization constant $K_{ b }$ and $pK _{ b }$
The hydrogen ion concentration of $0.1\,N$ solution of $C{H_3}COOH,$ which is $30\%$ dissociated, is
The solution of $N{a_2}C{O_3}$ has $pH$
Calculate $pH$ of solution of $6.0$ $gm$ acetic acid in $250$ $mL$. ( ${K_a} = 1.8 \times {10^{ - 5}}$ at $298$ $K$ ) ( $C = 12, H = 1, O = 16$ )