The solubility of a salt of weak acid $( A B )$ at $pH 3$ is $Y \times 10^{-3} mol L ^{-1}$. The value of $Y$ is
. . . . . (Given that the value of solubility product of $A B \left( K _{ sp }\right)=2 \times 10^{-10}$ and the value of ionization constant of $H B \left( K _{ a }\right)=1 \times 10^{-8}$ )
$4.47$
$4.48$
$4.49$
$4.50$
Calculate the $pH$ of $0.08\, M$ solution of hypochlorous acid, $HOCl$. The ionization constant of the acid is $2.5 \times 10^{-5}$ Determine the percent dissociation of $HOCl.$
The hydrogen ion concentration of a $0.006\,M$ benzoic acid solution is $({K_a} = 6 \times {10^{ - 5}})$
The hydrogen ion concentration in weak acid of dissociation constant ${K_a}$ and concentration $c$ is nearly equal to
What is polyprotic acid ? Give examples of polyprotic acid and its ionization.
Ionic product of water at $310 \,K$ is $2.7 \times 10^{-14}$. What is the $\mathrm{pH}$ of neutral water at this temperature?