Ramendra C Mukerjee Solutions for Chapter: Ionic Equilibrium in Aqueous Solutions, Exercise 2: Objective Problems

The solubility of ${\mathrm{A}}_2{\mathrm{X}}_3$ is $\mathrm{y} \mathrm{mol} {\mathrm{dm}}^{-3}$. Its solubility product is

Which of the following statements about buffer solutions is wrong?

$10 \mathrm{mL}$ of $0.1 \mathrm{M} \mathrm{HCl}$ is titrated with $0.1 \mathrm{M} \mathrm{NaOH}$. When the volume of $\mathrm{NaOH}$ added from the burette is from $9.99 \mathrm{mL}$ to $10.01 \mathrm{mL}$, the $\mathrm{pH}$ jumps approximately from

When one drop of a concentrated $\mathrm{HCl}$ solution is added to one litre of pure water at $25°\mathrm{C}$, the $\mathrm{pH}$ drops suddenly from $7$ to about $4$. When the second drop of the same acid is added, the $\mathrm{pH}$ of the solution further drops to about

In which of the following aqueous solutions is the degree of dissociation of water maximum?

$\mathrm{pH}$ of an aqueous $1\times {10}^{-8} \mathrm{M} \mathrm{NaOH}$ solution is:

The $\mathrm{pH}$ of $1\times {10}^{-3} \mathrm{M} {\mathrm{H}}_2{\mathrm{O}}_2$ solution $\left({\mathrm{K}}_{\mathrm{a}}=2.2\times {10}^{-12}\right)$ is:

The $\mathrm{pH}$ of an aqueous solution of $0.01 \mathrm{M} {\mathrm{CH}}_3{\mathrm{COONH}}_4$ at $25 °\mathrm{C}$ is:

$\left({\mathrm{K}}_{\mathrm{a}}\left({\mathrm{CH}}_3\mathrm{COOH}\right)={\mathrm{K}}_{\mathrm{b}}\left({\mathrm{NH}}_4\mathrm{OH}\right)=1.8\times {10}^{-5}\right)$