S C Kheterpal, S N Dhawan and, P N Kapil Solutions for Chapter: Ionic Equilibrium in Solution, Exercise 43: Competition Focus

A solution containing ${\mathrm{Na}}_2{\mathrm{CO}}_3$ and $\mathrm{NaOH}$ requires $300 \mathrm{mL}$ of $0.1 \mathrm{N} \mathrm{HCl}$ using phenolphthalein as an indicator. Methyl orange is then added to above titrated solution when a further $25 \mathrm{ML}$ of $0.2 \mathrm{M}$ $\mathrm{HCl}$ is  required. The amount of $\mathrm{NaOH}$ present in the original solution is 

$50 {\mathrm{cm}}^3$ of $0.2 \mathrm{N}$ $\mathrm{HCl}$ is titrated against $0.1 \mathrm{N} \mathrm{NaOH}$ solution. The titration is discontinued after adding $50 {\mathrm{cm}}^3$ of $\mathrm{NaOH}$. The remaining titration is completed by adding $0.5 \mathrm{N} \mathrm{KOH}$. The volume of $\mathrm{KOH}$ required for completing the titration is 

$20.0 \mathrm{L}$ of $0.2 \mathrm{M}$ weak acid $({\mathrm{pK}}_{\mathrm{a}}=5.0)$ is titrated against $0.2 \mathrm{M}$ strong base. What is the $\mathrm{pH}$ at the equivalence point ?

The rapid change of $\mathrm{pH}$ near the stoichiometric point of an acid-base titration is the basis of indicator detection. $\mathrm{pH}$ of the solution is related to ratio of concentration of conjugate acid $\left({\mathrm{HI}}_{\mathrm{n}}\right)$ and the base $\left({{\mathrm{I}}_{\mathrm{n}}}^{-}\right)$ forms of the indicator by the expression 

An alkali is titrated against an acid with methyl orange as indicator, which of the following is a correct combination?

Among the following hydroxides, the one which has the lowest value of ${\mathrm{K}}_{\mathrm{sp}}$ at ordinary temperature $($about ${25}^{\circ }\mathrm{C}$) is 

The solubility of $\mathrm{AgCl} \left(\mathrm{s}\right)$ with solubility product $1.6\times {10}^{-10}$ in $0.1 \mathrm{M} \mathrm{NaCl}$ solution would be

The solubility product of $\mathrm{AgCl}$ is $4.0\times {10}^{-10}$ at $298 \mathrm{K}$. The solubility of $\mathrm{AgCl}$ in $0.04 \mathrm{M}$ ${\mathrm{CaCl}}_2$ will be