S C Kheterpal, S N Dhawan and, P N Kapil Solutions for Chapter: Ionic Equilibrium in Solution, Exercise 32: PROBLEMS FOR PRACTICE

Calculate the $\mathrm{pH}$ of a solution obtained by mixing $50 \mathrm{mL}$ of $0.2 \mathrm{M} \mathrm{HCl}$ with $49.9 \mathrm{mL}$ of $0.2 \mathrm{M} \mathrm{NaOH}$ solution.

Calculate the $\mathrm{pH}$ of a solution obtained by mixing equal volumes of $\mathrm{N}/10 \mathrm{NaOH}$ and $\mathrm{N}/20 \mathrm{HCl}$.

Calculate the $\mathrm{pH}$ value of a mixture containing $50 \mathrm{mL}$ of $1 \mathrm{N} \mathrm{HCl}$ and $30 \mathrm{mL}$ of $1 \mathrm{N} \mathrm{NaOH}$ solution, assuming both to be completely dissociated.

A $50 \mathrm{mL}$ solution of $\mathrm{pH}=1$ is mixed with $50 \mathrm{mL}$ solution of $\mathrm{pH}=2$. What will be the $\mathrm{pH}$ of the mixture?

What will be the resultant $\mathrm{pH}$ when $200 \mathrm{mL}$ of an aqueous solution of $\mathrm{HCl} (\mathrm{pH} = 2.0)$ is mixed with $300 \mathrm{mL}$ of an aqueous solution of $\mathrm{NaOH} (\mathrm{pH}= 12.0)$?