QUESTIONS

$50 \mathrm{ml}$ of $0.1 \mathrm{M} {\mathrm{H}}_2{\mathrm{SO}}_4$ were added to $100 \mathrm{ml}$ of $0.2 \mathrm{M} {\mathrm{HNO}}_3$. Then the solution is diluted to $300 \mathrm{ml}$. What is the $\mathrm{pH}$ of the resulting solution?

Calculate ${\mathrm{K}}_{\mathrm{a}}$ of acetic acid from equilibrium concentration given below-

$\left[{\mathrm{H}}_3{\mathrm{O}}^{+}\right] = \left[\mathrm{CH}3{\mathrm{COO}}^{-}\right] =1.34 \times {10}^{-3} \mathrm{M}, \left[\mathrm{CH}3\mathrm{COOH}\right] = 9.866 \times {10}^{-2} \mathrm{M}$

${\mathrm{K}}_{\mathrm{a}}$ of $0.02 \mathrm{M} {\mathrm{CH}}_3\mathrm{COOH}$ is $1.8 \times {10}^{-5}$. Calculate $\%$ ionisation.

${\mathrm{K}}_{\mathrm{a}}$ of $0.02 \mathrm{M} {\mathrm{CH}}_3\mathrm{COOH}$ is $1.8 \times {10}^{-5}$. Calculate $\mathrm{pH}$.

The $0.005 \mathrm{M}$ monobasic acid has a $\mathrm{pH}$ of $5$. What is the extent of ionisation?

$50 \mathrm{ml}$ of $0.1\mathrm{M} {\mathrm{NH}}_4\mathrm{OH}, 25 \mathrm{ml}$ of $0.2\mathrm{M} {\mathrm{NH}}_4\mathrm{Cl}$ were used to make a buffer. What is the $\mathrm{pH}$ if ${\mathrm{pK}}_{\mathrm{b}}$ is $4.8$?

The $\mathrm{pH}$ of a buffer solution prepared by mixing $50\mathrm{ml}$ of  $0.2\mathrm{M} {\mathrm{CH}}_3\mathrm{COOH}$ and $25\mathrm{ml}$ of ${\mathrm{CH}}_3\mathrm{COONa}$ is $4.8$. What is the strength of ${\mathrm{CH}}_3\mathrm{COONa}$?$[\mathrm{pKa} \mathrm{of} {\mathrm{CH}}_3\mathrm{COOH}=4.8]$

$50 \mathrm{ml}$ of $0.1 \mathrm{M}$ sodium acetate, $25 \mathrm{ml}$ of $0.2 \mathrm{M}$ acetic acid were added together to form the buffer solution. $\mathrm{pKa}$ of ${\mathrm{CH}}_3\mathrm{COOH}$ is $4.8$. Find the $\mathrm{pH}$ of the solution.