Calculate the $pH$ of a mixed solution containing $10 \ mL$ of $0.2 \ M$ $Ca(OH)_2$ and $25 \ mL$ of $0.1 \ M$ $HCl$.

At $27^{\circ}C$,$100 \ mL$ of $0.4 \ M$ $HCl$ is mixed with $100 \ mL$ of $0.5 \ M$ $NaOH$ solution. To the resultant solution,$800 \ mL$ of distilled water is added. What is the $pH$ of the final solution?

If $20 \, mL$ of $0.25 \, N$ strong acid and $30 \, mL$ of $0.2 \, N$ strong base are mixed,then the resulting solution is

What is the $pH$ of a solution containing $10 \, mL$ of $0.1 \, M \, NaOH$ and $10 \, mL$ of $0.05 \, M \, H_2SO_4$?

When $100 \ mL$ of $0.1 \ M$ $NaCN$ solution is titrated with $0.1 \ M$ $HCl$ solution,the variation of $pH$ of the solution with the volume of $HCl$ added will be:

The degree of dissociation of $0.01 \ M$ solution of $NH_4OH$ is $4.2 \times 10^{-2}$. What is the percent dissociation of $NH_4OH$ (in $\%$)?