100 ml of 0.1 M $C{H}_{3}COOH$ is mixed with 50 ml of 0.1 M $NaOH$ solution and pH of the resulting solution is 5. The change in pH if 100 ml of 0.05 M $NaOH$ is added in the above solution is:

The correct option is D 3.8
A mixture containing 100 ml of 0.1 M acetic acid and 50 ml of 0.1 M NaOH is acidic buffer soluion. Its pH is given by the expression $pH=p{K}_a+log\frac{salt}{acid}$.
Substitute values in the above expression.
$5=p{K}_a+log\frac{0.1\times 0.05}{0.1\times 0.05}$ or $p{K}_a=5$.
When 100 ml of 0.05 M NaOH is added, the acid is completely neutralized and the solution contains salt sodium acetate.
The expression for the hydrogen ion concentration of the salt of weak acid and strong base is $pH=\frac{1}{2}(p{K}_w+p{K}_a+logc)$.
Substitute values in the above expression.
$pH=\frac{1}{2}(14+5+log(\frac{0.1}{0.25}\left)\right)=8.8$.
Hence, the change in pH is $\Delta pH=8.8-5=3.8$.