What is the $pH$ of the resulting solution when equal volumes of $0.1MNaOH$ and $0.01MHCl$ are mixed?

Key Concept - When equal volumes of acid and base are mixed, then resulting solution become alkaline if concentration of base is taken high. Let normality of the solution after mixing 0.1 M NaOH and 0.01 M HCl is N.
$\therefore N_1{V}_1-N_2{V}_2=NV$
or $0.1\times 1-0.01\times 1=N\times 2$
Since, normality of NaOH is more than that of HCl. Hence, the resulting solution is alkaline.
or $\left[\stackrel{-}{O}H\right]=N=\frac{0.09}{2}=0.045N$
or $pOH=-\log \left(0.045\right)=1.35$
$\therefore pH=14-pOH=14-1.35=12.65$