Chemistry - Ionic Equilibrium Question with Solution | TestHub

At pH$=3,\left[{\mathrm{H}}^{+}\right]=10^{-3}\mathrm{M}$
At pH$=4,\left[{\mathrm{H}}^{+}\right]=10^{-4}\mathrm{M}$
When in equal volume of the two solutions are mixed, the$\left[{\mathrm{H}}^{+}\right]$
$=\frac{10^{-3}+10^{-4}}{2}=\frac{10^{-3}[1+0.1]}{2}=\frac{1.1}{2}\times 10^{-3}$
$\left[{\mathrm{H}}^{+}\right]=5.5\times 10^{-4}$
$-\mathrm{l}\mathrm{o}\mathrm{g}\left[{\mathrm{H}}^{+}\right]=-\mathrm{l}\mathrm{o}\mathrm{g}\left(5.5\right)-\mathrm{l}\mathrm{o}\mathrm{g}10^{-4}$
pH$=-0.74+4=3.26$