When 400 mL of $0.2 \mathrm{M} \mathrm{H}_2 \mathrm{SO}_4$ solution is mixed with 600 mL of 0.1 M NaOH solution, the increase in temperature of the final solution is $\_\_\_\_$ $\times 10^{-2} \mathrm{~K}$. (Round off to the nearest integer).
[Use: $\mathrm{H}^{+}(\mathrm{aq})+\mathrm{OH}-(\mathrm{aq}) \rightarrow \mathrm{H}_2 \mathrm{O}$.
$$
\left.\Delta \gamma \mathrm{H}=-57.1 \mathrm{~kJ} \mathrm{~mol}^{-1}\right]
$$
Specific heat of $\mathrm{H}_2 \mathrm{O}=4.18 \mathrm{~J} \mathrm{~K}^{-1} \mathrm{~g}^{-1}$
density of $\mathrm{H}_2 \mathrm{O}=1.0 \mathrm{~g} \mathrm{~cm}^{-3}$
Assume no change in volume of solution on mixing.
