When \( 400 \, \text{mL} \) of \( 0.2 \, \text{M} \; \mathrm{H_2SO_4} \) solution is mixed with \( 600 \, \text{mL} \) of \( 0.1 \, \text{M} \; \mathrm{NaOH} \) solution, the increase in temperature of the final solution is ____________ \( \times 10^{-2} \) \( \text{K} \). (Round off to the Nearest Integer)
[Use : \( \mathrm{H^+ (aq)} + \mathrm{OH^- (aq)} \rightarrow \mathrm{H_2O} ; \; \Delta_\gamma H = -57.1 \, \text{kJ mol}^{-1} \)
Specific heat of \( \mathrm{H_2O} = 4.18 \, \text{J K}^{-1} \text{ g}^{-1} \)
Density of \( \mathrm{H_2O} = 1.0 \, \text{g cm}^{-3} \)
Assume no change in volume of solution on mixing.]
