200   mL of 0 . 2   M   HCl is mixed with 300   mL of 0 . 1   M   NaOH . The…

$200 \mathrm{mL}$ of $0.2 \mathrm{M} \mathrm{HCl}$ is mixed with $300 \mathrm{mL}$ of $0.1 \mathrm{M} \mathrm{NaOH}.$ The molar heat of neutralization of this reaction is $-57.1 \mathrm{kJ}.$ The increase in temperature in ${}^{\circ }\mathrm{C}$ of the system on mixing is $\mathrm{x}\times {10}^{-2}.$ The value of $\mathrm{x}$ is (Nearest integer)

[Given: Specific heat of water $=4.18 \mathrm{J} {\mathrm{g}}^{-1} {\mathrm{K}}^{-1}$ 

Density of water$=1.00 \mathrm{g}{ \mathrm{cm}}^{-3}$]

(Assume no volume change on mixing)