You mix $125mL$ of $0\mathrm{.}190M$

CsOH with $50\mathrm{.}0mL$ of $0\mathrm{.}475M$

HF in a coffee$-$cup calorimeter, and the temperature of both solutions rises from $21\mathrm{.}50C$ before mixing to $23\mathrm{.}70C$ after the reaction.

CsOH$(aq)+HF(aq)CsF(aq)+H_{2}O(l)$

What is the enthalpy of reaction per mole of CsOH $?$ Assume the densities of the solutions are all $1\mathrm{.}00\frac{g}{m}L,$ and the specific heat capacities of the solutions are $4\mathrm{.}2\frac{J}{g}*K.$

Enthalpy of reaction $=k\frac{J}{m}ol$