Consider the dissolution of \(\mathrm{CaCl}_{2}\) :

\[\mathrm{CaCl}_{2}(s) \longrightarrow \mathrm{Ca}^{2+}(a q)+2 \mathrm{Cl}^{-}(a q) \quad \Delta H=-81.5 \mathrm{~kJ}\]

An 11.0-g sample of \(\mathrm{CaCl}_{2}\) is dissolved in \(125 \mathrm{~g}\) of water, with both substances at \(25.0^{\circ} \mathrm{C}\). Calculate the final temperature of the solution assuming no heat loss to the surroundings and assuming the solution has a specific heat capacity of \(4.18 \mathrm{~J}^{\circ} \mathrm{C}^{-1} \mathrm{~g}^{-1}\).