A student dissolves \(2.00\text{ g}\) of \(\text{NaOH(s)}\) (molar mass \(40.0\text{ g/mol}\)) in \(98.0\text{ g}\) of distilled water in an insulated coffee-cup calorimeter. The temperature of the mixture increases from \(21.0\text{ }^\circ\text{C}\) to \(26.0\text{ }^\circ\text{C}\). Assume the specific heat capacity of the resulting solution is \(4.18\text{ J}/(\text{g}\cdot^\circ\text{C})\), the calorimeter absorbs negligible heat, and no heat is lost to the surroundings. Based on these data, what is the molar enthalpy of dissolution, \(\Delta H^\circ_{\text{soln}}\), of \(\text{NaOH(s)}\) in water?