Two solutions, initially at , were mixed in an insulated bottle. One contained 200 ml of 0.4 M weak — Thermodynamics and Thermochemistry Chemistry Question

Question

Two solutions, initially at $25^\circ\text{C}$, were mixed in an insulated bottle. One contained 200 ml of 0.4 M weak monoprotic acid solution. The other contained 100 ml of a solution having 0.5 mole NaOH per litre. After mixing, the temperature rose to $26^\circ\text{C}$. Assume that the densities of both the solutions are 1.0 g/ml and that their specific heat capacities are all 1.0 cal/g-K. The amount of heat evolved (in kcal) in the neutralization of 1 mole of the acid is