Chapter 6, Problem 98RQ

A dilute solution of hydrochloric acid with a mass of 610.29 g and containing 0.33183 mol of HCl was exactly neutralized in a calorimeter by the sodium hydroxide in 615.31 g of a comparably dilute solution. The temperature increased from 16.784 to $\text{20}\text{.610 °C}$. The specific heat of the HCl solution was 4.031 ${\text{J g}}^{\text{-1}}{\text{°C}}^{\text{-1}}$

; that of the NaOH solution was $\text{4}{\text{.046 J g}}^{\text{-1}}{\text{ °C}}^{\text{-1}}$. The heat capacity of the calorimeter was $\text{77}{\text{.99 J °C}}^{\text{-1}}$. Write the balanced equation for the reaction. Use the data above to calculate the heat evolved. What is the heat of neutralization per mole of HCl? Assume that the original solutions made independent contributions to the total heat capacity of the system following their mixing.