Chapter 9, Problem 52E

In a coffee cup calorimeter, $\text{100}\text{.0 mL}$ of $\text{1}\text{.0 M NaOH}$ and $\text{100}\text{.0 mL}$ of $\text{1}\text{.0 M HCl}$ are mixed. Both solutions were origniallyat $\text{24}\text{.6°C}$ . After the reaction, the final temperature is $\text{31}\text{.3°C}$ . Assuming that all the solutions have a density of $\text{1}{\text{.0 g/cm}}^{\text{3}}$ and a specific heat capacity of $\text{4}\text{.18 J}{\text{°C}}^{\text{-1}}{\text{ g}}^{\text{-1}}$ , calculate the enthalpy change for the neutralization of $\text{HCl}$ by $\text{NaOH}$ . Assume that no heat is lost to the surroundings or to the calorimeter.