Use the concept of calorimetry to determine the heat of neutralization between KOH and HNO_{3}

For this problem, follow the steps:

1. Determine the total mass of solution

2. Calculate change in temperature

3. Determine the amount of heat released

4. Calculate the heat of enthalpy

The *neutralization reaction* of KOH_{(aq)} and HNO_{3(aq)} is

**KOH _{(aq)} + HNO_{3(aq)} → KNO_{3(aq)} + H_{2}O**

A 100.0-mL sample of 0.662 M KOH is mixed with a 100.0-mL sample of 0.662 M HNO_{3} in a coffee cup calorimeter. If both solutions were initially at 30.64°C and the temperature of the resulting solution was recorded as 35.15°C, determine the ΔH°_{rxn} for the neutralization reaction between aqueous KOH and HNO_{3}. Assume that no heat is lost to the calorimeter or the surroundings, and that the density and the heat capacity of the resulting solution are 1.00 g/mL and 4.18 J/(g°C), respectively.

A) -27.9 kJ

B) -57.0 kJ

C) -16.7 kJ

D) - 34.4 kJ

E) -169 kJ

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