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

Frequently Asked Questions

What scientific concept do you need to know in order to solve this problem?

Our tutors have indicated that to solve this problem you will need to apply the Calorimetry concept. You can view video lessons to learn Calorimetry. Or if you need more Calorimetry practice, you can also practice Calorimetry practice problems.

What is the difficulty of this problem?

Our tutors rated the difficulty of*A 100.0-mL sample of 0.662 M KOH is mixed with a 100.0-mL sa...*as high difficulty.