# 50.0mL of a solution of HCl is combined with 100.0mL of 1.15 M NaOH in a calorimeter. The reaction mixture is initially at 22.4 degrees C and the final temperature after reaction is 31.2 degrees C. What is the molarity of the HCl solution? ( Assume that there is an excess of base (so all of the HCl has reacted), that the specific heat of the reaction mixture is 0.96 cal/g degrees C, and that the density of the reaction mixture is 1.02 g/mL. The heat of neutralization of HCl and NaOH is 13.6 kcal/mol.)

Question

50.0mL of a solution of HCl is combined with 100.0mL of 1.15 M NaOH in a calorimeter. The reaction mixture is initially at 22.4 degrees C and the final temperature after reaction is 31.2 degrees C. What is the molarity of the HCl solution? ( Assume that there is an excess of base (so all of the HCl has reacted), that the specific heat of the reaction mixture is 0.96 cal/g degrees C, and that the density of the reaction mixture is 1.02 g/mL. The heat of neutralization of HCl and NaOH is 13.6 kcal/mol.)

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Step 1

First calculate the number of moles of HCl reacted with NaOH so that we can easily calculate the concentration of HCl.

Given reaction,

Step 2

Calculate the value of heat of reaction (q) using the given values

Step 3

When one mole of HCl reacts with one mole of NaOH, it will liberate 13600 calories. But, only 1293 calories were liberated in the given reaction ...

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### Chemical Thermodynamics 