The heat of neutralization between an acid and a base was detemined using a coffee cup calorimeter with negligible contribution to the heat capacity. The aqueous solutions of the acid and base both registered an initial temperature of 28.0°C. Following the calorimetric procedure, 100 mL each of the two solutions with the same concentration were mixed in the calorimeter. After mixing, the temperature increased to 34.6°C. Assuming that the total volume of the mixture is also the volume of the water in the calorimeter and that the density of water is 1.00 g/mL, calculate the heat of neutralization of the process.

The heat of neutralization between an acid and a base was detemined using a coffee cup calorimeter with negligible contribution to the heat capacity. The aqueous solutions of the acid and base both registered an initial temperature of 28.0°C. Following the calorimetric procedure, 100 mL each of the two solutions with the same concentration were mixed in the calorimeter. After mixing, the temperature increased to 34.6°C. Assuming that the total volume of the mixture is also the volume of the water in the calorimeter and that the density of water is 1.00 g/mL, calculate the heat of neutralization of the process.

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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