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.
General Chemistry - Standalone book (MindTap Course List)
11th Edition
ISBN:9781305580343
Author:Steven D. Gammon, Ebbing, Darrell Ebbing, Steven D., Darrell; Gammon, Darrell Ebbing; Steven D. Gammon, Darrell D.; Gammon, Ebbing; Steven D. Gammon; Darrell
Publisher:Steven D. Gammon, Ebbing, Darrell Ebbing, Steven D., Darrell; Gammon, Darrell Ebbing; Steven D. Gammon, Darrell D.; Gammon, Ebbing; Steven D. Gammon; Darrell
Chapter6: Thermochemisty
Section: Chapter Questions
Problem 6.109QP: A 21.3-mL sample of 0.977 M NaOH is mixed with 29.5 mL of 0.918 M HCl in a coffee-cup calorimeter...
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