When 50.00 mL of aqueous HCI was mixed with 50.00 mL of NaOH (in large excess), the temperature of the solution increased from 25.00 °C to 28.79 °C. The reaction is NaOH(aq) + HCI(aq) NaCI(aq) + H 20(aq) -- AH = -57.3 k) What was the molarity of the original HCl solution? Assume the heat capacity of the solution is the same as pure water (4.184 J/g*°C), the density of the solution is 1.00 g/mL and there is no loss of heat to the surroundings.
When 50.00 mL of aqueous HCI was mixed with 50.00 mL of NaOH (in large excess), the temperature of the solution increased from 25.00 °C to 28.79 °C. The reaction is NaOH(aq) + HCI(aq) NaCI(aq) + H 20(aq) -- AH = -57.3 k) What was the molarity of the original HCl solution? Assume the heat capacity of the solution is the same as pure water (4.184 J/g*°C), the density of the solution is 1.00 g/mL and there is no loss of heat to the surroundings.
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
Chapter6: Thermochemistry
Section: Chapter Questions
Problem 70E: Consider the reaction 2HCl(aq)+Ba(OH)2(aq)BaCl2(aq)+2H2O(l)H=118KJ Calculate the heat when 100.0 rnL...
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