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A student tries to calculate the enthalpy of reaction for an acid-base reaction. 1.0 M HBr and 1.0 M KOH is used for the reaction shown below. Which of the following mistakes would cause the smallest deviation from the true value? O The final temperature of the mixture was taken before the contents of the calorimeter had reached thermal equilibrium. O The actual molarity of the base solution was 1.1 M but was recorded as 1.0 M. O The thermometer was incorrectly calibrated and read 2.0 Celsius degree too high during the procedure. O The volume of the acid solution added to the calorimeter was actually 0.5 mL less than what was recorded. The calorimeter was poorly insulated, and some heat escaped to the atmosphere during the procedure.

A student tries to calculate the enthalpy of reaction for an acid-base reaction. 1.0 M HBr and 1.0 M KOH is used for the reaction shown below. Which of the following mistakes would cause the smallest deviation from the true value? O The final temperature of the mixture was taken before the contents of the calorimeter had reached thermal equilibrium. O The actual molarity of the base solution was 1.1 M but was recorded as 1.0 M. O The thermometer was incorrectly calibrated and read 2.0 Celsius degree too high during the procedure. O The volume of the acid solution added to the calorimeter was actually 0.5 mL less than what was recorded. The calorimeter was poorly insulated, and some heat escaped to the atmosphere during the procedure.

Introductory Chemistry: A Foundation
Introductory Chemistry: A Foundation
9th Edition
ISBN:9781337399425
Author:Steven S. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Donald J. DeCoste
Chapter15: Solutions
Section: Chapter Questions
Problem 68QAP: 68. Aluminum ion may be precipitated from aqueous solution by addition of hydroxide ion, forming...
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A student tries to calculate the enthalpy of reaction for an acid-base reaction. 1.0 M HBr and 1.0 M KOH is used for the reaction shown below. Which of the following mistakes would cause the smallest deviation from the true value? The final temperature of the mixture was taken before the contents of the calorimeter had reached thermal equilibrium. The actual molarity of the base solution was 1.1 M but was recorded as 1.0 M. The thermometer was incorrectly calibrated and read 2.0 Celsius degree too high during the procedure. The volume of the acid solution added to the calorimeter was actually 0.5 mL less than what was recorded. The calorimeter was poorly insulated, and some heat escaped to the atmosphere during the procedure.
Transcribed Image Text:A student tries to calculate the enthalpy of reaction for an acid-base reaction. 1.0 M HBr and 1.0 M KOH is used for the reaction shown below. Which of the following mistakes would cause the smallest deviation from the true value? The final temperature of the mixture was taken before the contents of the calorimeter had reached thermal equilibrium. The actual molarity of the base solution was 1.1 M but was recorded as 1.0 M. The thermometer was incorrectly calibrated and read 2.0 Celsius degree too high during the procedure. The volume of the acid solution added to the calorimeter was actually 0.5 mL less than what was recorded. The calorimeter was poorly insulated, and some heat escaped to the atmosphere during the procedure.
A student conducted a precipitation experiment for Mg(OH)2 (s) by mixing 250 mL of 0.5 M MgCl2 (aq) and a 250 mL of 1.0 M NaOH (aq). If the student wants to repeat the experiment to produce the same final volume but double the amount of precipitate produced, which of the following changes should they make to the procedure? MgCl2 (aq) + 2 NaOH (aq) → 2 NaCI (aq) + Mg(OH)2 (s) O Using twice the molarity of MgCl2 (aq) and twice the molarity of NaOH (aq) Using the same molarity of MgCl2 (aq) but twice the molarity of NaOH (aq) O Using twice the molarity of MgCl2 (aq) but the same molarity of NaOH (aq) Using twice the molarity of MgCl2 (aq) but half the molarity of NaOH (aq)
Transcribed Image Text:A student conducted a precipitation experiment for Mg(OH)2 (s) by mixing 250 mL of 0.5 M MgCl2 (aq) and a 250 mL of 1.0 M NaOH (aq). If the student wants to repeat the experiment to produce the same final volume but double the amount of precipitate produced, which of the following changes should they make to the procedure? MgCl2 (aq) + 2 NaOH (aq) → 2 NaCI (aq) + Mg(OH)2 (s) O Using twice the molarity of MgCl2 (aq) and twice the molarity of NaOH (aq) Using the same molarity of MgCl2 (aq) but twice the molarity of NaOH (aq) O Using twice the molarity of MgCl2 (aq) but the same molarity of NaOH (aq) Using twice the molarity of MgCl2 (aq) but half the molarity of NaOH (aq)
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