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1. During the analyte preparation, if some of the solid precipitate of Ca(OH), is inadvertently transferred along with the supernatant liquid to the flask: Will more, less, or the same amount of the HCl be needed to perform the titration? Explain. a. b. What effect will this have on the calculated molar solubility compared to the actual value for Ca(OH),? Explain. C. What effect will this have on the calculated solubility product constant (K) compared to the actual value of Ca(OH),? Explain.

1. During the analyte preparation, if some of the solid precipitate of Ca(OH), is inadvertently transferred along with the supernatant liquid to the flask: Will more, less, or the same amount of the HCl be needed to perform the titration? Explain. a. b. What effect will this have on the calculated molar solubility compared to the actual value for Ca(OH),? Explain. C. What effect will this have on the calculated solubility product constant (K) compared to the actual value of Ca(OH),? Explain.

Chemistry: Principles and Reactions
Chemistry: Principles and Reactions
8th Edition
ISBN:9781305079373
Author:William L. Masterton, Cecile N. Hurley
Publisher:William L. Masterton, Cecile N. Hurley
Chapter14: Equilibria In Acid-base Solutions
Section: Chapter Questions
Problem 47QAP: A 0.4000 M solution of nitric acid is used to titrate 50.00 mL of 0.237 M barium hydroxide. (Assume...
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Name EXPERIMENT 11 DETERMINATION OF MOLAR SOLUBILITY 1 Volume of saturated Ca(OH), solution (mL) Volume of saturated Ca(OH), solution (L) Concentration of standardized HCI solution (mol/L) Initial buret reading (mL) 2 A. TITRATION TO DETERMINE THE MOLAR SOLUBILITY AND SOLUBILITY PRODUCT, KP OF CALCIUM HYDROXIDE 3 4 5 6 Volume of HCI added (mL) 7 8 Final buret reading (mL) 13 Date Volume of HCI added (L) 14 K of Ca(OH), 15 Average K of Ca(OH)," Trial 1 25.0 mL Instructor Report Sheet 0.05 M 0.0 0.0 20.6 20.7 20.6 20.7 0.0206 0.0207 Moles of HCI added (mol) 103x103 1.03X10-3 -3 9 Moles of OH-in saturated solution (mol) 1,03 x 10³ 103 X 10-3 MON-OH 10 [OH-], equilibrium (mol/L) 0.0412m 0.0414m 11 [Ca2+], equilibrium (mol/L) 0.0206 0.0207 12 Molar solubility of Ca(OH), (mol/L) 0.0206m 0.0207 Average molar solubility of Ca(OH)₂ (mol/L) 0.02065 0.02065 -S 3.50x10 3.5x10 3.52x10-5 3.52x10-5 Trial 2 25.0 mL 0.025 0.025 L 0.05 M Trial 3 mb) 25.0 mL 0.05 M Hol DETERMINATION OF MOLAR SOLUBILITY 129
Transcribed Image Text:Name EXPERIMENT 11 DETERMINATION OF MOLAR SOLUBILITY 1 Volume of saturated Ca(OH), solution (mL) Volume of saturated Ca(OH), solution (L) Concentration of standardized HCI solution (mol/L) Initial buret reading (mL) 2 A. TITRATION TO DETERMINE THE MOLAR SOLUBILITY AND SOLUBILITY PRODUCT, KP OF CALCIUM HYDROXIDE 3 4 5 6 Volume of HCI added (mL) 7 8 Final buret reading (mL) 13 Date Volume of HCI added (L) 14 K of Ca(OH), 15 Average K of Ca(OH)," Trial 1 25.0 mL Instructor Report Sheet 0.05 M 0.0 0.0 20.6 20.7 20.6 20.7 0.0206 0.0207 Moles of HCI added (mol) 103x103 1.03X10-3 -3 9 Moles of OH-in saturated solution (mol) 1,03 x 10³ 103 X 10-3 MON-OH 10 [OH-], equilibrium (mol/L) 0.0412m 0.0414m 11 [Ca2+], equilibrium (mol/L) 0.0206 0.0207 12 Molar solubility of Ca(OH), (mol/L) 0.0206m 0.0207 Average molar solubility of Ca(OH)₂ (mol/L) 0.02065 0.02065 -S 3.50x10 3.5x10 3.52x10-5 3.52x10-5 Trial 2 25.0 mL 0.025 0.025 L 0.05 M Trial 3 mb) 25.0 mL 0.05 M Hol DETERMINATION OF MOLAR SOLUBILITY 129
Name EXPERIMENT 11 DETERMINATION OF MOLAR SOLUBILITY Date ECTROCHEMI Post-Laboratory Questions 1. During the analyte preparation, if some of the solid precipitate of Ca(OH), is inadvertently transferred along with the supernatant liquid to the flask: Will more, less, or the same amount of the HCl be needed to perform the titration? Explain. Instructor, a. b. b. What effect will this have on the calculated molar solubility compared to the actual value for Ca(OH)₂? Explain. c. What effect will this have on the calculated solubility product constant (K) compared to the actual value of Ca(OH),? Explain. 2. If the end point was surpassed and a dark orange color produced before the titration was stopped, will the molar solubility calculated be higher or lower than the actual value for Ca(OH),? Explain. 3. A student forgot to record the actual molar concentration of the HCl and so used the 0.05 M value given in the procedure to perform the calculations and arrived at a molar solubility of 0.0112 M. If the acid was actually 0.045 M HCl: What is the correct molar solubility? What is the student's percent error? DETERMINATION OF MOLAR SOLUBILITY 131
Transcribed Image Text:Name EXPERIMENT 11 DETERMINATION OF MOLAR SOLUBILITY Date ECTROCHEMI Post-Laboratory Questions 1. During the analyte preparation, if some of the solid precipitate of Ca(OH), is inadvertently transferred along with the supernatant liquid to the flask: Will more, less, or the same amount of the HCl be needed to perform the titration? Explain. Instructor, a. b. b. What effect will this have on the calculated molar solubility compared to the actual value for Ca(OH)₂? Explain. c. What effect will this have on the calculated solubility product constant (K) compared to the actual value of Ca(OH),? Explain. 2. If the end point was surpassed and a dark orange color produced before the titration was stopped, will the molar solubility calculated be higher or lower than the actual value for Ca(OH),? Explain. 3. A student forgot to record the actual molar concentration of the HCl and so used the 0.05 M value given in the procedure to perform the calculations and arrived at a molar solubility of 0.0112 M. If the acid was actually 0.045 M HCl: What is the correct molar solubility? What is the student's percent error? DETERMINATION OF MOLAR SOLUBILITY 131
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