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Calculate the molar solubility and solubility product of Ca(OH)2 for each trial.

Calculate the molar solubility and solubility product of Ca(OH)2 for each trial.

Chemistry: Principles and Practice
Chemistry: Principles and Practice
3rd Edition
ISBN:9780534420123
Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer
Publisher:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer
Chapter16: Reactions Between Acids And Bases
Section: Chapter Questions
Problem 16.102QE
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Calculate the molar solubility and solubility product of Ca(OH)2 for each trial. Thank you!

Concentration of standardized HCl solution (M) 0.0646 Part A Trial 1 Trial 2 Volume of sample analyzed (mL) 25.00 25.00 Initial buret reading (mL) 0.75 26.03 Final buret reading (mL) 25.80 50.40
Transcribed Image Text:Concentration of standardized HCl solution (M) 0.0646 Part A Trial 1 Trial 2 Volume of sample analyzed (mL) 25.00 25.00 Initial buret reading (mL) 0.75 26.03 Final buret reading (mL) 25.80 50.40
Prenare a clean 50 mL buret for titration. Rinse the buret and tip with three 5 mL portions of the 1. standardized 0.05 M HCI solution and discard. Fill the buret with standardized 0.05 M HCI, remove the air bubbles in the buret tip, and, after 10-15 seconds, read and record the initial volume using all certain digits (from the labeled calibration marks on the buret) plus one uncertain digit (the last digit which is the best timate between the calibration marks). Place a sheet of white paper beneath the receiving flask to make the end point of the titration easier to see. Part A- Molar Solubility and Solubility Product of Calcium Hydroxide Obtain a sample of saturated Ca(OH)2 solution (without added CaCl2) from your instructor. 2. , Pinet 25 mL of the saturated Ca(OH)2 solution into a 125 mL flask and add 2 drops of methyl orange indicator. 4 Titrate the Ca(OH)2 solution to the methyl orange endpoint, where the color changes from yellow to red. Remember, the addition of HCl should stop within one-half drop of the end point. Read and record the final volume of standard HCl in the buret. 5. Titrate an additional 25 mL aliquot of the saturated Ca(OH)2 solution. Data Analysis Calculate the molar solubility and solubility product of Ca(OH)2 for each trial and report their average values.
Transcribed Image Text:Prenare a clean 50 mL buret for titration. Rinse the buret and tip with three 5 mL portions of the 1. standardized 0.05 M HCI solution and discard. Fill the buret with standardized 0.05 M HCI, remove the air bubbles in the buret tip, and, after 10-15 seconds, read and record the initial volume using all certain digits (from the labeled calibration marks on the buret) plus one uncertain digit (the last digit which is the best timate between the calibration marks). Place a sheet of white paper beneath the receiving flask to make the end point of the titration easier to see. Part A- Molar Solubility and Solubility Product of Calcium Hydroxide Obtain a sample of saturated Ca(OH)2 solution (without added CaCl2) from your instructor. 2. , Pinet 25 mL of the saturated Ca(OH)2 solution into a 125 mL flask and add 2 drops of methyl orange indicator. 4 Titrate the Ca(OH)2 solution to the methyl orange endpoint, where the color changes from yellow to red. Remember, the addition of HCl should stop within one-half drop of the end point. Read and record the final volume of standard HCl in the buret. 5. Titrate an additional 25 mL aliquot of the saturated Ca(OH)2 solution. Data Analysis Calculate the molar solubility and solubility product of Ca(OH)2 for each trial and report their average values.
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