5. A water supply company, One Team, found out that their water supply had been contaminated with a sparingly soluble magnesium salt. They requested the help of Magent Analytical Laboratory to identify the magnesium salt. They chose to identify this using Ksp determination after narrowing it down to 2 salts: Salt MgCO3 Mg(OH)2 Theoretical Ksp 3.5 x 10-8 1.8 x 10-11 For the standardization of the HCl titrant, 5.230 mg Na2CO3 (98.9% purity, MW = 105.99 g/mol) required 24.4 mL of the titrant to reach the phenolphthalein endpoint. After isolating and precipitating the magnesium salt A, a portion was dissolved in distilled water in order to make a 250.0-mL saturated solution. The titration of a 50.0-mL aliquot of the saturated solution required 8.20 mL of HCl titrant to reach the phenolphthalein endpoint. Meanwhile, dissolving this magnesium salt in 250.0 mL of 0.0200 M MgCl2 required 1.51 mL of the same HCl titrant to titrate a 100.0-mL solution. a. What is the molarity of the HCl titrant? b. Comparing the data in distilled water with the two possible solids, which is the most likely identity of the magnesium salt? Show your full solutions in getting your conclusion. Note: Don't forget to factor in stoichiometry c. What is the average experimental Ksp for both solvents (distilled water and 0.0200 M MgCl2) and individual solubility in each solvent of the magnesium salt?
5. A water supply company, One Team, found out that their water supply had been contaminated with a sparingly soluble magnesium salt. They requested the help of Magent Analytical Laboratory to identify the magnesium salt. They chose to identify this using Ksp determination after narrowing it down to 2 salts: Salt MgCO3 Mg(OH)2 Theoretical Ksp 3.5 x 10-8 1.8 x 10-11 For the standardization of the HCl titrant, 5.230 mg Na2CO3 (98.9% purity, MW = 105.99 g/mol) required 24.4 mL of the titrant to reach the phenolphthalein endpoint. After isolating and precipitating the magnesium salt A, a portion was dissolved in distilled water in order to make a 250.0-mL saturated solution. The titration of a 50.0-mL aliquot of the saturated solution required 8.20 mL of HCl titrant to reach the phenolphthalein endpoint. Meanwhile, dissolving this magnesium salt in 250.0 mL of 0.0200 M MgCl2 required 1.51 mL of the same HCl titrant to titrate a 100.0-mL solution. a. What is the molarity of the HCl titrant? b. Comparing the data in distilled water with the two possible solids, which is the most likely identity of the magnesium salt? Show your full solutions in getting your conclusion. Note: Don't forget to factor in stoichiometry c. What is the average experimental Ksp for both solvents (distilled water and 0.0200 M MgCl2) and individual solubility in each solvent of the magnesium salt?
Chemistry: The Molecular Science
5th Edition
ISBN:9781285199047
Author:John W. Moore, Conrad L. Stanitski
Publisher:John W. Moore, Conrad L. Stanitski
Chapter15: Additional Aqueous Equilibria
Section: Chapter Questions
Problem 15.BCP
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Transcribed Image Text:5. A water supply company, One Team, found out that their water supply had been
contaminated with a sparingly soluble magnesium salt. They requested the help of
Magent Analytical Laboratory to identify the magnesium salt. They chose to identify this
using Ksp determination after narrowing it down to 2 salts:
Salt
MgCO3
Mg(OH)2
Theoretical Ksp
3.5 x 10-8
1.8 x 10-11
For the standardization of the HCl titrant, 5.230 mg Na2CO3 (98.9% purity, MW = 105.99
g/mol) required 24.4 mL of the titrant to reach the phenolphthalein endpoint.
After isolating and precipitating the magnesium salt A, a portion was dissolved in distilled
water in order to make a 250.0-mL saturated solution. The titration of a 50.0-mL aliquot
of the saturated solution required 8.20 mL of HCl titrant to reach the phenolphthalein
endpoint.
Meanwhile, dissolving this magnesium salt in 250.0 mL of 0.0200 M MgCl2 required 1.51
mL of the same HCl titrant to titrate a 100.0-mL solution.
a. What is the molarity of the HCl titrant?
b. Comparing the data in distilled water with the two possible solids, which is the most
likely identity of the magnesium salt? Show your full solutions in getting your
conclusion.
Note: Don't forget to factor in stoichiometry
c.
What is the average experimental Ksp for both solvents (distilled water and 0.0200
M MgCl2) and individual solubility in each solvent of the magnesium salt?
d. What is the percent error in the obtained Ksp value?
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