Identify the sparingly soluble magnesium salt. They chose to identify this using Ksp determination after narrowing it down to 2 salts:

Salt	Theoretical Ksp
MgCO3	3.5 x 10-8
Mg(OH)2	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: Dont 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?