You add an excess of Ca(OH)2 to water maintained at a particular temperature, st

Question

You add an excess of Ca(OH)2 to water maintained at a particular temperature, stir until the solution is saturated, filter, then determine the [OH-] in the solution by titration with acid. Titration of 10.0 mL of the calcium hydroxide solution to the endpoint requires 4.86 mL of 0.070 M HCl solution.

-What is the molar quantity of OH- in the 10.0 mL of solution?

-What are the concentrations of Ca 2+ and OH-?

-What is the solubility of Ca(OH)2 under these conditions?

-What is the Ksp for Ca(OH)2 under these conditions?

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Explanation / Answer

a) Moles of OH- = 2* moles of H+ consumed = 2*4.86ml * .070M = 0.6804 mili Moles

b) [Ca+] = [OH-] = 0.6804mili moles/10 mL = 0.06804 M

c) Ca(OH)2 is sparingly soluble in water with solubility = 0.06804 moles per liter

d) Ksp = [Ca+2][OH-]^2 = 0.06804^3 = 3.15e-4

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