You add an excess of Ca(OH) 2 to water maintained at a particular temperature, s
ID: 631722 • Letter: Y
Question
You add an excess of Ca(OH)2to 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 of25mL of the calcium hydroxide solution to the endpoint requires10.63mL of 0.080M HCl solution. Part A What is the millimolar quantiy of OH?in the25mL of solution?Part B What are the concentrations of Ca2+and OH??
Part C What is the solubility of Ca(OH)2under these conditions? (Expressed as g/dL). Give your answer to three significant figures.
Part D What is the Kspfor Ca(OH)2under these conditions?
You add an excess of Ca(OH)2to 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 of25mL of the calcium hydroxide solution to the endpoint requires10.63mL of 0.080M HCl solution. Part A What is the millimolar quantiy of OH?in the25mL of solution?
Part A What is the millimolar quantiy of OH?in the25mL of solution?
Part B What are the concentrations of Ca2+and OH??
Part B What are the concentrations of Ca2+and OH??
Part C What is the solubility of Ca(OH)2under these conditions? (Expressed as g/dL). Give your answer to three significant figures.
Part C What is the solubility of Ca(OH)2under these conditions? (Expressed as g/dL). Give your answer to three significant figures.
Part D What is the Kspfor Ca(OH)2under these conditions?
Part D What is the Kspfor Ca(OH)2under these conditions?
Explanation / Answer
10.63*0.08 = 2*25*M
M = 0.017 M Ca(OH)2
(a) OH- = 2*0.017*25 = 0.8504 miliMoles of OH-
(b) [Ca2+] = 0.017 M
[OH-] = 0.034 M
(c) solubility = 74*0.017 = 1.258 g/L
(d) Ksp = [Ca]*[OH-]^2 = 0.017*0.034^2 = 1.965E-5.
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