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2. Calculate the molar solubility of lead(II) phosphate in a pH 10 solution. Ksp = 1.0 x 10-54 Kf = 8.0 x 1013 Pb3(PO4)2(s) 3 Pb²+ (aq) + 2 PO4³- (aq) Pb²+ (aq) + 3 OH(aq) Pb(OH)3 (aq) Pb3(PO4)2(s) + 9 OH (aq) 3 Pb(OH)3 (aq) + 2 PO4³- (aq)

2. Calculate the molar solubility of lead(II) phosphate in a pH 10 solution. Ksp = 1.0 x 10-54 Kf = 8.0 x 1013 Pb3(PO4)2(s) 3 Pb²+ (aq) + 2 PO4³- (aq) Pb²+ (aq) + 3 OH(aq) Pb(OH)3 (aq) Pb3(PO4)2(s) + 9 OH (aq) 3 Pb(OH)3 (aq) + 2 PO4³- (aq)

Chemistry for Engineering Students
Chemistry for Engineering Students
4th Edition
ISBN:9781337398909
Author:Lawrence S. Brown, Tom Holme
Publisher:Lawrence S. Brown, Tom Holme
Chapter12: Chemical Equilibrium
Section: Chapter Questions
Problem 12.88PAE: Which of the following is more likely to precipitate the hydroxide ion? Cu(OH)2(s) *=» Ctr+(aq) + 2...
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2. Calculate the molar solubility of lead(II) phosphate in a pH 10 solution. Pb3(PO4)2(s) 3 Pb²+ (aq) + 2 PO4³- (aq) Pb²+ (aq) + 3 OH(aq) Pb(OH)3(aq) Ksp = 1.0 x 10-54 Kf = 8.0 x 1013 Pb3(PO4)2(s) + 9 OH(aq) 3 Pb(OH)3 (aq) + 2 PO4³- (aq)
Transcribed Image Text:2. Calculate the molar solubility of lead(II) phosphate in a pH 10 solution. Pb3(PO4)2(s) 3 Pb²+ (aq) + 2 PO4³- (aq) Pb²+ (aq) + 3 OH(aq) Pb(OH)3(aq) Ksp = 1.0 x 10-54 Kf = 8.0 x 1013 Pb3(PO4)2(s) + 9 OH(aq) 3 Pb(OH)3 (aq) + 2 PO4³- (aq)
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