A saturated solution of lead iodate in pure water has a lead ion concentration of 4.0×10³ mole liter at 25°C. per (a) Calculate the value for the solubility-product constant of Pb(IO3)2 at 25°C. (b) Calculate the molar solubility of Pb(IO3)2 in a 0.10 molar Pb(NO3): solution at 25°C. (c) To 333 milliliters of a 0.120-molar Ph(NO), solution, 667 milliliters of 0.435-molar KIO; is added. Calculate the concentrations of Pb and IO in the solution at equilibrium at 25°C.
A saturated solution of lead iodate in pure water has a lead ion concentration of 4.0×10³ mole liter at 25°C. per (a) Calculate the value for the solubility-product constant of Pb(IO3)2 at 25°C. (b) Calculate the molar solubility of Pb(IO3)2 in a 0.10 molar Pb(NO3): solution at 25°C. (c) To 333 milliliters of a 0.120-molar Ph(NO), solution, 667 milliliters of 0.435-molar KIO; is added. Calculate the concentrations of Pb and IO in the solution at equilibrium at 25°C.
Chemistry by OpenStax (2015-05-04)
1st Edition
ISBN:9781938168390
Author:Klaus Theopold, Richard H Langley, Paul Flowers, William R. Robinson, Mark Blaser
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Chapter15: Equilibria Of Other Reaction Classes
Section: Chapter Questions
Problem 84E: A saturated solution of a slightly soluble electrolyte in contact with some of the solid electrolyte...
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Transcribed Image Text:A saturated solution of lead iodate in pure water has a lead ion concentration of 4.0×10³ mole
liter at 25°C.
per
(a) Calculate the value for the solubility-product constant of Pb(IO3)2 at 25°C.
(b) Calculate the molar solubility of Pb(IO3)2 in a 0.10 molar Pb(NO3): solution at 25°C.
(c) To 333 milliliters of a 0.120-molar Ph(NO), solution, 667 milliliters of 0.435-molar KIO;
is added. Calculate the concentrations of Pb and IO in the solution at equilibrium at
25°C.
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