CHEM 451DP #337.9 The thermodynamic solubility product of AgCl is 1.6x10-10. What is [Ag+] in (a) a 0.020 M KNO3solution and (b) a 0.020 M KCl solution?

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Answered: CHEM 451 DP #33 7.9 The thermodynamic…

Chemistry: Principles and Reactions

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Author:William L. Masterton, Cecile N. Hurley

Publisher:William L. Masterton, Cecile N. Hurley

Chapter21: Chemistry Of The Nonmetals

Section: Chapter Questions

Problem 48QAP: Calculate the solubility in grams per 100 mL of BaF2 in a 0.10 M BaCl2 solution.

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The Handbook of Chemistry and Physics (http://openstaxcollege.org/l/16Handbook) gives solubilities of the following compounds in grams per 100 mL of water. Because these compounds are only slightly soluble, assume that the volume does not change on dissolution and calculate the solubility product for each. (a) BaSiF6, 0.026 g/100 mL (contains SiF62- ions) (b) Ce(IO3)4, 1.5102 g/100 mL (c) Gd2(SO4)3, 3.98 g/100 mL (d) (NH4)2PtBr6, 0.59 g/100 mL (contains PtBr62- ions)
Calculate the solubility in grams per 100 mL of BaF2 in a 0.10 M BaCl2 solution.
Assuming that no equilibria other than dissolution are involved, calculate the concentrations of ions in a saturated solution of each of the following (see Appendix J for solubility products): (a) Agl. (b) Ag2SO4. (c) Mn(OH)2. (d) Sr(OH)28H2O (e) the mineral brucite, Mg(OH)2
The text describes zinc hydroxide as an amphoteric hydroxide, so Zn(OH)2 is soluble in basic solution. What is the molar solubility of Zn(OH)2 in 1.00 M NaOH? What is the pH of the equilibrium solution?
The solubility of cadmium oxalate. CdC2O4, in 0.150 M ammonia is 6.1 103 mol/L. What is the oxalate-ion concentration in the saturated solution? If the solubility product constant for cadmium oxalate is 1.5 108, what must be the cadmium-ion concentration in the solution? Now calculate the formation constant for the complex ion Cd(NH3)42+.
Solid Pbl2 (Ksp = 9.8 109) is placed in a beaker of water. After a period of time, the lead(II) concentration is measured and found to be 1.1 103 M. Has the system reached equilibrium? That is, is the solution saturated? If not, will more Pbl2 dissolve?
Calculate the solubility of copper(II) iodate, Cu(IO3)2 (Ksp = 7.4 108), in (a) water. (b) a 0.10 M copper(II) nitrate solution.
At 25C, 10.24 mg of Cr(OH)2 are dissolved in enough water to make 125 mL of solution. When equilibrium is established, the solution has a pH of 8.49. Estimate Ksp for Cr(OH)2.
A solution saturated with a salt of the type M3X2 has an osmotic pressure of 2.64 102 atm at 25C. Calculate the Ksp value for the salt, assuming ideal behavior.
Each pair of ions below is found together in aqueous solution. Using the table of solubility product constants in Appendix J, devise a way to separate these ions by adding a reagent to precipitate one of the ions as an insoluble salt and leave the other in solution. (a) Cu2+ and Ag+ (b) A13+ and Fe3+
Calculate the mass of manganese hydroxide present in 1300 mL of a saturated manganese hydroxide solution. For Mn(OH)2, Ksp = 2.0 1013.
What is the solubility of silver oxide, Ag2O, in a solution buffered at pH 10.78? The equilibrium is Ag2O(s) + H2O(l) 2Ag+(aq) + 2OH (aq); Kc = 2.0 108.

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CHEM 451 DP #33 7.9 The thermodynamic solubility product of AgCl is 1.6x10-10. What is [Ag+] in (a) a 0.020 M KNO3 solution and (b) a 0.020 M KCl solution?