a. Calculate the molar solubility of AgI in pure water. Ksp for AgI is 1.5 × 10-¹6 . Solubility = M b. Calculate the molar solubility of AgI in 2.5 M NH3. The overall formation constant for Ag (NH3)2† is 1.7 × 107. Solubility = M c. Compare the calculated solubilities from parts a and b. O The solubility from (a) is greater. O The solubility from (b) is greater. O The solubilities from (a) and (b) are the same.

a. Calculate the molar solubility of AgI in pure water. Ksp for AgI is 1.5 × 10-¹6 . Solubility = M b. Calculate the molar solubility of AgI in 2.5 M NH3. The overall formation constant for Ag (NH3)2† is 1.7 × 107. Solubility = M c. Compare the calculated solubilities from parts a and b. O The solubility from (a) is greater. O The solubility from (b) is greater. O The solubilities from (a) and (b) are the same.

Chemistry: An Atoms First Approach

2nd Edition

ISBN:9781305079243

Author:Steven S. Zumdahl, Susan A. Zumdahl

Publisher:Steven S. Zumdahl, Susan A. Zumdahl

Chapter15: Solubility And Complex Lon Equilibria

Section: Chapter Questions

Problem 101CP: a. Calculate the molar solubility of AgBr in pure water. Ksp for AgBr is 5.0 1013. b. Calculate the...

See similar textbooks

Similar questions

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)
Consider 0.0010-M solutions of these sparingly soluble solutes in equilibrium with their ions. Predict the effect on each equilibrium if a saturated solution of sodium iodide were added. Explain your prediction in each case. AgI(s) ⇌ Ag+(aq) + I−(aq) PbI2(s) ⇌ Pb2+(aq) + 2 I−(aq)
The solubility of zinc oxalate, ZnC2O4, in 0.0150 M ammonia is 3.6 104 mol/L. What is the oxalate-ion concentration in the saturated solution? If the solubility product constant for zinc oxalate is 1.5 109, what must be the zinc-ion concentration in the solution? Now calculate the formation constant for the complex ion Zn(NH3)42+.
What is the solubility (in grams per liter) of strontium sulfate, SrSO4, in 0.36 M sodium sulfate, Na2SO4?
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 leaving the other in solution. (a) Ba2+ and Na+ (b) Ni2+ and Pb2+
Assume you dissolve 0.235 g of the weak acid benzoic acid, C6H5CO2H, in enough water to make 1.00 102 mL of solution and then titrate the solution with 0.108 M NaOH. C6H5CO2H(aq) + OH(aq) C6H5CO2(aq) + H2O() (a) What was the pH of the original benzoic add solution? (b) What are the concentrations of all of the following ions at the equivalence point: Na+, H3O+, OH, and C6H5CO2? (c) What is the pH of the solution at the equivalence point?
a. Calculate the molar solubility of AgBr in pure water. Ksp for AgBr is 5.0 1013. b. Calculate the molar solubility of AgBr in 3.0 M NH3. The overall formation constant for Ag(NH3)2+ is 1.7 107, that is, Ag+(aq)+2NH3(aq)Ag(NH3)2+(aq)K=1.7107. c. Compare the calculated solubilities from parts a and b. Explain any differences. d. What mass of AgBr will dissolve in 250.0 mL of 3.0 M NH3? e. What effect does adding HNO3 have on the solubilities calculated in parts a and b?