Both silver(I) bromide and silver(I) iodide are slightly soluble salts, with Ksp values at 25°C of 5.40×10-13 and 8.30×10-17, respectively. A solution of silver(I) nitrate is added to a solution that is 0.434 M in bothBr– andI–. What are the minimum Ag+ concentrations required for precipitation of AgBr and of AgI to occur? AgBr mol/L AgI mol/L

Both silver(I) bromide and silver(I) iodide are slightly soluble salts, with Ksp values at 25°C of 5.40×10-13 and 8.30×10-17, respectively. A solution of silver(I) nitrate is added to a solution that is 0.434 M in bothBr– andI–. What are the minimum Ag+ concentrations required for precipitation of AgBr and of AgI to occur? AgBr mol/L AgI mol/L

Chemistry: Principles and Reactions

8th Edition

ISBN:9781305079373

Author:William L. Masterton, Cecile N. Hurley

Publisher:William L. Masterton, Cecile N. Hurley

Chapter15: Complex Ion And Precipitation Equilibria

Section: Chapter Questions

Problem 68QAP

See similar textbooks

Similar questions

Suppose that solid AgCl and AgI are placed in 1.0 L water in separate beakers. Some, but not all, of each solid compound dissolves. In which beaker is the silver ion concentration, [Ag+], larger? Does the volume of water in which each compound dissolves affect the equilibrium concentration?
Both silver(I) bromide and silver(I) iodide are slightly soluble salts, with Ksp values at 25°C of 5.40×10-13 and 8.30×10-17, respectively. A solution of silver(I) nitrate is added to a solution that is 0.504 M in both Br– and I–. What are the minimum Ag+ concentrations required for precipitation of AgBr and of AgI to occur? AgBr = Agl = What percentage of the halide ion that is precipitated first remains in solution before the second begins to precipitate?
Both silver(I) bromide and silver(I) iodide are slightly soluble salts, with Ksp values at 25°C of 5.40×10-13 and 8.30×10-17, respectively. A solution of silver(I) nitrate is added to a solution that is 0.504 M in both Br– and I–. What are the minimum Ag+ concentrations required for precipitation of AgBr and of AgI to occur? - AgBr = AgI = What percentage of the halide ion that is precipitated first remains in solution before the second begins to precip itate?
Will Mn(OH)2 precipitate from a 0.01 M solution of MnCl2 at pH = 9? Ksp(Mn(OH)2) = 1,0 x 10-13. Discuss from solubility diagrams and prove by calculation.calculation. Co is a metal that is present in every lithium battery to stabilize its charge and toincrease stability. Every cell phone, tablet and electric car relies on the availability ofcobalt, 97% of which is extracted from mines in places like the Congo, where essentially slave labor is used.Cobalt ions form complexes with e.g. CN- . You see solubility diagrams and fraction diagrams for CoCO3 with and without the addition of 10 mM CN- .. Explain whythe solubility of cobalt carbonate increases at high pH when cyanide ions are present.Write reaction formulas for the formation of the dominant cobalt cyanide complexes.
The solubility of Ag2CrO4 (Ksp = 1.2 x 10-12) is several times greater than that of AgCl (Ksp = 1.82 x 10-10), so the red precipitate cannot form until all the chloride ions have effectively been removed from the solution. If a student uses 1 mg of K2CrO4 Aas an indicator for 100 mL of sample solution, what is the concnetrion of chloride ion in the solution when the red precipitate (Ag2CrO4) starts to form?
Sodium sulfate is slowly added to a solution containing 0.0500 M Ca2+(aq) and 0.0260 M Ag+(aq). What will be the concentration of Ca2+(aq) when Ag2SO4(s) begins to precipitate? Solubility-product constants, ?sp, can be found in the chempendix. [Ca2+]= M What percentage of the Ca2+(aq) can be precipitated from the Ag+(aq) by selective precipitation? percentage:
Calculate the molar solubility of lead (II) chloride in a solution of 0.0250 M CaCl2. Ksp for PbCl2 is 1.6x10-5
When silver chromate, Ag2CrO4, dissolves in otherwise pure water, what is the relation between [Ag+] and [CrO42-]? The solubility product of Ag2CrO4 is 1.9x10-12. Show that its solubility in pure water is 0.78x10-4 M.
Determine the molar solubility for Ag₂SO₄ (Ksp = 1.5 × 10⁻⁵) in a solution that already contains 0.200 M AgNO₃.
The solubility of lead (II) iodide is found to be .00130 M What is the Ksp for PbI2?
calculate the molar solubility of AgBr in 3.1×10−2 M AgNO3 solution. Ksp = 5.0x10-13 for AgBr
a. Calculate the molar solubility of AgBr in pure water.Ksp for AgBr is 5.0×10-13. 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 = 1.7×107 . 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?