student leärns that the precipitate, AgCI(s), is slightly soluble in water. To determine the solubility, the student mixes a sample of the precipitate with warm, distilled water to make a saturated solution. The student finds the following equation for the dissolution of AgCl(s) in water and a Kp value at the temperature of the water. AgCl(s) Ag+(aq) + Cl (aq) Kp = 4.0 x 10-10 (d) Calculate Ag+] in the student's solution. B IU x? X, 0/ 10000 Word Limit (e) The value of Kp of another silver salt, AgBr(s), is 5.0 x 10-13 If separate, saturated solutions of AgBr and AgCl are prepared, which solution will have the greater [Ag+]? Justify your answer. B IU x? x, 5

student leärns that the precipitate, AgCI(s), is slightly soluble in water. To determine the solubility, the student mixes a sample of the precipitate with warm, distilled water to make a saturated solution. The student finds the following equation for the dissolution of AgCl(s) in water and a Kp value at the temperature of the water. AgCl(s) Ag+(aq) + Cl (aq) Kp = 4.0 x 10-10 (d) Calculate Ag+] in the student's solution. B IU x? X, 0/ 10000 Word Limit (e) The value of Kp of another silver salt, AgBr(s), is 5.0 x 10-13 If separate, saturated solutions of AgBr and AgCl are prepared, which solution will have the greater [Ag+]? Justify your answer. B IU x? x, 5

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 12.60PAE

See similar textbooks

Similar questions

Consider a metal ion A2+ and its nitrate salt, In an experiment, 35.00 mL of a 0.217 M solution of A(NO3)2 is made to react with 25.00 mL of 0.195 M NaOH. A precipitate, A(OH)2, forms. Along with the precipitation, the temperature increases from 24.8C to 28.2C. What is H for the precipitation of A(OH)2? The following assumptions can be made. â€¢ The density of the solution is 1.00 g/mL. â€¢ Volumes are additive. â€¢ The specific heat of the solution is 4.18 J/g C.
Use the solubility product constant from Appendix F to determine whether a precipitate will form if 10.0 mL of 1.0 106 M iron(II) chloride is added to 20.0 mL of 3.0 104 M barium hydroxide.
Calculate G at 25C for the reaction BaSO4(s)Ba2+(aq)+SO42(aq) See Appendix C for values of Gf.What is the value of the solubility product constant, Ksp, for this reaction at 25C?
Describe a nonchemical system that is not in equilibrium, and explain why equilibrium has not been achieved.
Write the expression of the reaction quotient for the ionization of HOCN in water.
The ore cinnabar (HgS) is an important source of mercury. Cinnabar is a red solid whose solubility in water is 5.5 X 10-2 mol L-1. Calculate its \p. What is its solubility' in grams per 100 g of water?
The solubility of thallium(1) iodide, TII, in water at 20 °C is 5.9 × 10-³ g L-¹. Using this fact, calculate Ksp for TII on the assumption that it is a saturated solution. Ksp =
Consider the reversible dissolution of lead (II) chloride. PbCl2 (s) = Pb2+ (aq) + Cl- (aq) Suppose you add 0.2435g of PbCl2 (s) to 50.0 mL of water. When the solution reaches equilibirum, you find that the concentration of Pb2+ (aq) is 0.0159M and the concentration of Cl- (aq) is 0.0318M. What is the value of the equilibrium constant, Ksp, for the dissolution of PbCl2?
Calculate the solubility of magnesium carbonate at 25 C in a solution that is 0.35 M sodium carbonate. (Note: just F.Y.I.: the solubility of magnesium carbonate in pure water is 2.6 x 10–3 M (25 C). Make sure you include the appropriate units in your answer. Ksp(MgCO3) = 6.8 x 10–6 (at 25 C)
To compute the solubility product (Ksp) of barium nitrate (Ba(NO3)2), an excess amount of Ba(NO3)2 was added to 2 liters of water at 25 degrees celcius until the solution is saturated. Ba(NO3)2 is only slightly soluble in water. It was observed in their experiments that the solution boils at 100.15 K. Barium nitrate dissociates via the process: ?a(NO3)2(s) ⇄ Ba2+(aq) + 2NO3- (aq) Ksp = [Ba2+][NO3-]2 What is the solubility product Ksp and vapor pressure of the solution?
Consider the reversible dissolution of lead(II) chloride. PbCl2 (s) Pb²+ (aq) + 2 Cl¯ (aq) Suppose you add 0.2311 g of PbCl2 (s) to 50.0 mL of water. When the solution reaches equilibrium, you find that the concentration of Pb2+ (aq) is 0.0159 M and the concentration of Cl¯ (aq) is 0.0318 M. What is the value of the equilibrium constant, K, for the dissolution of PbCl, ? Type answer:
Chapter 12 part 1 #12