The molarity of a solution is 0.15 M in NaI (aq) at 298.15 K. A large excess of HgI2 (s) to the solution. What is the solubility (in grams) of HgI2 (s) at saturation? HgI2 (s)<------->Hg2+ (aq) + 2I- (aq) Ksp= 2.7 × 10^-29 HgI2 (s) + 2I- <------> [HgI4]2- (aq) Kf= 0.75 M

The molarity of a solution is 0.15 M in NaI (aq) at 298.15 K. A large excess of HgI2 (s) to the solution. What is the solubility (in grams) of HgI2 (s) at saturation? HgI2 (s)<------->Hg2+ (aq) + 2I- (aq) Ksp= 2.7 × 10^-29 HgI2 (s) + 2I- <------> [HgI4]2- (aq) Kf= 0.75 M

Principles of Modern Chemistry

8th Edition

ISBN:9781305079113

Author:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Publisher:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Chapter14: Chemical Equilibrium

Section: Chapter Questions

Problem 94AP

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The molarity of a solution is 0.15 M in NaI (aq) at 298.15 K. A large excess of HgI2 (s) to the solution. What is the solubility (in grams) of HgI2 (s) at saturation?

HgI2 (s)<------->Hg2+ (aq) + 2I- (aq) Ksp= 2.7 × 10^-29
HgI2 (s) + 2I- <------> [HgI4]2- (aq) Kf= 0.75 M

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