1. An aqueous solution is prepared that is initially 0.100 M Cdl2. After the equilibrium is established, the solution is found to be 0.013 M in Cd2+. The products of equilibrium are Cd2+ (aq)and I (aq). a) Write the expression of equilibrium constant b) Find the value of K. c) What will be the Cd2+ concentration, if 0.400M moles of KI is added to 1.00 L of the solution in the question. d) A solution is prepared by mixing 0.500 L of the solution from part c and mixed with 0.500 L of 2.0 X 10-5 m NaOH. Write the reaction. e) Will Cd (OH)2 precipitate. (HINT: Q is less than Ksp, there will be no precipitate) f) When the initial solution is heated, the Cd2+ increases. Is the equilibrium endothermic or exothermic and why?

1. An aqueous solution is prepared that is initially 0.100 M Cdl2. After the equilibrium is established, the solution is found to be 0.013 M in Cd2+. The products of equilibrium are Cd2+ (aq)and I (aq). a) Write the expression of equilibrium constant b) Find the value of K. c) What will be the Cd2+ concentration, if 0.400M moles of KI is added to 1.00 L of the solution in the question. d) A solution is prepared by mixing 0.500 L of the solution from part c and mixed with 0.500 L of 2.0 X 10-5 m NaOH. Write the reaction. e) Will Cd (OH)2 precipitate. (HINT: Q is less than Ksp, there will be no precipitate) f) When the initial solution is heated, the Cd2+ increases. Is the equilibrium endothermic or exothermic and why?

Chemistry: Principles and Practice

3rd Edition

ISBN:9780534420123

Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer

Publisher:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer

Chapter14: Chemical Equilibrium

Section: Chapter Questions

Problem 14.40QE

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