1. Consider the process by which potassium hydroxide dissolves in water and dissociates into its individual ions.

a. Write a balanced equation for this process, indicating all relevant phases (2 pts)

b. Using values from Appendix 4 in your textbook, calculate the standard enthalpy change

associated with this process. (3 pts)

c. Which is stronger: the IMF in water and the ionic bonding in potassium hydroxide, or the

IMF formed between water and the respective ions when potassium hydroxide is

dissolved? Explain how you know. (3 pts)

d. If potassium hydroxide comes out of the drying oven at a temperature of 88C and is

immediately mixed into a beaker of water at 32C, will its dissolution be spontaneous?

Please provide relevant work to support your answer. (6 pts)

e. What is the change in Gibbs free energy for the dissolution described in part d? (3 pts)