Consider the dissolution of calcium hydroxide:

ca(oh)2(s) --> ca2+(aq) + 2oh‑(aq)

k = 4.7 x 10‑6

write the equilibrium expression for this reaction.

2. identify whether the following actions would favor the formation of products, reactants, or have no affect upon the dissolution of calcium hydroxide. explain each answer.

a. addition of caco3 to an equilibrium mixture of calcium hydroxide and water.

b. addition of na2co3 to an equilibrium mixture of calcium hydroxide and water.

c. addition of hcl to an equilibrium mixture of calcium hydroxide and water.

d. addition of naoh to an equilibrium mixture of calcium hydroxide and water

1.

2. a. No effect;

b. Products;

c. Products;

d. Reactants

Explanation:

1. Equilibrium constant might be written using standard guidelines:

Based on the guidelines, we have two ions on the product side, a solid on the left side. Thus, the equilibrium constant has the following expression:

2. a. In the following problems, we'll be considering the common ion effect. According to the principle of Le Chatelier, an increase in concentration of any of the ions would shift the equilibrium towards the formation of our precipitate.

In this problem, we're adding calcium carbonate. It is insoluble, so it wouldn't have any effect on the equilibrium.

b. Sodium carbonate is completely soluble, it would release carbonate ions. The carbonate ions would combine with calcium cations and more precipitate would dissolve. This would shift the equilibrium towards formation of the products to reproduce the amount of calcium cations.                                      

c. HCl would neutralize calcium hydroxide to produce calcium chloride and water, so the amount of calcium ions would increase, therefore, the products are favored.

d. NaOH contains hydroxide anions, so we'd have a common ion. An increase in hydroxide would produce more precipitate, so our reactants are favored.

the increase of protons   hope this