Question

Using your value of Ksp, and starting with an equilibrium system consisting of a saturated solution of calcium hydroxide, predict whether the solubility will increase or decrease it you add a. A. 5.00 mL of 0.100 M HNO3 Ksp = 2.966610-5 b. 5.00 mL of 0.100 M NaOH C. 5.00 mL of 0.100 M Ca(NO3)2

Answer 1

(A)
`HNO_(3)` Solubility will increase.

(B)
`NaOH` Solubility will decrease.

(C)
`Ca(NO_(3) )_(2)` Solubility will decrease.

Step-by-step explanation:

a) According to Le Chatelier's Principle when a change is introduced in a reaction system at equilibrium, the system responds by the reaction shifting in the direction to counter the change introduced.

When the change introduced is addition of acid, some
`OH^(-)` are consumed due to it and the system would respond by reaction shifting towards creation of more
`OH^(-)` in the system by increased dissolution. Thus solubility increase.

(b) When
`OH^(-)` are added, the reaction shifts to counter the change introduced of increased
`OH^(-)` by shifting to side that decreases the increased
`OH^(-)`. That happens by reaction shifting towards some
`Ca (OH)_(2)` precipitating back. Hence solubility decreases.

(c) The change introduced is addition of
`Ca^(2+)` which will be countered by reaction shifting to side that decreases increased
`Ca ^(2+)`, which happens by some
`Ca(OH)_(2)` precipitating back. Hence solubility decreases.