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

Answer:

(A) $HNO_{3}$ Solubility will increase.

(B) $NaOH$ Solubility will decrease.

(C) $Ca(NO_{3} )_{2}$ Solubility will decrease.

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.