Solution Chemistry

Question 1

Hydration

Answer 1

Hydration is where water forms a shell around ions in solution.

Question 2

Normality

Answer 2

Equivalents per unit volume. Molarity of species that matter (usually hydrogen)

Question 3

Solubility product constant, the equilibrium expression

Answer 3

Equilibrium constant for a solid substance dissolving in an aqueous solution. It represents the level at which a solute dissolves in solution. A more a substance dissolves, the higher the K_sp value it has.

Question 4

Common Ion Effect:

Answer 4

The solubility of the reaction is reduced by the common ion, so if dealing with two of the same reactions the reaction with the ion will have a lesser Ksp and the reaction without the ion will have a greater Ksp.

Question 5

Salt Effect (diverse ion effect)

Answer 5

Having an opposing effect on the Ksp value compared to the common ion effect, uncommon ions increase the Ksp value. Uncommon ions are those that are different from those involved in equilibrium.

Question 6

Ion Pairs

Answer 6

When you have an ionic pair (cation and anion) the Ksp value calculated will be lower than the actual value due to ions involved in pairing. To reach the calculated Ksp value, more solute must be added.

Question 7

What is the solubility product constant expression for MgF₂?

Answer 7

MgF₂(s) ↔ Mg²⁺(aq) + 2F^-(aq) so the Ksp = [Mg²⁺][F-]²

Question 8

What is the solubility of MX₂ if given Ksp?

Answer 8

Ksp = 4[M²⁺]³

Question 9

Complex ion formation

Answer 9

Metal+ + Lewis base: → Complex ion

Question 10

Solubility and pH

Answer 10

Acids are more soluble in bases. and Bases are more soluble in acids.