u2: solubility product constant

Question 1

how do u write net ionic eqns?

Answer 1

1. do solid to aqueous
2. expand both and add charges, except the solid
3. cancel out wtvrs on both sides

Question 2

types of solutions

Answer 2

• unsaturated: more solute can dissolve
• saturated: more solute can’t dissolve
• supersaturated: unstable + crystals

Question 3

degrees of solubility

Answer 3

• soluble: more than 1g per 100mL
• insoluble: less than 0.1g per 100mL
• slightly soluble: 0.1 to 1g per 100mL

Question 4

when is solubility equilibrium

Answer 4

rate of dissolution = rate of precipitation

Question 5

Ksp

Answer 5

• equilibrium constant between ionic solid and saturated sol’n
• smaller value = lower solubility
• solubility of a substance can change as concentrations of other solutes change
• Ksp has only one value at any temp.

Question 6

Qsp

Answer 6

• trial ion product
• can be compared to Ksp to determine if precipitate formed when metal cations and nonmental anions mixed

Question 7

Qsp in relation to Ksp

Answer 7

Qsp > Ksp: precipitate forms, supersaturated sol’n
Qsp = Ksp: preciptate doesn’t form, saturated sol’n
Qsp < Ksp: precipitate doesn’t form, unsaturated sol’n

Question 8

what is Ksp used for

Answer 8

only for saturated solutions w/ dynamic equilibrium between dissolved and undissolved solute

Question 9

relationship between Ksp value and solubility

Answer 9

smaller Ksp = less soluble