9.3 - Solution Equilibrium

Question 1

Saturation point

Answer 1

An energetic equilibrium: low energy state found between tendency toward precipitation or dissolution

Question 2

Law of mass action

Answer 2

Dictates and predicts behaviors of solutions that are in dynamic equilibrium; discusses reaction rates based on relative concentrations

Question 3

Molar solubility

Answer 3

-molarity (of parent molecule) of solute at equilibrium

Question 4

Ksp

Answer 4

• the solubility product constant (an equilibrium constant), referring to the solubility of ionic compounds in water
• Ksp: [product]/[reactant] = [X]^a[Y]^b (solids, liquids don’t appear in equilibrium expressions)

Question 5

Solubility product constants: general facts

Answer 5

• increases with increasing temperature for non gas solutions and decreases for gas solutions
• high pressure favors dissolution of gas solutes

Question 6

Ion Product

Answer 6

-product of Ksp reaction taken at any moment rather than at equilibrium

Question 7

Common ion effect

Answer 7

• molar solubility of a salt decreases by presence of one of its ions in solution
• note Ksp doesn’t change

Question 8

Formation (equilibrium) constant

Answer 8

• Kf = [complex ion] / [X]^a[Y]^b
• oft significantly higher than Ksps, thus increase solubility of salt (higher Ksp)
• don’t precipitate out
• oft are formed from a mixture of solutions

Question 9

Discovery of Ksp from molar solubility

Answer 9

• every sparingly soluble salt of general form will have following where x is the molar solubility
  
  • MX, Ksp = x^2
  • MX^2, Ksp = 4x^3
  • MX^3, Ksp = 27x^4