7.5 Introduction to Solubility Equilibria

• What is solubility typically measured in?

  g/L or mol/L
• What type of solution has a solute amount equal to its solubility?

  Saturated
• What is the K_{sp}</latex> expression for $AgCl$?


  $K_{sp} =$$[Ag^ + ][Cl^ - ]$
• For gases dissolving in liquids, solubility decreases with temperature
• Solubility is equal to the square root of $K_{sp}$.


  True
• What happens to $KCl$ when temperature increases?


  $KCl(s) \xrightarrow{\Delta T} KCl(aq)$
• How can complex ion formation enhance solubility?

  Forms soluble complex ions
• What is the key reaction in the formation of calcium oxalate kidney stones?

  $Ca^{2 + }(aq) +$$C_{2}O_{4}^{2 - }(aq) \rightleftharpoons CaCO_{4}(s)$
• A saturated solution contains the maximum amount of solute that can dissolve at a specific temperature
• The equilibrium constant for the dissolution of an ionic compound is called the solubility product
• For most solids, solubility increases with temperature.


  True
• What is the dissolution of silver chloride ($AgCl$) represented as?


  $AgCl(s) \rightleftharpoons Ag^ +$$(aq) +$$Cl^ - (aq)$
• For gases dissolving in liquids, solubility increases with temperature.

  False
• pH affects the solubility of salts containing acidic or basic ions.


  True
• Solubility equilibria are used in selective precipitation to separate ions.


  True
• At 25°C, NaCl has a solubility of 360 g/L in water.


  True
• A supersaturated solution is stable and contains no excess solute.

  False
• What is the relationship between $K_{sp}$ and solubility?


  $Solubility =$$\sqrt{K_{sp}}$
• A higher $K_{sp}$ value indicates greater solubility.


  True
• Match the concept with its explanation:

  Equilibrium Constant ($K_{sp}$) ↔️ Equilibrium constant for dissolution of ionic compounds

  Solubility Product ↔️ Alternative name for $K_{sp}$

  Relationship to Solubility ↔️ $Solubility =$$\sqrt{K_{sp}}$
• What happens to $CO_{2}$ when pressure increases?


  $CO_{2}(g) \xrightarrow{P} CO_{2}(aq)$
• What happens to the solubility of salts in acidic or basic solutions?

  Increases
• Solubility equilibria have applications only in laboratory settings.

  False
• Which ions are separated in selective precipitation using AgCl</latex> and $Ag_{2}CrO_{4}$?


  Chloride and chromate ions