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# Ksp: Common Ion Effect

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Sections
Intro to Buffers
Henderson-Hasselbalch Equation
Intro to Acid-Base Titration Curves
Strong Titrate-Strong Titrant Curves
Weak Titrate-Strong Titrant Curves
Acid-Base Indicators
Titrations: Weak Acid-Strong Base
Titrations: Weak Base-Strong Acid
Titrations: Strong Acid-Strong Base
Titrations: Diprotic & Polyprotic Buffers
Solubility Product Constant: Ksp
Ksp: Common Ion Effect
Precipitation: Ksp vs Q
Selective Precipitation
Complex Ions: Formation Constant

Common Ion Effect occurs when an ionic solid is dissolved in a solution containing ions common to it,

Concept #1: Common Ion Effect on Solubility

Solubility of an ionic solid decreases in the presence of common ions.

Example #1: Determine molar solubility of CuCO(Ksp = 2.4 x 10-10) in 0.15 M MgCO3 solution.

Concept #2: Common Ion Effect: Acids & Bases

Solubility of base decreases in presence of OH- ions, while solubility of acid decreases in presence of H+ ions.

Example #2: Find solubility (g/mL) of Cr(OH)(Ksp = 6.7 x 10-31) if the solution is buffered at pH of 8.4 at 25ºC.

Practice: Which of the following compounds will become more soluble in basic solution?

a) PbF2 (s)

b) ZnCl2 (s)

c) Al(OH)3 (s)

d) MgCO3 (s)

Practice: A solution of Ba(OH)2 has a Ksp of 5.0 x 103.

i) Determine the pH of this solution.

ii) Determine the pH if Ba(OH)2 was added to a solution containing 3.2 M of BaF2 and 0.94 M of Al(OH)3.