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Ch.16 - Aqueous Equilibrium WorksheetSee all chapters

# Precipitation: Ksp vs Q

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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

Comparing Ksp value to Q value determines if a precipitate is likely to form.

Concept #1: Solution Saturation

Relative values of Ksp vs Q determine the degree of solution saturation.

Example #1: Will BaSO4 precipitate out when 8.2 x 10-7 M BaCO3 is mixed with 5.7 x 10-6 M SrSO4? Ksp of BaSO4 is 1.1 x 10-10.

Practice: Two mixtures are added into one flask at 25 °C, one mixture contains 0.55 mL of 0.75 M BaF2 and another 0.25 mL of 1.3 M Mg(OH)2. Ksp of Magnesium Fluoride, MgF2, is 7.4 x 109. Identify the correct option.

a) MgF2 solid will form

b) MgF2 solid forms, along with Mg+2 and F ions

c) solution is unsaturated, precipitate does not form

d) solution is saturated, precipitate forms