CaF₂ (s) ⇄Ca (aq) + 2F (aq)
KP = [Ca²⁺][F]²
Use the stoichiometry of the reaction to prepare an ICE table showing the initial concentration of the common ion.
CaF2 (s) ⇄ Ca (aq) + 2F (aq)
initial 0 0.010
change +S +S
equili S 0.010+S
Kp = [Ca²⁺][F]²
= (S)(0.010+S)²
= S(0.010)²
S= KP/(0.010)²
= 4.0×10⁻¹¹/1x104
= 4×10⁻⁷ M
A saturated solution is a solution in which as many solutes as possible are dissolved. At a certain temperature, solutes can no longer dissolve in saturated solutions. A saturated solution can be made by dissolving more solutes until no more solutes are dissolved. If adding more solute does not dissolve it, the original solution is saturated. If the added solute dissolves, the original solution was unsaturated.
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