객관식
Determine the equilibrium expression of the barium nitride solid.
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7. Energy, Rate and Equilibrium
Solubility Product Constant (Ksp)
Multiple Choice
The Ksp value for strontium fluoride, SrF2, is 7.9×10–10 at 25ºC. Calculate its solubility in g/L.
A
5.8×10–4 g/L
B
7.3x10-2 g/L
C
4.6×10–6 g/L
D
0.092 g/L
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검증된 단계별 안내1
Write the dissolution equation for strontium fluoride: SrF2(s) ⇌ Sr²⁺(aq) + 2F⁻(aq).
Express the solubility product constant (Ksp) in terms of the concentrations of the ions: Ksp = [Sr²⁺][F⁻]².
Let the solubility of SrF2 be 's' mol/L. Then, [Sr²⁺] = s and [F⁻] = 2s because each formula unit of SrF2 produces one Sr²⁺ ion and two F⁻ ions.
Substitute the expressions for the ion concentrations into the Ksp expression: Ksp = (s)(2s)² = 4s³.
Solve for 's' by setting 4s³ equal to the given Ksp value (7.9×10⁻¹⁰) and then convert the solubility from mol/L to g/L using the molar mass of SrF2.
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