Multiple Choice
Calculate the molar solubility of tin(II) hydroxide (Sn(OH)₂) in pure water given that its solubility product constant (Ksp) is 5.45 x 10⁻²⁷.
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18. Aqueous Equilibrium
Solubility Product Constant: Ksp
Multiple Choice
Calculate the solubility of LaF₃ in grams per liter in pure water, given that the Ksp of LaF₃ is 2.0 x 10⁻¹⁹.
A
0.00013 g/L
B
0.013 g/L
C
0.13 g/L
D
0.0013 g/L
Verified step by step guidance1
Understand the dissolution process of LaF₃ in water: LaF₃(s) ⇌ La³⁺(aq) + 3F⁻(aq). This indicates that one mole of LaF₃ produces one mole of La³⁺ ions and three moles of F⁻ ions.
Write the expression for the solubility product constant (Ksp) for LaF₃: Ksp = [La³⁺][F⁻]³. Given Ksp = 2.0 x 10⁻¹⁹, this expression will help us find the solubility in terms of molarity.
Let the solubility of LaF₃ be 's' mol/L. Then, [La³⁺] = s and [F⁻] = 3s because three fluoride ions are produced for each formula unit of LaF₃ that dissolves.
Substitute the concentrations into the Ksp expression: Ksp = (s)(3s)³ = 27s⁴. Set this equal to the given Ksp value: 27s⁴ = 2.0 x 10⁻¹⁹.
Solve for 's' to find the molar solubility, and then convert this molar solubility to grams per liter using the molar mass of LaF₃ (195.9 g/mol). This will give you the solubility in g/L.
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