Multiple Choice
Determine the molar solubility of Ag2CrO4 in a solution containing 0.153 M AgNO3. The Ksp for Ag2CrO4 is 2.0 × 10^-12.
18. Aqueous Equilibrium
Solubility Product Constant: Ksp
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Given the solubility product constant (Ksp) of NiS is 3.0 x 10^-15, determine the molar solubility of NiS in 0.052 M K2C2O4.
A
1.2 x 10^-7 M
B
5.8 x 10^-8 M
C
2.3 x 10^-6 M
D
4.5 x 10^-5 M
Verified step by step guidance1
Start by writing the balanced dissolution equation for NiS: NiS(s) ⇌ Ni²⁺(aq) + S²⁻(aq).
Express the solubility product constant (Ksp) for NiS in terms of the concentrations of the ions: Ksp = [Ni²⁺][S²⁻].
Let the molar solubility of NiS be 's'. Then, [Ni²⁺] = s and [S²⁻] = s. Substitute these into the Ksp expression: Ksp = s².
Since NiS is dissolving in a solution containing K2C2O4, consider any common ion effect. However, K2C2O4 does not provide Ni²⁺ or S²⁻ ions, so the common ion effect does not apply here.
Solve for 's' using the Ksp value: s = √(Ksp). Substitute Ksp = 3.0 x 10⁻¹⁵ into the equation to find the molar solubility of NiS.
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