Multiple Choice
What is the molar solubility of Fe(OH)2 at 25°C if the Ksp of the compound is 7.9 × 10⁻¹⁶?
18. Aqueous Equilibrium
Solubility Product Constant: Ksp
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A solution containing Ca(NO3)2 is mixed with a solution of Li2S to form a solution that is 2.1 × 10^-5 M in calcium ion and 4.75 × 10^-5 M in sulfide ion. What will happen once these solutions are mixed? Ksp (CaS) = 2.3 × 10^-9.
A
The solution will become supersaturated with CaS.
B
Nothing will happen since the ion product is less than the Ksp.
C
A precipitate of CaS will form since the ion product exceeds the Ksp.
D
The concentration of calcium ions will increase.
Verified step by step guidance1
Identify the ions present in the solution: calcium ions (Ca²⁺) and sulfide ions (S²⁻).
Calculate the ion product (Q) for the potential formation of calcium sulfide (CaS) using the concentrations of the ions: Q = [Ca²⁺][S²⁻].
Substitute the given concentrations into the ion product expression: Q = (2.1 × 10^-5 M) × (4.75 × 10^-5 M).
Compare the calculated ion product (Q) with the solubility product constant (Ksp) for CaS, which is 2.3 × 10^-9.
Determine the outcome: if Q > Ksp, a precipitate of CaS will form; if Q < Ksp, no precipitate will form and the solution remains unsaturated.
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