Multiple Choice
Given that the solubility product constant (Ksp) of La(IO3)3 is 7.5 × 10^{-12}, what is the molar solubility of La(IO3)3 in pure water?
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18. Aqueous Equilibrium
Solubility Product Constant: Ksp
Multiple Choice
Given that the solubility product constant (Ksp) of C2D3 is 9.14 × 10^{-9}, what is the molar solubility of C2D3 in mol/L?
A
1.32 × 10^{-2} mol/L
B
1.32 × 10^{-3} mol/L
C
1.32 × 10^{-3} mol/L
D
1.32 × 10^{-2} mol/L
Verified step by step guidance1
Identify the dissociation equation of the compound C2D3 in water. For example, if C2D3 dissociates as C2D3 (s) \(\rightarrow\) C^{+} + D_3^{-}, then the molar solubility is represented by the concentration of ions produced.
Express the solubility product constant (K_{sp}) in terms of the molar solubility (s). For a salt that dissociates into one cation and one anion, K_{sp} = [C^{+}][D_3^{-}] = s \(\times\) s = s^{2}.
Set up the equation using the given K_{sp} value: s^{2} = 9.14 \(\times\) 10^{-9}.
Solve for the molar solubility s by taking the square root of both sides: s = \(\sqrt{9.14 \times 10^{-9}\)}.
Interpret the result as the molar solubility of C2D3 in mol/L, which represents the maximum concentration of C2D3 that can dissolve in water at equilibrium.
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