객관식
Complete the following solubility product constant expression for the dissolution of silver chloride (AgCl) in water: AgCl(s) ⇌ Ag^+(aq) + Cl^-(aq). Which of the following correctly represents the K_{sp} expression for AgCl?
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18. Aqueous Equilibrium
Solubility Product Constant: Ksp
객관식
Solubility of Sn(OH)2 was found to be 1.11 × 10-9 M; calculate Ksp of this compound.
A
5.47 × 10−27
B
4.44 × 10−9
C
1.23 × 10−18
D
1.37 × 10−27
검증된 단계별 안내1
Write the dissociation equation for Sn(OH)\_2 in water: Sn(OH)\_2 (s) \(\rightleftharpoons\) Sn^{2+} (aq) + 2 OH^{-} (aq).
Define the solubility (S) as the molar concentration of Sn(OH)\_2 that dissolves. Since the solubility is given as 1.11 \(\times\) 10^{-9} M, this means [Sn^{2+}] = S = 1.11 \(\times\) 10^{-9} M.
Express the hydroxide ion concentration in terms of solubility: for every 1 mole of Sn(OH)\_2 that dissolves, 2 moles of OH^{-} are produced, so [OH^{-}] = 2S = 2 \(\times\) 1.11 \(\times\) 10^{-9} M.
Write the expression for the solubility product constant, K_{sp}, based on the dissociation: K_{sp} = [Sn^{2+}] \(\times\) [OH^{-}]^{2}. Substitute the concentrations in terms of S: K_{sp} = S \(\times\) (2S)^{2} = S \(\times\) 4S^{2} = 4S^{3}.
Substitute the given solubility value into the expression for K_{sp} without calculating the final number: K_{sp} = 4 \(\times\) (1.11 \(\times\) 10^{-9})^{3}. This expression can then be evaluated to find the numerical value of K_{sp}.
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