객관식
What is the molar solubility of Fe(OH) 3 (s) in a solution that is buffered at pH 3.50 at 25°C? The Ksp of Fe(OH)3 is 6.3 x 10–38 at 25°C.
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6. Chemical Equilibrium
Solubilty Product Constant
객관식
Arsenic trisulfide (As2S3) occurs naturally as the orange-yellow colored mineral orpiment. As2S3 is a highly insoluble substance with a Ksp value of 2.90×10−72. Calculate the solubility of As2S3 in g/100mL. (Molar mass of As2S3 = 246.04 g/mol)
A
2.12×10−17 g/100 mL
B
1.87×10−13 g/100 mL
C
6.25×10−15 g/100 mL
D
4.75×10−14 g/100 mL
검증된 단계별 안내1
First, write the dissolution equation for arsenic trisulfide (As2S3) in water: As2S3(s) ⇌ 2As^3+(aq) + 3S^2−(aq).
Next, express the solubility product constant (Ksp) in terms of the concentrations of the ions: Ksp = [As^3+]^2[S^2−]^3.
Let the solubility of As2S3 be 's' mol/L. Then, [As^3+] = 2s and [S^2−] = 3s. Substitute these into the Ksp expression: Ksp = (2s)^2(3s)^3.
Simplify the expression: Ksp = 4s^2 * 27s^3 = 108s^5. Set this equal to the given Ksp value: 108s^5 = 2.90×10^−72.
Solve for 's' to find the molar solubility, then convert this to grams per 100 mL using the molar mass of As2S3 (246.04 g/mol) and the conversion factor (1 L = 1000 mL).
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