Ca(OH)2 is sparingly soluble having solubility constant value 6.5 x 10-6. What'll be its solubility:
Correct answer: C. 1.17 x 10^-2
- A. 2.75 x 10^-2
- B. 2.75 x 10^2
- C. 1.17 x 10^-2
- D. 3.63 x 10^3
Explanation
The solubility product constant (Ksp) expression for Ca(OH)2is: Ca(OH)2(s) ⇌ Ca2+(aq) + 2OH-(aq) The Ksp expression can be written as: Ksp = [Ca2+][OH-]^2 Given that the solubility constant value (Ksp) is 6.5 x10^-6, we can assume that x mol/L of Ca(OH)2 dissolves, leading to theformation of x mol/L of Ca2+ and 2x mol/L of OH-. Substituting these values into the Ksp expression, we get: 6.5 x 10^-6 = (x)(2x)^2 6.5 x 10^-6 = 4x^3 Dividing both sides by 4, we have: 1.625 x 10^-6 = x^3 To find x, we can take the cube root of both sides: x = (1.625 x 10^-6)^(1/3) Calculating this value gives us: x ≈ 0.0117 mol/L Therefore, the solubility of Ca(OH)2 is approximately 0.0117mol/L.
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