Answer:
1.40 × 10⁻⁴ M
Explanation:
Let's consider the solution of magnesium hydroxide.
Mg(OH)₂(s) = Mg²⁺(aq) + 2 OH⁻(aq)
We can relate the solubility (S) of the hydroxide with the solubility product (Ksp) using an ICE chart.
Mg(OH)₂(s) = Mg²⁺(aq) + 2 OH⁻(aq)
I 0 0
C +S +2S
E S 2S
The solubility product is:
Ksp = [Mg²⁺] × [OH⁻]² = S × (2S)² = 4 S³
S = ∛(Ksp/4) = ∛(1.1 × 10⁻¹¹/4)
S = 1.40 × 10⁻⁴ M
Answer:
S = 0.00014 moles /L = 1.4 * 10^-4 moles/L
Explanation:
Step 1: Data given
Temperature = 25.0 °C
Ksp = 1.1 * 10^-11
Step 2: The balanced equation
Mg(OH)2(s) ⇆ Mg^2+(aq) + 2OH-(aq)
Step 3: Define Ksp
[Mg(OH)2 = 1.11 * 10^-11 = S
[Mg^2+] = S
[OH-] = 2S
Ksp = [Mg^2+]*[OH-]²
Ksp = S * (2S)²
1.1 * 10^-11 = 4S³
S³ = 2.75 * 10^-12
S = 0.00014 moles /L
