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18 February, 00:52

What is the solubility in moles/liter for magnesium hydroxide at 25 oC given a Ksp value of 1.1 x 10-11. Write using scientific notation and use 1 or 2 decimal places (even though this is strictly incorrect!)

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Answers (2)
  1. 18 February, 01:25
    0
    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
  2. 18 February, 01:50
    0
    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
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