Answer:
3.2 × 10⁻⁸
Explanation:
Let's consider the solution of magnesium carbonate.
MgCO₃ ⇄ Mg²⁺(aq) + CO₃²⁻(aq)
We can relate the molar solubility (S) with the solubility product (Ksp) using an ICE chart.
MgCO₃ ⇄ Mg²⁺(aq) + CO₃²⁻(aq)
I 0 0
C +S +S
E S S
The Ksp is:
Ksp = [Mg²⁺] × [CO₃²⁻] = S × S = S² = (1.8 × 10⁻⁴)² = 3.2 × 10⁻⁸
Answer:
Ksp = 3.2 * 10^-8
Explanation:
Step 1: Data given
magnesium carbonate = MgCO3
The molar solubility of magnesium carbonate = 1.8 * 10^-4 mol/L
Step 2: The balanced equation
MgCO3(s) ⇔ Mg^2+ + CO3^2-
For 1 mol MgCO3 we'll have 1 mol Mg^2+ and 1 mol CO3^2-
Step 3: Calculate Ksp for this compound
Ksp = [Mg^2+][Co3^2-]
For 1 mol MgCO3 we'll have 1 mol Mg^2+ and 1 mol CO3^2-
Ksp = X * X = X²
X = 1.8 * 10^-4
Ksp = (1.8 *10^-4 )* (1.8 * 10^-4)
Ksp = 3.2 * 10^-8
