The molar solubility of magnesium carbonate is 1.8 × 10–4 mol/l. What is ksp for this compound?

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

i'm assuming that it's c.) red bank..

it is a solid

explanation: