Given 4.2 moles of magnesium, how many moles of oxygen gas will be needed for the reaction? 2Mg () + 0, (g) - 2MgO (s)

Given:

Ksp of CaSO4 = 7.10 *10⁻⁵

Molar mass of CaSO4 = 136.1 g/mol

Volume of the solvent = 69.0 L

To determine:

The grams of CaSO4 that would dissolve in 69.0 L of solvent

Explanation:

CaSO4(s) ↔ Ca2+ (aq) + SO42-(aq)

Ksp = [Ca2+][SO42-]

Let 's' be the solubility i.e. moles of CaSO4 dissolved in a given volume of water

Therefore,

Ksp = (s)(s)

s = √Ksp = √7.10 *10⁻⁵ = 8.43 *10⁻³ moles/lit

i.e 0.00843 moles of CaSO4 can dissolve in 1 L of water

Therefore, # moles that can dissolve in 69.0 L = 0.00843 * 69.0 = 0.582 moles of CaSO4

The corresponding mass of CaSO4 = 0.582 moles * 136.1 g/mole = 79.21 g

Ans: 79.2 g of CaSO4 can dissolve in 69.0 L of water