Consider mixing 5.1×10^{- 6} moles of Na₂SO₄ and 1.2×10^{- 5} moles of BaCl₂ in enough water to form 1.0 L of an aqueous solution. BaSO₄ has limited solubility with a K _sp= 1.1×10^{- 10}. Na₂SO₄ (aq) + BaCl₂ (aq)→BaSO₄ (s) + 2 NaCl (s) Which statement below is true regarding the solubility reaction quotient, Q _sp, and whether or not a precipitate of BaSO₄ will form?

Question

Quizplus · Accepted Answer

The reaction quotient, Q _sp, can be calculated using the concentrations of the products and reactants at any given moment during the mixing process. However, the solubility product constant, K _sp, is a constant value that represents the maximum value of Q _sp at which the solution is still in equilibrium and no precipitate of BaSO₄ will form. If Q _sp is less than K _sp, then the solution is not saturated with BaSO₄ and no precipitate will form. Therefore, the correct choice is D, Q _sp < K _sp and a precipitate of BaSO₄ will not form.

Consider Mixing 5