Equal volumes of 2 × 10 −3 M BaCl 2 and 2 × 10 −3 M Na 2 SO 4 are mixed. Given K sp (BaSO 4 ) = 1 × 10 −10 , will BaSO 4 precipitate?

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Equal volumes of 2 × 10⁻³ M BaCl₂ and 2 × 10⁻³ M Na₂SO₄ are mixed. Given K_sp(BaSO₄) = 1 × 10⁻¹⁰, will BaSO₄ precipitate?

Answer: Yes, because Q > K_sp.

A No, because Q < K_sp
B No, Q equals K_sp exactly
C Yes, because Q > K_sp
D It cannot be predicted

Correct answer: C. Yes, because Q > K_sp

Explanation: After mixing each ion is halved to 1 × 10⁻³ M; Q = (10⁻³)(10⁻³) = 10⁻⁶ > K_sp, so it precipitates.

As the reaction proceeds, reactant concentration falls and product concentration rises until both level off at equilibrium.

Concept context

When forward and reverse reaction rates are equal, equilibrium is reached. Learn about Kc, Kp, Le Chatelier's principle, and acid-base equilibria, including pH, buffer solutions, and solubility product.

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Equal volumes of 2 × 10−3 M BaCl2 and 2 × 10−3 M Na2SO4 are mixed. Given Ksp(BaSO4) = 1 × 10−10, will BaSO4 precipitate?

Concept context

More Equilibrium questions

Equal volumes of 2 × 10⁻³ M BaCl₂ and 2 × 10⁻³ M Na₂SO₄ are mixed. Given K_sp(BaSO₄) = 1 × 10⁻¹⁰, will BaSO₄ precipitate?