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?

🧪 Chemistry · Equilibrium · NEET & JEE

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?

Answer: Yes, because Q > K sp.

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

Correct answer: C. Yes, because Q > Ksp

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

Read the full Equilibrium notes →

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

Concept context

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