Excess of BaSO4 was dissolved in pure water at 250C. If its Ksp = 1 x 10^-10 what is the Conc: of Ba2+ ions in water?
Correct answer: C. 10-5
- A. 10-10
- B. 10-20
- C. 10-5
- D. 10-6
Explanation
The solubility product constant (Ksp) for BaSO4 at 25°C is given as 1 x 10-10. The dissolution of BaSO4 in water is represented by the equation:BaSO4 (s) ⇌ Ba2+ (aq) + SO42- (aq)According to the solubility product expression, Ksp = [Ba2+][SO42-]. Assuming the solubility of BaSO4 is x, we have [Ba2+] = x and [SO42-] = x.Therefore, Ksp = x2 = 1 x 10-10. Solving for x gives x = 10-5. This means the concentration of Ba2+ ions in water is 10-5 M, making Option C the correct choice.Options A, B, and D lead to incorrect values for the solubility product, hence they are incorrect.
This question appeared on the ETEA MDCAT 2016 paper, which you can sit online with every answer explained.
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About Solubility Product
The solubility product constant, Ksp, represents the equilibrium concentrations of ions from a sparingly soluble salt, each raised to its stoichiometric power. Problems involve writing Ksp expressions, calculating molar solubility, applying the common-ion effect and predicting precipitation from the ionic product.
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