A salt AB ionizes as AB = A+ > B- .The solubility product for the salt AB is 4.0 x 10-4. The molar solubility of the salt is:
Correct answer: B. 2.0 x 10^-2 M
- A. 4.0 x 10^-4 M
- B. 2.0 x 10^-2 M
- C. 8.0 x 10^-4 M
- D. 2.0 x 10^-4 M
Explanation
The solubility product (Ksp) of a salt AB that ionizes as AB = A+ + B- is given as 4.0 x 10-4. For a salt that dissociates in a 1:1 ratio, the Ksp expression is [A+][B-] = x2, where x represents the molar solubility. Solving for x, we find that x = √(4.0 x 10-4) = 2.0 x 10-2 M, which is option B. The other options are incorrect because they either confuse the Ksp value as the molar solubility or incorrectly perform the square root calculation.
This question appeared on the ETEA MDCAT 2013 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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