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.
Last updated
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.
Practise Chemical Equilibrium
625 free Chemical Equilibrium MCQs from Chemistry, each with the correct answer and an explanation. Unlimited attempts, no account needed.
Exams that ask Chemistry questions like this
Chemistry is on 12 papers prepared for on TestUstad, and all of them draw the same bank, so this question is worth knowing for every one of them.
Related questions
A saturated solution of a sparingly soluble salt is one in which
A solution can be both____________________?
Concentration of solute molecule when they are in equilibrium with solid substance at particular temperature is called________________?
Dissolution of which of these increases with temperature
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?