If ionic product is less than Ksp then:
Correct answer: D. No precipitation will occur
- A. Solution will be saturated
- B. Precipitation will occur
- C. Solution will be super saturated
- D. No precipitation will occur
Explanation
Option D is correct. The ionic product is less than the solubility product, meaning the solution contains fewer ions than it could have at equilibrium. There is room for more ions and the saturation point is not reached. As saturation is not attained, therefore, precipitation does not occur. There are insufficient ions to exceed Ksp and form a solid precipitate. ==> Precipitation only occurs when the ionic product exceeds Ksp.
This question appeared on the KMU MDCAT 2023 paper, which you can sit online with every answer explained.
Report an error
The more specific you are, the faster it gets fixed. A source beats an opinion.
Prefer email? [email protected]
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.
Discussion
Stuck on an option, or know a faster way to get there? Ask or explain it here.
No comments yet. Be the first to explain this one.
Exams that ask Chemistry questions like this
Chemistry is on 14 papers prepared for on TestUstad, and all of them draw the same bank, so this question is worth knowing for every one of them.
More Solubility Product questions
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?
Salts which dissolve in water with evolution of heat. The effect of temperature on their solubility will be:
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:
Solubility of Ce2(SO4)3.