If Ca(OH)2 is dissolved in a solution of NaOH, its solubility, compared with that in pure water, is
Correct answer: B. Decreased
- A. Increased
- B. Decreased
- C. Unaffected
- D. None of these
Explanation
In a solution where Ca(OH)2 is dissolved in NaOH, the solubility of Ca(OH)2 decreases due to the common ion effect. The NaOH solution already contains OH- ions, which are also a product of the dissociation of Ca(OH)2. According to Le Chatelier's principle, the increased concentration of OH- ions shifts the equilibrium to favor the formation of solid Ca(OH)2, thus reducing its solubility. Option A is incorrect because solubility does not increase in the presence of a common ion. Option C is incorrect as the solubility is indeed affected by the common ion. Option D is incorrect because the correct answer has been provided in option B.
Report an error
The more specific you are, the faster it gets fixed. A source beats an opinion.
Prefer email? [email protected]
About Chemical Equilibrium
Reversible reactions reach dynamic equilibrium when forward and reverse rates become equal, and Le Chatelier's principle predicts the effect of changing concentration, pressure or temperature. The chapter also covers solubility product, the common ion effect, buffer action and the conditions used in Haber's process, with equilibrium shifts distinguished from changes in the equilibrium constant.
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 Chemical Equilibrium questions
Change in which of these conditions will change the K of an equilibrium given as a starting point?
In the Haber process for making ammonia, an increase in pressure favors
A small value for K, the equilibrium constant, indicates that
If Kc >> 1,
In a certain equilibrium process, the activation energy of the forward reaction is greater than the activation energy of the reverse reaction. This reaction is
What is the concentration of the Ag+ ion in a saturated solution of AgCl?(Ksp for AgCl = 1.7 × 10−10)