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.
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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.
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