Amongst the following hydroxides, the one which has the lowest value of Ksp at ordinary temperature (about 25°C) is
Correct answer: D. Be(OH)2
- A. Mg(OH)2
- B. Ba(OH)2
- C. Ca(OH)2
- D. Be(OH)2
Explanation
Be(OH)2 has the lowest value of Ksp at ordinary temperature because Be2+ ion is smaller than the other metal ions in the group, which results in a tighter bond with the 0H− ions, thus much lower solubility. The solubility of a hydroxide of group 2 elements increases down the group because as you go down the group size of metal increases thereby increasing the bond length and decreasing bond energy.
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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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