Which of the following will have the largest value of solubility product, or is most soluble in water?

B e {(O H)}_{2}

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B a {(O H)}_{2}

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C a {(O H)}_{2}

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M g {(O H)}_{2}

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Solution

The correct option is B $B a {(O H)}_{2}$
On moving down the group of alkaline earth metals, the solubility of metal hydroxides increases. The size of metal ion increases on moving down the group. Hence, the lattice energy decreases to greater extent than hydration energy. Hence, the solubility increases.

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While comparing solubility do we compare Ksp(solubility product values) or solubility (s) value

B a (O H)_{2} > S r (O H)_{2} > C a (O H)_{2} > B e (O H)_{2}

H_{2} O ?

(1) B e S O_{4} > M g S O_{4} > C a S O_{4} > B a S O_{4}

(2) B e (O H)_{2} > M g (O H)_{2} > C a (O H)_{2} > B a (O H)_{2}

(3) L i O H < N a O H < K O H < R b O H

(4) L i_{2} C O_{3} < N a_{2} C O_{3} < K_{2} C O_{3} < R b_{2} C O_{3}

H_{2} O

B e S O_{4} > M g S O_{4} > C a S O_{4} > B a S O_{4}

B e (O H)_{2} > M g (O H)_{2} > C a (O H)_{2} > B a (O H)_{2}

L i O H < N a O H < K O H < R b O H

L i_{2} C O_{3} < N a_{2} C O_{3} < K_{2} C O_{3} < R b_{2} C O_{3}

C a (O H)_{2}

C a (O H)_{2}

5.5 \times 10^{- 6}, {1.375}^{\frac{1}{3}} = 1.11

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