Which of the following sulphates has the highest solubility in water?

M g {S O}_{4}

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B a {S O}_{4}

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C a {S O}_{4}

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B e {S O}_{4}

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Solution

The correct option is C $B e {S O}_{4}$
Answer (D) $B e S O_{4}$
Solubility depends upon the resulting enthalpy of lattice energy and hydration enthalpy. For $M g S O_{4}$ , hydration enthaply is more hence it is soluble in water. Whereas, for $B a S O_{4}$ it is not enough that's why it is not soluble in water.
As sulphate ion has a much larger size , the relative increase in size from Be to Ba doesn't matter and the compounds have more or less the same lattice enthalpy. But hydration enthalpy steadily decreases from Be to Ba.. This solubility decreases.

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Similar questions

B e S O_{4}, M g S O_{4}, C a S O_{4}, S r S O_{4}, B a S O_{4}

N a_{2} S O_{4}, B e S O_{4}, M g S O_{4}

B a S O_{4}

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

B e S O_{4}, M g S O_{4}, C a S O_{4}, S r S O_{4}

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}

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