Which of the following will be more soluble in an acidic solution than in pure water? Be(OH)2 RbClO4 CuCl AlPO4 PbSO4

Ans: Be(OH)₂, AlPO₄ , PbSO₄ are more soluble in an acidic solution than in pure water.

Explanation:

Be(OH)₂ ---------> Be⁺² + 2OH^-

RbClO₄ -----------> Rb⁺ + ClO₄^-

CuCl ---------------> Cu⁺ + Cl^-

AlPO₄ --------------> Al⁺³ + PO₄^-3

PbSO₄ --------------.> Pb⁺² + SO₄^-2

Any base which accepts protons from acid in an acid solution is more soluble in acid than in water.

The anions OH^-, ClO₄^-, Cl^-,PO₄^-3 and SO₄^-2, are the resulting bases from Be(OH)₂, RbClO₄,CuCl, AlPO₄,PbSO₄^.

There are six strong acids, HClO₄, H₂SO₄, HNO₃, HI,HBr and HCl. They completely dissociate in water to ClO₄^-, HSO₃^-, HNO₃^-, Cl^-, I^- and Br^- ions. Therefore, these six anions will not accept protons and their salts will not be more soluble in acid solution.

Hence,

1) Be(OH)₂ ---------> Be⁺² + 2OH^-

OH^- will accept protons in acid solution. Hence,Be(OH)₂ is more soluble in acid solution.

2) RbClO₄ -----------> Rb⁺   + ClO₄^-

ClO₄^- will not accept protons in acid solution. Hence, RbClO₄ will not be more soluble in acid.

3) CuCl ---------------> Cu⁺ + Cl^-

Cl^- will not accept protons in acid solution. Hence,CuCl will not be more soluble in acid.

4) AlPO₄ --------------> Al⁺³ + PO₄^-3

PO₄^-3 will accept protons in acid solution. Hence, AlPO₄ is more soluble in acid solution.

5) PbSO₄ --------------.> Pb⁺² + SO₄^-2

SO₄^-2 will accept protons in acid solution. Hence, PbSO₄ is more soluble in acid solution.