Determine whether or not Hg2Br2 will be more soluble in acidic solution than in

Question

Determine whether or not Hg2Br2 will be more soluble in acidic solution than in pure water.

Determine whether or not  will be more soluble in acidic solution than in pure water.

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Part B

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Part C

Determine whether or not Mg(OH)2 will be more soluble in acidic solution than in pure water.

Determine whether or not  will be more soluble in acidic solution than in pure water.

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Part D

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Part E

Determine whether or not CaCO3 will be more soluble in acidic solution than in pure water.

Determine whether or not  will be more soluble in acidic solution than in pure water.

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Part F

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Part G

Determine whether or not AgI will be more soluble in acidic solution than in pure water.

Determine whether or not  will be more soluble in acidic solution than in pure water.

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Explanation / Answer

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

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.

Except these 6, remaining all are more soluble in acidic solution than in pure water.

Hence,

1) Hg2Br2 ---------> Hg2+ + 2Br-

Br- will not accept protons in acid solution. Hence,  Hg2Br2will not be more soluble in acidic solution.

2) Mg(OH)2 ---------> Mg+2 + 2OH-

OH- will accept protons in acid solution. Hence, Mg(OH)2 will be more soluble in acidic solution than in pure water.

3) CaCO3 -----------> Ca2+   + CO32-

CO32- will accept protons in acid solution. Hence, CO32-will be more soluble in acidic solution than in pure water.

4) AgI ---------------> Ag+ + l-

l- will not accept protons in acid solution. Hence, Agl will not be more soluble in acidic solution.

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