Question

Which of the following salts are more soluble in acidic solution than in pure water?(a) Al(OH)3, (B)BaF2, (C)PbCl2,(D) Hg2Br2, (E) NiS,(F) AgI

Answer 1

the salts that will be more soluble in an acidic solution than in pure water will be those that contain basic anions

F-,OH-,S2- are basic anions

Ex

Al(OH)3 + 3 H+ --> Al3+ + 3H2O

This reaction is favourable and has a high reaction constant

Answer 2

acidic solution has high content of H+

(a) Al(OH)3 --> OH- ions in acidic solutions are low, therefore expect plenty of OH- ions from Al(OH)3 to dissociate; this will increase its solubilit

(B)BaF2 --> this increases solubility since F- ions form acid HF; Ba+2 incresaes in solution

(C)PbCl2 --> won't be good in acidic conditions since Pb+2 and Cl- do not form any equilibrium with H+

(D) Hg2Br2 --> no increase/decrease in solubility

(E) NiS --> May form HS equilibrium and H2S: Ni+2 may be high in solution

(F) AgI --> No increase/decrease in solution

Therefore options are

Al(OH)3 or BaF2

Since OH- ions inf Al are 3 times more fo that of F2 in BaF2

choose Al(OH)3

Answer 3

the order of acidic nature is

HI>HBr>HCl>HF>H2O>H2S

and on dissolution with an acidsolution, the given salts will form the above products .Now the order of stability of above products will be the reverse of the above order.

So, the solubility order will be

AgI