For which salt in each of the following groups will the solubility depend on pH?

Pb(OH)2
PbCl2

could you explain too?
thanks!

Answered above.

To determine whether the solubility of a salt depends on pH, we need to consider its acidic or basic properties. In this case, we are considering two salts: Pb(OH)2 and PbCl2.

1. Pb(OH)2:
Pb(OH)2 is a basic salt because it contains the hydroxide ion (OH-). When dissolved in water, it hydrolyzes to form Pb2+ ions and OH- ions. The OH- ions can react with H+ ions from the water, which can affect the solubility of the salt.

To determine if the solubility of Pb(OH)2 depends on pH, we need to know the solubility product constant (Ksp) for this salt. The Ksp is an equilibrium constant that describes the solubility of a salt in water. The expression for the Ksp of Pb(OH)2 is:

Ksp = [Pb2+][OH-]^2

The solubility of Pb(OH)2 depends on how the concentration of OH- ions (which is pH dependent) affects the value of Ksp. Since the solubility of Pb(OH)2 is influenced by pH, we can conclude that the solubility of Pb(OH)2 is pH dependent.

2. PbCl2:
PbCl2 is a neutral salt because it does not contain any acidic or basic ions. When dissolved in water, it dissociates into Pb2+ ions and Cl- ions. Neither of these ions reacts with water or contributes to a pH-dependent reaction.

Therefore, the solubility of PbCl2 does not depend on pH.

In summary, the solubility of Pb(OH)2 depends on pH due to the presence of OH- ions, while the solubility of PbCl2 is not affected by pH.