Which of the following will be more soluble in an acidic solution than in pure water?

Be(OH)2 and CaCO3 should be much more soluble in acid solution than in pure water. I don't know the level of chemistry you are in but after beginning chemistry you will learn that PbSO4 is somewhat more soluble in acid solution, too although it isn't highly soluble.

Which of the following ionic compounds will be more soluble in acid solution than in water: (a) BaSO4, (b) PbCl2, (c) Fe(OH)3, (d) CaCO3? with explanation

The solubility of a substance is influenced by the pH of the solution. In general, substances that can form soluble species or have basic properties tend to be more soluble in an acidic solution than in pure water.

Based on this information, the substance that will be more soluble in an acidic solution than in pure water is:

Be(OH)2

Be(OH)2 is a metal hydroxide that can act as a base and react with acid to form a soluble species. In an acidic solution, the Be(OH)2 will react with the acid (proton acceptor) and form the soluble species, which will increase its solubility. In pure water, the lack of acid reduces the chances of formation of the soluble species, making it less soluble.

The other compounds listed (AgBr, RbClO4, CaCO3, and PbSO4) are not expected to show increased solubility in an acidic solution.

To determine which compound will be more soluble in an acidic solution than in pure water, we need to consider the solubility rules and how the compounds react with acid.

1. AgBr (Silver Bromide): AgBr is generally insoluble in water. However, in an acidic medium, AgBr can form a soluble complex ion called Ag(H2O)4Br2+ due to the reaction with acid. This increased solubility makes AgBr more soluble in an acidic solution than in pure water.

2. Be(OH)2 (Beryllium Hydroxide): Be(OH)2 is a base and tends to be insoluble in water, including in acidic conditions. So, it will not be more soluble in an acidic solution compared to pure water.

3. RbClO4 (Rubidium Perchlorate): RbClO4 is highly soluble in both water and acidic solutions. The acidity of the solution does not significantly affect the solubility of RbClO4.

4. CaCO3 (Calcium Carbonate): CaCO3 is generally insoluble in water, including in acidic conditions. It is only slightly soluble in water due to the reaction with water forming a small amount of HCO3- (bicarbonate) ions and a weak carbonic acid. The acidity of the solution does not increase the solubility of CaCO3 significantly compared to pure water.

5. PbSO4 (Lead(II) Sulfate): PbSO4 is generally considered insoluble or slightly soluble in water, including in acidic conditions. The solubility of PbSO4 is not affected significantly by the acidity of the solution.

In summary, AgBr is the compound that will be more soluble in an acidic solution compared to pure water.