addition of a strong acid would increase the solubility of which of the following salts
AgCl
CaSO4
CdS
CaCO3
PbBr2
CaHPO4
Cd(OH)2
AuCl
Strong acid will increase the solubility of any of the salts in which the anion is a base that reacts with the H^+. For example, CaSO4 will be increased with strong acid because the SO4^-2 reacts as follows:
SO4^-2 + H^+ ==> HSO4^-
and this is k2 for the reaction. k2 = 1.2E-2. It will NOT increase solubility of PbBr2 because Br^- + H^+ ==> HBr is a strong acid itself. As an added piece of information, and one which I'm relatively certain is not one of the answers, if the strong acid is HCl, the solubility of all of the salts you have identified above plus the AgCl and AuCl will increase because of the formation of complex ions if the HCl is concentrated HCl. AgCl2^-, AgCl3^-2 are two of the complexes with Ag ion. AuCl reacts in a similar fashion.
Ah, the joys of chemistry! If we're talking about increasing solubility, let me think... Ah, got it! It's like turning up the heat on a cold day. Adding a strong acid can increase the solubility of some salts, namely CaCO3, PbBr2, and CaHPO4. So those are the lucky ones that'll dissolve like a dream with a friendly acid around!
The solubility of salts can be affected by the addition of a strong acid. A strong acid will increase the solubility of salts with anions that are basic in nature. Based on this, the strong acid would increase the solubility of the following salts:
1. AgCl: No effect. AgCl is an insoluble salt and remains unaffected by the addition of a strong acid.
2. CaSO4: No effect. CaSO4 is a sparingly soluble salt and remains unaffected by the addition of a strong acid.
3. CdS: No effect. CdS is an insoluble salt and remains unaffected by the addition of a strong acid.
4. CaCO3: No effect. CaCO3 is a sparingly soluble salt and remains unaffected by the addition of a strong acid.
5. PbBr2: No effect. PbBr2 is an insoluble salt and remains unaffected by the addition of a strong acid.
6. CaHPO4: No effect. CaHPO4 is a sparingly soluble salt and remains unaffected by the addition of a strong acid.
7. Cd(OH)2: Solubility will increase. Cd(OH)2 is an insoluble salt, but upon addition of a strong acid, it will dissolve to form Cd2+ ions since they are acidic.
8. AuCl: Solubility will increase. AuCl is an insoluble salt, but upon addition of a strong acid, it will dissolve to form AuCl4- ions since they are acidic.
Therefore, the addition of a strong acid would increase the solubility of Cd(OH)2 and AuCl.
To determine which of the given salts would have an increased solubility when a strong acid is added, we need to consider the concept of common ion effect.
The common ion effect states that the solubility of a salt is reduced when a common ion is present in the solution. In other words, if an ion that is already present in the salt is also present in the solution, the solubility of the salt will decrease.
When a strong acid is added, it dissociates completely into its respective ions. Therefore, we need to identify the ion that is common between the strong acid and each of the given salts.
Let's go through each of the salts and determine whether the addition of a strong acid would increase their solubility:
1. AgCl: Adding a strong acid like HCl would increase the concentration of chloride ions (Cl-) in the solution. Since AgCl contains the chloride ion, the presence of additional chloride ions from the strong acid would decrease the solubility of AgCl.
2. CaSO4: Adding a strong acid would release hydrogen ions (H+) and sulfate ions (SO4^2-) in the solution. Since CaSO4 does not contain a common ion with the strong acid, the solubility of CaSO4 would not be affected significantly.
3. CdS: Adding a strong acid would release hydrogen ions (H+) and sulfide ions (S^2-) in the solution. Since CdS contains the sulfide ion, the addition of more sulfide ions from the strong acid would decrease the solubility of CdS.
4. CaCO3: Adding a strong acid like HCl would release hydrogen ions (H+) and carbonate ions (CO3^2-) in the solution. Since CaCO3 contains carbonate ions, the addition of more carbonate ions from the strong acid would decrease the solubility of CaCO3.
5. PbBr2: Adding a strong acid would increase the concentration of bromide ions (Br-) in the solution. Since PbBr2 contains the bromide ion, the presence of additional bromide ions from the strong acid would decrease the solubility of PbBr2.
6. CaHPO4: Adding a strong acid would release hydrogen ions (H+) and phosphate ions (PO4^3-) in the solution. Since CaHPO4 does not contain a common ion with the strong acid, the solubility of CaHPO4 would not be affected significantly.
7. Cd(OH)2: Adding a strong acid would increase the concentration of hydroxide ions (OH-) in the solution. Since Cd(OH)2 contains the hydroxide ion, the addition of more hydroxide ions from the strong acid would increase the solubility of Cd(OH)2.
8. AuCl: Adding a strong acid like HCl would increase the concentration of chloride ions (Cl-) in the solution. Since AuCl contains the chloride ion, the presence of additional chloride ions from the strong acid would decrease the solubility of AuCl.
Based on the analysis above, the salt whose solubility would increase with the addition of a strong acid is Cd(OH)2.