Which of the following will be more soluble in an acidic solution than in pure water?
1.PbBr2
2.CsClO4
3.Cd(OH)2
4.Ag2(SO4)
5.BaSO3
How can I find which is which?
Could you tell me the best way to find
which one is more soluble?
Thank you!
To determine which compound will be more soluble in an acidic solution than in pure water, you need to consider the nature of the compound and how it reacts with acid. The general principle is that compounds that can undergo acid-base reactions or dissolve in acidic conditions will have enhanced solubility in an acidic solution compared to pure water.
Let's analyze each compound:
1. PbBr2: This compound is a salt and is usually insoluble in water. It will not significantly dissolve in an acidic solution.
2. CsClO4: This compound is a strong ionic compound and dissociates completely in water, making it very soluble. However, its solubility is not influenced by acidity.
3. Cd(OH)2: This compound is a base, and it can react with acidic solutions to form soluble Cd salts. Therefore, Cd(OH)2 will be more soluble in an acidic solution.
4. Ag2(SO4): This compound is a salt and is usually slightly soluble in water. However, it can form soluble silver salts in acidic conditions. Therefore, it will also have enhanced solubility in an acidic solution.
5. BaSO3: This compound is an insoluble sulfate salt and generally shows low solubility in pure water. However, it will remain insoluble in an acidic solution.
Based on this analysis, Cd(OH)2 (compound 3) and Ag2(SO4) (compound 4) are expected to be more soluble in an acidic solution than in pure water.
Remember, solubility can vary depending on specific conditions, so it's always good to consult reference materials or experimental data for accurate values.
To determine which compound will be more soluble in an acidic solution than in pure water, you need to examine the solubility rules and the effect of pH on solubility.
1. PbBr2: According to the solubility rules, most bromides (except those of Ag+, Pb2+, and Hg22+) are soluble. However, in an acidic solution, PbBr2 will be more soluble because lead(II) ions form a soluble complex with bromide ions under acidic conditions.
2. CsClO4: Perchlorates (such as CsClO4) are generally soluble in water, including both acidic and neutral solutions.
3. Cd(OH)2: Hydroxides (like Cd(OH)2) are generally insoluble, but they do dissolve to a small extent in water to form hydroxide ions. In an acidic solution, the concentration of hydroxide ions is reduced due to the acid, making Cd(OH)2 less soluble than in pure water.
4. Ag2(SO4): According to the solubility rules, sulfates are generally soluble. However, under acidic conditions, Ag2(SO4) will be less soluble. This is because silver(I) ions (Ag+) react with hydrogen ions (H+) from the acid to form insoluble silver salts (like AgCl, AgBr, and AgI).
5. BaSO3: Sulfites (like BaSO3) are typically insoluble. In both an acidic solution and pure water, BaSO3 will have limited solubility.
To summarize, PbBr2 will be more soluble in an acidic solution due to the formation of soluble lead(II) complexes. Ag2(SO4) will be less soluble in an acidic solution due to the formation of insoluble silver salts. The other compounds (CsClO4, Cd(OH)2, BaSO3) will have relatively similar solubility in both an acidic solution and pure water.
Remember to always consult solubility rules and consider the effect of pH on compounds to determine their relative solubility in different solutions.