Which of the following will be more soluble in an acidic solution than in pure water?
Be(OH)2
Ag2SO4
RbClO4
CuCN
Cul
Well, I must say, it seems these chemicals really enjoy the company of acids more than pure water. It's like they can't resist the temptation!
Out of the options you presented, Be(OH)2 will be more soluble in an acidic solution than in pure water. You know, Be(OH)2 just can't help but party when acids show up. It's like the acids bring out its inner dancing queen!
As for the others, they may not be as keen on the acid party. They might prefer the solitude of pure water. But hey, who am I to judge? We all have our preferences, right?
To determine which compound will be more soluble in an acidic solution than in pure water, we need to consider their solubility behavior in different environments.
In general, acidic solutions can dissolve compounds that are basic or contain anions that can act as weak bases. Let's analyze each compound:
1. Be(OH)2: Be(OH)2 is a basic compound that tends to dissolve better in water with a higher pH. Therefore, it is less likely to be more soluble in an acidic solution compared to pure water.
2. Ag2SO4: Ag2SO4 is a salt of silver that tends to dissolve in water regardless of its pH. Therefore, its solubility is not affected by the acidity of the solution.
3. RbClO4: RbClO4 is a salt of rubidium and perchlorate. The perchlorate anion (ClO4-) is stable and does not act as a base. Therefore, RbClO4 is not likely to be more soluble in an acidic solution than in pure water.
4. CuCN: CuCN is a compound containing the cyanide anion (CN-), which can act as a weak base. In acidic solutions, the concentration of H+ ions will increase, making it more likely to react with the CN- ion and form HCN (hydrogen cyanide) gas. This reaction helps to keep the concentration of CN- ions low, increasing the solubility of CuCN in an acidic solution compared to pure water.
5. Cul: Cul is a salt of copper(I) iodide. Similar to Ag2SO4, its solubility is not expected to be significantly affected by the acidity of the solution.
In conclusion, CuCN is expected to be more soluble in an acidic solution compared to pure water.
To determine which compound will be more soluble in an acidic solution than in pure water, we need to analyze the nature of the compounds and their behavior in acidic conditions.
First, let's understand the concept of solubility. Solubility refers to the ability of a substance, known as the solute, to dissolve in a solvent. Acids can significantly affect the solubility of different substances due to their ability to donate protons (H+ ions) to the solution.
Now, let's analyze each of the compounds and their behavior in an acidic solution:
1. Be(OH)2:
This compound is a hydroxide (OH-) and is considered a basic compound. In an acidic solution, it will react with acid to form water and a salt. Since it reacts with acid, it is not expected to be more soluble in an acidic solution than in pure water. Therefore, Be(OH)2 is not the correct answer.
2. Ag2SO4:
Silver sulfate is an ionic compound containing the sulfate ion (SO4^2-) and silver ions (Ag+). In an acidic solution, the sulfate ion is not expected to be affected significantly since it is a common ion that doesn't actively participate in acid-base reactions. The solubility of silver sulfate may change due to the formation of complex ions, but it won't increase significantly. Therefore, Ag2SO4 is not the correct answer.
3. RbClO4:
Rubidium perchlorate is a strong ionic compound consisting of rubidium ions (Rb+) and perchlorate ions (ClO4-). In an acidic solution, the perchlorate ion is not expected to be significantly affected, as it is already an anion that is stable in acidic conditions. Therefore, RbClO4 is not the correct answer.
4. CuCN:
Copper(I) cyanide is an ionic compound, and in an acidic solution, the cyanide ion (CN-) can react with the excess H+ ions to form hydrocyanic acid (HCN). The formation of hydrocyanic acid increases the concentration of cyanide ions, which can make CuCN more soluble in an acidic solution than in pure water. Therefore, CuCN is a possible correct answer.
5. CuI:
Copper(I) iodide is also an ionic compound. Like CuCN, in an acidic solution, iodide ions (I-) can react with excess H+ ions to form hydroiodic acid (HI). The formation of hydroiodic acid increases the concentration of iodide ions, which can make CuI more soluble in an acidic solution than in pure water. Therefore, CuI is a possible correct answer.
Based on the analysis above, the compounds CuCN and CuI are expected to be more soluble in an acidic solution than in pure water.