Question

For which of the following pairs of salts could you compare their solubility using only their ksp values?

1) Salt 1: NaCl, Salt 2: KCl
2) Salt 1: CaCO₃, Salt 2: MgCO₃
3) Salt 1: AgCl, Salt 2: AgBr
4) Salt 1: FeCl₃, Salt 2: Fe₂⁺(SO₄)3

Answer 1

The solubility of salts can be compared using their Ksp values. We can compare the solubility of Salt 1: NaCl and Salt 2: KCl because they are both alkali metal salts. We can also compare the solubility of Salt 1: AgCl and Salt 2: AgBr because they both contain the same metal cation (Ag+) with different anions. However, we cannot accurately compare the solubility of Salt 1: CaCO₃ and Salt 2: MgCO₃ using only their Ksp values.

Step-by-step explanation:

The solubility of salts can be compared using their Ksp values, which represent the solubility product constant. The larger the Ksp value, the more soluble the salt is. Therefore, we can compare the solubility of salts by comparing their Ksp values.

In the given options, we can compare the solubility of Salt 1: NaCl and Salt 2: KCl because they are both alkali metal salts and can have similar solubility trends. Similarly, we can compare the solubility of Salt 1: AgCl and Salt 2: AgBr because they both contain the same metal cation (Ag+) with different anions. However, we cannot compare the solubility of Salt 1: CaCO₃ and Salt 2: MgCO₃ because they are different compounds and their solubility cannot be accurately determined by only their Ksp values.

Therefore, the correct pair of salts for comparing solubility using only Ksp values is Salt 1: NaCl and Salt 2: KCl, which are both alkali metal salts.