Do you expect the solubility of in 0.1 M to be equal to, greater than, or less than that of in water? Explain
To determine whether the solubility of a compound A in 0.1 M solution of another compound B is expected to be equal to, greater than, or less than its solubility in water, we need to consider the concept of common-ion effect.
When a compound dissolves in a solvent such as water, it dissociates into ions. The solubility of a compound is affected by the presence of common ions in the solution, which can either enhance or reduce its solubility.
In this case, we are comparing the solubility of compound A in a 0.1 M solution of compound B to its solubility in water. If compound B ionizes or dissociates in water to produce ions that are also present in the compound A, we can expect the solubility of compound A in the 0.1 M solution of B to be *less than* its solubility in water.
This is because the presence of a common ion from compound B in the 0.1 M solution will increase the concentration of that ion in the solution. According to Le Chatelier's principle, when the concentration of a common ion increases, it shifts the equilibrium of the dissolution reaction of compound A to the left, reducing the solubility of compound A.
On the other hand, if compound B does not produce any common ions with compound A when dissolved in water, the solubility of compound A in the 0.1 M solution of B would be *equal to* its solubility in water. This is because there are no additional ions in the solution that can affect the equilibrium of compound A's dissolution.
In summary, to determine whether the solubility of compound A in the 0.1 M solution of compound B is expected to be equal to, greater than, or less than its solubility in water, we need to consider whether compound B produces any common ions with compound A when dissolved in water.