Question

Using a value of Ksp = 1.8 x 10-2 for the reaction PbCl2(s) Pb+2(aq) + 2Cl-(aq). If a solution has a current value of Keq of 1.2 x 10-2, which statement is true? Too much solid has dissolved. Additional precipitate is forming. The solution is unsaturated. The ions are now combining to reduce their concentrations.

Answer 1

Answer : The correct option is, The solution is unsaturated.

Explanation :

The relation between the solubility product and the ionic product are:

When the ionic product is greater than or equal to the solubility product then there is formation of precipitate.

`K_(eq)\geq K_(sp)`

When the ionic product is less than the solubility product then there is no formation of precipitate.

`K_(eq)<K_(sp)`

According to the question, the value of solubility product is greater than the ionic product, there is no formation of precipitate. That means the solution is unsaturated.

Hence, the he correct option is, The solution is unsaturated.

Answer 2

"The solution is unsaturated" is the statement among the following choices given in the question that is true. The correct option among all the options that are given in the question is the third option or the penultimate option. I hope that this is the answer that has actually come to your desired help.