At 25 °C, only 0.0990 mol of the generic salt AB3 is soluble in 1.00 L of water. What is the Ksp of the salt at 25 °C? AB3(s)↽−−⇀A3+(aq)+3B−(aq)

Explanation:

Hello,

In this case, given the 0.0990 moles of the salt are soluble in 1.00 L of water only, we can infer that the molar solubility is 0.099 M. Next, since the dissociation of the salt is:

The concentrations of the A and B ions in the solution are:

Then, as the solubility product is defined as:

Due to the given dissociation, it turns out:

Regards.

c is the answer because when something is left after something evaporates that shows the chemical change.