chromate is sparingly soluble in aqueous solutions. The Ksp of Ag2CrO4 is 1.12×10−12 . What is the solubility (in mol/L) of silver chromate in 1.00 M potassium chromate aqueous solution?

Explanation:

For this question, we have to start with the ionization equation for , so:

With this in mind we can write the Ksp expression:

Additionally, for every mole of  formed, 2 moles of are formed. We can use "X" for the unknown concentration of each ion, so:

 and  

Now, we can plug the values into the Ksp expression:

Now we can solve for "X" :

I hope it helps!