[pt999]

Hello! I have been assigned a review for topics 3.7 through 3.13. I am stuck on an FRQ, question 4c to be specific. The information I have been given is as follows

"After the experiment, the student learns that the precipitate,  AgCl(s) , is slightly soluble in water. To determine the solubility, the student mixes a sample of the precipitate with warm, distilled water to make a saturated solution. The student finds the following equation for the dissolution of  AgCl(s)  in water and a  Ksp  value at the temperature of the water.

AgCl(s)⇄Ag+(aq)+Cl−(aq)                    Ksp=4.0×10−10"

The information I have already is: 1.46 grams of AgCl, 0.0102 mols of AgCl, and 0.05 M Ag. The AP videos did not cover these kinds of equations yet, so I am very lost. Any help is appreciated!

[AWK]

What should you calculate?

http://www2.ucdsb.on.ca/tiss/stretton/CHEM4/APSolubility.html

[pt999]

I think im supposed to calculate molarity, at least thats what the people on reddit said… But Im given very little information to work with

[AWK]

For the solubility product, the concentration of ions or dissolved salt in a saturated solution is usually calculated (for AgCl these are the same numbers). You are given a specially crafted solubility product so that calculations can be done without a calculator. Please read the attached link.