Solubility Lesson 8 Review Notes

Adding a Solid to a Saturated Solution Consider the saturated solution- the rate of crystallizing equals the rate of dissolving More solid AgCl is added The solution is full so the ion concentrations remain constant Ag+ Cl- The rate of dissolving and rate of crystallizing both increase by the same amount.

Describe the change in each of the following when more solid AgCl is added to a saturated solution. Constant 1. [Ag+] 2. [Cl-] Constant Cl- Ag+ 3. Rate of dissolving Increases 4. Rate of crystallizing Increases

5. The ions in hard water are Mg2+ and Ca2+ Na2CO3 can be added to water to remove these ions

6. Calculate the total ion concentration of 1.0 M AlCl3 AlCl3  Al3+ + 3Cl- 1.0 M 1.0 M 3.0 M Total 4.0 M

7. What is the molar solubility of CaC2O4? Ksp = s2 2.3 x 10-9 = s2 4.8 x 10-5 M

8. The solubility is 7.1 x 10-5 M. The compound is: A. CaSO4 Ksp = s2 = 5.0 x 10-9 B. CaCO3

9. A solution of AgNO3 is added slowly to each of the following 0.10 M solutions. Which forms a precipitate first? A. NaCl ksp = 1.8 x 10-10 B. NaIO3 ksp = 3.2 x 10-8

10. Small amounts of AgNO3 are added to three solutions. One solution a precipitate, which one is it? does not form A. NaCl ksp = 1.8 x 10-10 B. NaIO3 ksp = 3.2 x 10-8 C. NaBr ksp = 5.4 x 10-13

11. Which solution has the greatest conductivity? A. 1.0 M NaCl B. 1.0 M CaCO3 D. 1.0 M CaCl2 1.0 M 3.0 M = 4.0 M C. 1.0 M AlCl3  Al3+ + 3Cl-  Ca2+ + 2Cl- 1.0 M 2.0 M = 3.0 M

12. Calculate the maximum number of grams BaCl2 that will dissolve in 0.50 L of 0.20 M AgNO3 solution. AgCl(s) ⇄ Ag+ + Cl- 0.20 M Ksp = [Ag+][Cl-] 1.8 x 10-10 = [0.20][Cl-] [Cl-] = 9.0 x 10-10 M BaCl2(s) ⇄ Ba2+ + 2Cl- 4.5 x 10-10 M 9.0 x 10-10 M 0.50 L x 4.5 x 10-10 mole x 208.3 g = 4.7 x 10-8 g 1 L 1 mole