Solubility Review Name ________________ 1. What is the [Ba2+] and [Cl-] in a 1.5 M solution of BaCl2? 2. What is a saturated solution? 3. What is another term for the concentration of a saturated solution? 4. How can you increase the solubility of a solution? 5. How would you make a saturated solution of CaSO4? 6. Consider the following 2 solutions: 1.0 M Na3PO4 and 2.0 M NaCl. Which solution would have the greatest conductivity and why? 7. Write the balanced formula equation, total ionic equation and net ionic equation including all states for the reaction of : PbCl4 (aq) + Cu2SO4 (aq) 8. Consider a saturated Pb(OH)2 solution at equilibrium. Explain what the following would do to the position of equilibrium and the reaction rates. Pb(OH)2 (s) ↔ Pb2+(aq) + 2 OH-(aq) a. adding NaOH b. adding Pb(NO3)2 c. adding Pb(OH)2 d. cooling the mixture down e. adding Mg(NO3)2 f. adding 1.0 M HNO3 (an acid) 9. A chemist has a solution which may contain any or all of: Ca2+ Pb2+ Mg2+ To test this, the chemist : a. adds Na2S and a precipitate appears, which is filtered b. adds Na2SO4 to the filtered solution and nothing happens c. adds 1.0 M NaOH to the solution and a white precipitate appears. Which ion(s) were present in the original solution? 9. A chemist removes 10.00 mL of a hot saturated Mg(OH)2 solution and evaporates the 10.00 mL sample to dryness. The mass of the dry residue is 0.4505 g. a. What is the solubility of Mg(OH)2 in mol/L? b. What is the [Mg2+] and [OH-] in the saturated solution? c. What is the equilibrium constant expression for this equilibrium? d. What is the Ksp of Mg(OH)2 at this temperature?