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?