Chemistry 11
Name: __________________________________________
Unit 5: Solubility Review
1. Distinguish between the terms solvent and solute.
2. With respect to polarity, explain the phase “like dissolves like”.
3. Water is a polar molecule. What does this mean?
4. Why is water a liquid rather than a gas at room temperature?
5. For each compound, write the dissociation equation for each as they dissolve in water. Also, calculate
the molarity of the individual ions. Note, you may first have to calculate the molarity of the compound
or determine the formula. The first one is done for you.
Compound
Sr(OH)2
0.44 M
AlBr3
0.030 M
(NH4)2C2O4
1.50 M
beryllium sulfide
0.050 M
sodium phosphate
0.300 M
ammonium carbonate
2.34 M
NiI2
10.00 g in 150.0 mL
Dissociation Equation and Ion Concentration
Sr(OH)2(s)  Sr2+(aq)
+
2 OH-(aq)
0.44 M
0.88 M
Chemistry 11
Name: __________________________________________
6. When 1.50 L of 0.600 M NaI(aq) is mixed with 2.50 L of a 3.00 M CaI2(aq), no reaction occurs.
Calculate the concentration of each ion in the new solution after mixing.
7. When 8.00 L of 1.00 M solution of MgCl2(aq) is mixed with 2.00 L of a 5.00 M solution of AlCl3(aq),
no reaction occurs. Find the concentration of each ion after mixing.
8. When 25 mL of a 5.00 M solution of FeBr2(aq) is mixed with 75 mL of a 2.00 M solution of CrBr3(aq),
no reaction occurs. Calculate the concentration of the bromide ion after mixing.
9. Use the table “Solubility of Common Compounds in Water” to determine whether each of the following
is soluble (S) or has low solubility (LS).
AgCl
Al2(CO3)3
CuCl2
NaOH
CuI
______
______
______
______
______
FeS
Na3PO4
FeSO4
Fe(NO3)3
Cr(OH)3
______
______
______
______
______
10. Determine whether 0.2 M solutions of the following mixtures form a precipitate
when mixed, and give the formula of any precipitate.
a. AgNO3(aq) and NH4Br(aq)
b. SrBr2(aq) and NaNO3(aq)
c. KOH(aq) and AlCl3(aq)
d. NaI(aq) and Pb(NO3)2(aq)
Chemistry 11
Name: __________________________________________
11. Write and balance the formula equation, complete ionic equation and net ionic equation for the
following: (Show states.)
a)
AgNO3(aq) + Na2CO3(aq)

b) silver nitrate solution and sodium chloride solution
12. A solution of NaF is prepared. A 25.00 mL sample of the solution is placed into a
test tube. The solution is then heated in the test tube over a Bunsen burner until all the water has
evaporated. The empty test tube has a mass of 96.32 g. With the sodium fluoride residue in it, the total
mass is 104.61 g. Find [NaF].
13. Oil is a non-polar liquid. Explain why NaCl(s) will not dissolve in oil.