Review – Part I
Here is a sample of the items we covered this unit with some questions to go along with them.
a. Writing solubility product expressions.
1. Write a balanced equation showing the dissociation of PbBr2. Then write the Ksp expression for the
salt.
b. Calculating Ksp when given molar solubility.
c. Calculating Ksp when given a solubility that must be first converted to molar solubility.
2. At a given temperature, 2.12 x 10-3 g of magnesium fluoride, MgF2(s) can dissolve in 125.00 ml of
solution. Determine Ksp for magnesium fluoride at this temperature.
d. Calculate solubility given Ksp.
3. The Ksp for copper (I) chloride is 1.73 x 10-7. What would be the maximum ion concentrations when
copper (II) chloride is dissolved in pure water.
e. calculating pH from solubility data (see example from powerpoint on day 2).
f. The common-ion effect.
4. What is the molar solubility of lead (II) chloride, PbCl2(s) with Ksp = 1.7 x 10-5, in i) pure water and ii) a
solution of 0.0185 mol/L sodium chloride (iii) explain the difference between the answers in i) and ii).
g. predicting whether or not a precipitate will form.
5. Will a precipitate form when 125.00 ml of 3.5 x 10-4 mol/L copper (I) nitrate, CuNO3(aq) is mixed with
75.00 ml of 8.1 x 10-4 mol/L sodium chloride, NaCl(aq)? The Ksp for copper chloride, CuCl(s), is 1.7 x 10-7.
Justify your answer.
h. theories of acids and bases.
i) conjugate acid-base pairs.
6. What would be the conjugate acid of CH3-(aq)?
j. calculating pH, pOH, [H3O+] from pH or pOH, [OH-] from pH or pOH.
7. Calculate the [OH-] of a solution that has a pH of 2.40.
k. auto-ionization of water and Kw