Chem 30 – Unit 2 Exam – Solutions and Solubility
Name____________
March 4th, 2011
Part A. Match each of the statements from the first column with a term in the second
column. Place the letter of the term in the second column in the correct blank. Each
part is worth one mark.
_____ the ability a substance has to dissolve at a specific
temperature and pressure
_____ least abundant substance in a solution
_____ two or more substances mixed together forming a
homogeneous mixture
_____ act of adding more solvent to a solution
_____ act of precipitating one ion at a time from a
solution
A.
B.
C.
D.
E.
F.
G.
H.
I.
J.
K.
_____ most abundant substance in a solution
L.
_____ a solution containing the maximum amount of
dissolved substance it can hold
dilution
concentration
molarity
precipitate
saturated
solution
selective
precipitation
solubility
solute
solution
solvent
supersaturated
solution
unsaturated
solution
_____ a solution which can still dissolve more solute
_____ a solid that forms when certain aqueous solutions are
mixed together
_____ a solution which contains undissolved solute
Part B. Problems. Answer the following questions. Each question is worth a differing
amount of marks. Questions out of 3 marks require the formula, substitution of values
into the formula with correct units, and the correct answer with sig-figs and units.
1. What is the concentration of a solution of barium nitrate that contains 12.6 g of
solute in 2.50 L of solution?
2. What volume of 12.0 M hydrochloric acid will contain 8.35 g?
3. If 0.200 g of sodium hydroxide are dissolved with water to form a 2.00 kg solution,
what is the concentration of this solution in ppm?
4. What is the final concentration when 14.0 mL of a 4.20 M Na2CO3 solution is diluted
to 86.0 mL.
5. If 200.0 mL of 0.200 M sodium sulfate is added to 800.0 mL of water, what is [Na+]
and [SO42-]?
6. Describe how you would prepare 0.500 L of an 18.0 M solution of hydrobromic
acid.
7. Using a solubility curve, answer the following questions:
a) At what temperature will 75.0g of KNO3 completely dissolve in 100.0 g of
water? Describe this solution in terms of saturation.
b) How many grams of KClO3 will dissolve in 1.00 L of water at 70.0oC? Show
your math.
8. For each of the following reactions predict the products with their states and
balance the equation. If a reaction occurs write the balanced net ionic equation. If
no reaction occurs, indicate so and state the spectator ions.
(1 mark for each product with states, 1 mark for balancing the equation, 1 mark for
balanced net ionic equation or stating no reaction with spectator ions)
a) calcium carbonate and hydrobromic acid
b) ammonium bromide and lead (II) acetate
9. Pb(NO3)2, Sr(NO3)2, and Mg(NO3)2 are all mixed together in an aqueous solution.
Create a table to determine the order must you add NaOH, HCl, and (NH4)2SO4 to
selectively precipitate each original cation out individually. Which precipitates will
form with each solution added?
Order
Precipitate