CH 17-18 REVIEW
1. A clear solution of silver nitrate is mixed with a
solution of sodium chloride and a white precipitate
forms.
a.
a.
a.
Write a balanced equation for this reaction.
AgNO3 + NaCl  NaNO3 + AgCl(s)
Write a complete ionic equation.
Ag+ + NO3- + Na+ + Cl-  AgCl (s) + Na+ + NO3Write a net-ionic equation
Ag+ + Cl-  AgCl (s)
2. Define the following:
a. Hydrogen bonds – a weak bond between hydrogen
and an element with a higher electronegativity
b. Hygroscopic – salts and other compounds that remove
moisture from the air
c. Desiccant – drying agents
d. Deliquescent – remove water from the air to dissolve
completely to form solutions
e. Efflorescent – process at which the hydrate losses
water of hydration
3. Water is a polar solvent; gasoline is a nonpolar
solvent. Decide which compounds are more likely
to dissolve in water and which are more likely to
dissolve in gasoline?
a. Sucrose (C12H22O11) will dissolve in water
b. Na2SO4 will dissolve in water
c. Methane (CH4) will dissolve in gas
d. KCl will dissolve in water
4. Match each term with the following descriptions. A description may
apply to more than one term.
a. True solution
b. Colloid
c. Suspension
(1)
Does not settle out on standing a, b
(2)
Heterogeneous mixture b, c
(3)
Particle size less than 1.0nm a
(4)
Particles can be filtered out c
(5)
Demonstrates the Tyndall Effect b, c
(6)
Particles are invisible to the unaided eye a, b
(7)
Homogeneous milk b
(8)
Salt water a
(9)
Jelly b
5.
Name and distinguish between the two components
of a solution.
solute – substance being dissolved
solvent – substance doing the dissolving
6.
Explain the difference between miscible and
immiscible. Provide examples of each.
miscible – 2 liquids that will dissolve in each other
Ex. Water and vinegar
immiscible – 2 liquids that will not dissolve in each
other
Ex. Water and oil
7.
Explain the difference between an unsaturated,
saturated and supersaturated solution.
Unsaturated – contains less than the maximum amount
of solute dissolved at a given temperature
Saturated – contains the maximum amount of solute
dissolved at a given temp.
Supersaturated – contains more than the maximum
amount of solute at a given temp
8.
What mass of KNO3 can be dissolved into100 g
of water at 20oC. (use Figure 18.4 on page 504)
About 27 grams
9. The solubility of methane, the major component of
natural gas, in water at 20oC and 1.00 atm of
pressure is 0.026 g / L. If the temperature
remains constant, what will be the solubility of this
gas at the following pressure?
a. 0.60 atm
b. 1.80 atm
0.016 g / L
0.047 g / L
10. Calculate the molarity (M) of each solution:
a.
b.
1.0 mol KCl in 750 mL of solution 1.3 M
0.50 mol MgCl2 in 1.5 L of solution 0.33 M
11. Calculate the moles and grams of solute in each
solution:
a.
b.
1.0 L of 0.50M NaCl 0.50 mol and 29 grams
5.0 x 102 mL of 2.0M KNO3 1.0 mol and 100. grams
12. What is the concentration (in % m/v) of the
following solutions:
a. 20.0 g KCl in 0.60 L of solution 3.3%
b. 32 g NaNO3 in 2.0 L of solution
1.6%
HINT: (m / v) = mass / vol
(g / mL)
13. What is the freezing point of each solution?
a. 1.40 mol Na2SO4 in 1750 g H2O
b. 0.060 mol MgSO4 in 100 g H2O
-4.46 oC
-1.1 oC
14. Determine the freezing points of each 0.20m
aqueous solutions. (use the Kf for water)
a.
b.
c.
K2SO4 -1.1 oC
CsNO3 -0.74 oC
Al(NO3)3 -1.5 oC