Super Duper Solutions Review
Name _________________________ Pd ______
Use the terms below to complete the passage.
aqueous
immiscible
liquid
insoluble
miscible
soluble
solute
solution
solvent
All (1) _ solutions _ are homogeneous mixtures. Since air is 20% oxygen and 79% nitrogen
air is a(n) (2) _ solution _ of oxygen gas dissolved in nitrogen gas. The oxygen in air is the
(3)_ solute _, and nitrogen is the (4) _ solvent _. Because oxygen gas dissolves in a solvent,
oxygen gas is a(n) (5) _ soluble _ substance. A substance that does not dissolve is (6) _
insoluble _. (7) _ Liquid _ solutions are the most common type of solutions. If one liquid is
soluble in another liquid, such as acetic acid in water, the two liquids are (8) _ miscible _.
However, if one liquid is insoluble in another, the liquids are (9) _ immiscible _.
10. Fill in the following blanks with the word polar or the word nonpolar or the word ionic:
a. Polar molecules can only dissolve other _ polar _ molecules or _ ionic _ compounds
b. Nonpolar molecules can only dissolve other _ nonpolar _ molecules.
c. Polar molecules WILL NOT dissolve _ nonpolar _ molecules.
11. Fill in the chart with the appropriate information.
Compound
C6H12O6
Ionic or Covalent?
Polar or Nonpolar?
C
Nonpolar (Slightly polar)
I
Will dissolve
better in…
H2O
Oil
X
X
(somewhat)
NH3
C
Ionic – polar nonpolar
X
refers to covalent molec.
P
X
C6H14
C
N
MgCl2
X
12. Fill in the following blanks with one of the following terms: soluble, insoluble, immiscible, miscible.
a. Chalk will not dissolve in water. It is said to be _ insoluble _.
b. Oil will not dissolve in water. It is said to be _ immiscible _.
c. Sucrose (sugar) will dissolve in water. It is said to be _ soluble _.
d. Lemon juice will dissolve in water. It is said to be _ miscible _.
e. _ Miscible _ and _ immiscible _ refer to solutions made of two liquids.
13. Water allows many substances to dissolve in it because of its polar nature.
It is often referred to as the _ Universal Solvent _.
In a(n) _ aqueous _ solution, water is the solvent.
Directions: Use the graph below to answer 14 - 25. SHOW ALL WORk for Calculations!!!
14. How much sodium nitrate is dissolved in
100 g of water at 60C?_ 124 g + 2 g_
15. How much ammonium chloride is
dissolved in 100 g of water at 10C?
_ 35 g _
16. What is the mass of KNO3 than can
dissolve in 800 g of water at 50C?
_ 640 g _
17. What is the minimum mass of water at
100C needed to dissolve 80 g NaCl?
_ 200 g H2O_
18. If 50 g of ammonium chloride is
dissolved at 40C, is the solution saturated,
unsaturated or supersaturated?
_ supersaturated _
19. If 70 g of KNO3 is dissolved at 60C,
how much more solute can be added
before the solution becomes saturated?
100-70 = 30 g KNO3
20. At 50C, 115 g of sodium nitrate is dissolved. If the solution is cooled to 10C,
how much solute will precipitate out of solution?
_5 g_
21. What happens to the solubility of a solid as temperature increases?
_ increases _
22. What happens to the solubility of a gas as temperature increases?
_ decreases _
Refer to the solubility graph and tell if the solution described is unsaturated (US),
saturated (S) or supersaturated (SS)
22. 100 g KNO3 in 100 grams of water at 50OC __ SS __
23. 50 g KCl in 100 grams of water at 80OC __ S _
24. 50 g KCl in 200 grams of water at 80OC _ US __
25.
70 grams of ammonium chloride at 90OC _ SS _
Use the terms unsaturated (US), saturated (S) or supersaturated (SS) to identify
each solution described below:
26. When more solute is added the additional solute “disappears” _ US _
27. When a crystal of solute is added the excess precipitates out _ SS _
28. When more solute is added the additional solute just falls to the bottom _ S _
29. A solution containing more solute than it “should” be able to hold at that temperature _ SS _
30. A solution containing exactly the amount of solute the graph shows it can hold at a specific
temperature __ S _
31. A solution containing less solute than it can hold at a specific temperature _ US _
Solution Concentration
32. Determine the molarity of a 1000 mL solution containing 3.5 mol of sodium nitrate. 3.5 M
33. Calculate the number of grams of silver(I) nitrate (AgNO3) needed to make 200 L of a 4M
solution. 800 mol = 169.9 g/mol AgNO3 = 135,968 g
34. Calculate the volume of a 0.25M solution containing 20 g of NaOH. 0.5 mol NaOH
35. Calculate molarity of a solution containing 20 g of sodium oxide (Na2O) in 200 mL of solution.
Is this solution dilute or concentrated? 1.6 M dilute
Solution Dilution
M1V1 = M2V2
36. What will be the final concentration of the solution indicated that will result from the
following dilutions?
a. 14.0 mL of a 4.20 M Na2CO3 solution is diluted to 86.0 mL.
M2 = 0.68 M
b. 450. mL of a 1.22 M HCl solution is diluted to 1.26 liters.
M2 = 0.436 M
37. To what volume should the indicated solution be diluted to produce a solution of the
desired concentration?
a. 12.0 mL of a 0.64 M KCl solution to produce a 0.19 M solution.
V2 = 40.4 mL
b. 84.2 mL of a 4.60 M KMnO4 solution to produce a 1.42 M solution. V2 = 272.8 mL
38.
What volume of the indicated solution is needed to produce the volume and concentration
of a diluted solution as indicated?
a. 2.73 M NaOH solution to prepare 142 mL of a 0.540 M solution.
V1 = 28.1 mL
b. 0.0076 M SnF2 solution to prepare 25.0 mL of a 0.00027 M solution.
V1 = 0.964 mL
Colligative Properties
39. What is Freezing Point?
How does adding a solute to a pure solvent influence freezing point of the solution?
Lowers Freezing Point
40. What is Boiling Point?
How does adding a solute to a pure solvent influence boiling point of the solution?
Raises Boiling Point
More:
41. Circle all of the following solutes that will dissolve in H2O
a. KBr
b. NaCl
c. CH4 (nonpolar)
d. NH3 (polar)
42. Nonpolar solutes dissolve in _ nonpolar _ solvents
43. The unit used for molarity (molar concentration) is __ Molar ___ _ M _
44. _ 1000 _ mL = 1 L
45. Identify the solute and solvent in a liquid solution of sugar water:
Solute: _ Sugar _
Solvent: _ Water _
46. Explain the difference between a solution, a colloid and a suspension. Identify each as
homogeneous or heterogeneous.
The primary difference is the size of the solute or suspended particle.
- Solutions have the smallest particles and are homogeneous – solute particles
and solvent particles are the same size.
- Colloids are heterogeneous; the particles are still very small and stay
suspended in the solvent but they are large enough to reflect light (Tyndall
Effect)
- Suspension particles are so large that they settle out, making a suspension a
heterogeneous mixture