Solutions Review WS
Name__________________________________Per. _____
1. __solute_______ gets dissolved in the _solvent____ to make a _solution_______. (choices: solvent,
mixture, solution, suspension, colloid, solute)
2. A can of soda is an example of a __gas/liquid_____ solution. (gas/liquid, liquid/liquid, solid/liquid,
gas/gas). The _gas______ is the solute and the water is the _solvent__________.
3. When the soda tastes “flat” we mean there is less ________________in it.
4. Adding more solute to a solution _increases________ the concentration. But, increasing the solvent
in a solution ___decreases______ the concentration. (agitates, decreases, evaporates, increases)
5. Name 3 things that increase the rate of solution (think sugar cubes in water):
a)________increasing heat________________
b)________increasing surface area of solute___
c)_________agitation (stirring)______________
6. The rate of solution is increased because there are more _collisions__________ between molecules of
solute and solvent. (collisions, vapor pressures, colligative properties).
7. What are 2 properties of water resulting from hydrogen bonding: ___surface tension___ and __high
boiling point, cohesion/adhesion, capillary action…___
8. In what type of mixture is the rate of solution actually decreased when heat is applied?
____gas/liquid_______________ (solid/liquid, gas/liquid, liquid/liquid)
9. How many moles of solute would be needed to form 1 liter of a 3 M solution of NaCl?
(Hint: what is the definition of M (Molarity)?)
a. 1 mole
b. 3 moles
c. 1/3 moles
Recall the definition of Molarity = moles solute /L solution
3 M = x/1 L x = 3 moles
10. A student adds 0.5 moles of solute to enough water to form 500 ml of solution. What is the
concentration of the solution this student made?
a.
0.1 M
b. 0.2 M
c. 1 M
.5 moles/.5 L = 1 Molar
d. 2 M
11. Adding antifreeze to a car’s radiator increases the boiling point of the solution. T or
F
12. Adding a solid solute to a solvent ____d________.
a. Raises the freezing point of the solution
b. Raises the vapor pressure of the solvent
c. Lowers the boiling point of the solution
d. None of the above
13. Which one of these decreases as the amount of solute particles in a solution increases? (Hint:
osmotic pressure increases as solute particles increase).
a. Osmotic pressure
b. molality
c. freezing point
d. boiling point
14. From the table below, which solute would lower/raise (circle one) the boiling point the most?
__________Na2CO3____________________
Explain why:___When dissolved in water it has 3 particles
(2 Na+ ions and 1 CO3 2- ion)
15. True or False: A suspension is an example of a heterogeneous mixture?
16. How many grams of NaCl are dissolved in 500.0 mL of a 0.0500 M solution of NaCl?
0.0500 M = x/.500 L x=0.25 moles NaCl convert to grams  0.25 x 58.45 g/mol = 1.46 g NaCl
17. Which of the following is not a colligative property?
a. Freezing point depression
b. Boiling point elevation
c. Vapor pressure lowering
d. Increasing solubility
18. Calculate the freezing point of a solution that contains 8.0 g of sucrose (C12H22O11) in 100.0 g of H2O.
Kf for H2O = 1.86°C/m
(Hint: subtract the temp change from the freezing pt. of water)
Sucrose = 1 particle molar mass of sucrose = 342.3 g/mol
Calculate molality:
moles sucrose = 8.0/342.3 = 0.023
m = moles/kg solvent = 0.023 / .100 kg water = 0.23
Use delta T = Kf x i x m = (1.86)(1)(0.23) = 0.43 oC
The new freezing point is 0-0.43 = -0.43oC
19. A 6.600 g sample of a solute is dissolved in 105.0 g of water. The molar mass of the solute = 58.5
g/mol. The solute dissociates into 2 particles. Calculate the new boiling point of the solution. Kb for
water = 0.512°C/m. (Hint: you must add the temperature change you calculate to the normal bp of
water!)
6.600 g/58.5 = 0.1128 moles solute molality = 0.1128/0.105 kg = 1.07
Delta T = Kim = (0.512)(2)(1.07) = 1.1oC New boiling pt = 100 + 1.1 = 101.1oC
20. What is the molarity of a solution that contains 20.45 g of sodium chloride (NaCl) dissolved in 700.0
mL of solution?
20.45/58.44g/mol = 0.3499 moles Molarity = moles/ L = 0.3499/0.700 L = 0.5 M
21. A 22.0-mL sample of 12M H2SO4 is diluted to a volume of 1200.0 mL. What is the molarity of the
diluted solution?
M1V1 = M2V2 (12M)(22.0 mL) = M2(1200.0mL)
M2= 0.22 M
22. A mass of 134 g of manganese (II) bromide (MnBr2) is dissolved in 225 g of water. What is the
molality of the solution?
134/214.75 = 0.624 moles MnBr2
molality = 0.624/.225 kg = 2.77m
23. Calculate the molality of a solution that contains 106 g naphthalene (C10H8) dissolved in 3.15 kg of
carbon tetrachloride (CCl4).
106 g/128.17 g/mole = 0.827 moles
molality = 0.827/3.15 kg = 0.263 m
24. What volume, in milliliters, of a 1.15M stock solution of potassium nitrate is needed to make 0.75 L of
0.578M potassium nitrate?
(1.15)(V1) = 0.578 (0.75)
V1= 0.377 L or 377 mL
25. Suppose you wished to make 0.879 L of 0.250M silver nitrate by diluting a stock solution of 0.675M
silver nitrate. How many milliliters of the stock solution would you need to use?
(0.675)(V1)=0.250(0.879)
V1= 0.326 L or 326 mL
26. If 55.0 mL of a 2.45M stock solution of sucrose is diluted with water to make 168 mL of sucrose
solution, what is the molarity of the final solution?
2.45(55.0) = M2(168)
M2=0.802 M
27.
What is the molality of a solution that contains 16.3 g of potassium
chloride dissolved in 845 g of water?
16.3 g/(74.55g/mole) = 0.219 moles
molality = 0.219/.845kg = 0.259 m
28.
What are the boiling and freezing points of a 1.34m water solution
of calcium chloride (CaCl2)? Kb for water = 0.512°C/m and Kf for water =
1.86 oC/m
CaCl2= 3 particles; delta T = Kf i m = 1.86x3x1.34= 7.48oC
New freezing point = 0 -7.48 = -7.48oC
For boiling: Kb I m = 0.512 x 3 x 1.34 = 2.06oC
New boiling point = 100 + 2.06 = 102.06oC
37. Four mixtures having the following properties are examined. Identify each mixture as a solution, a suspension, or a
colloid. If the properties are not conclusive for identification, state which types of mixtures are possible.
a. quickly settles out into a watery liquid and an oily liquid ______suspension________________
b. solution scatters the light from a flashlight beam ________colloid_____________________
c. is transparent and does not scatter the light from a flashlight beam solution____________________
38. What is the difference between a 2M solution and a 2m solution?
2M means 2 moles/ L solution and 2m means 2 moles/kg solvent
39. Define colligative property, and identify four colligative properties.
Colligative property: a colligative property is a physical property of a solution that is affected by the number of dissolved
solute particles in the solution
1.
boiling point elevation
2. Freezing point depression
3.
Vapor pressure lowering
4. Change in osmotic pressure
40. Would you expect the freezing point depression of a 1m-solution of sucrose and that of a 1m-solution of sodium
chloride to be the same? Explain
No because NaCl dissociates into 2 particles per formula unit and sucrose does not dissociate so it only has 1 particle
per molecule. NaCl would have a bigger effect on freezing point lowering than sucrose.
For problems 42.-48. Write how many particles of solute will form.
SOLUTE
41.
42.
43.
44.
45.
46.
47.
CaCl2
N2
CO2
AgNO3
Mg3(PO4)2
CaSO4
C6H12O6
# OF
PARTICLES
3
1
1
2
5
2
1