Solutions Practice Test
1) Which of the following would INCREASE as the concentration of solute increases?
a) osmotic pressure only
c) boiling point and osmotic pressure
b) vapor pressure only
d) freezing point only
2) What mass of C12H22O11 is needed to make 2000 mL of a 0.35 M solution?
3) During a lab, Kelly needs 255 mL of 6.0 M hydrochloric acid. Because she spilled some on
the floor, she only has 115 mL of the 6.0 M acid left. Instead of telling Mrs. Gannon about the
spill, she just added the acid he had left to some distilled water to make 255 mL of solution.
What is the molarity of this new solution?
M1V1 = M2V2
5) What is the boiling point of an aqueous 0.200m AlBr3 solution?
6) What is “moles solute/kilograms solvent”
a) mole fraction solute
b) molarity
c) molality
d) % mass solute
7) What is the molarity of a solution that has 11 moles of solute in 585 mL of solution?
8) How many grams of KBr are needed to make 125.0 L of 0.850 M solution?
9) What type of property depends on the amount of solute particles but not their nature?
_________________________________________
10) What do we call the substance that dissolves in another substance? _________________
11) The sum of these in a solution is always equal to one hundred.
a) ppm
b) molarity
c) mass percent
d) mole fraction
12) Menards is having a sale on salt used to de-ice driveways and sidewalks. All bags are
$2.00 and contain 1000 moles of salt. Being a smart shopper you check out the ingredient
for each brand. Which brand will melt the most ice?
a) SUPER MELT— AlCl3
b) MELT ALL— KCl
c) MAMA’S MIGHTY MELT— CaCl2
13) As the solvent evaporates, what happens to the boiling point of a solution?
______________________________
14) Jeremy does a freezing point depression lab and collects the following data:
mass solvent = 150.25 g
mass unknown = 15.55 g
freezing point solvent = 65.2 oC
freezing point solution = 62.3 oC
Kf of solvent = 15.5 oC/m (from the Handbook of Chemistry and Physics 55th Edition)
The unknown does not conduct electricity when dissolved in water.
What is the molar mass of the unknown?
15) The boiling point of 1000 g of water would be raised most by adding 25 grams of:
a) KOH
b) KBr
c) Al(NO3)3
d) C2H5OH
16) Andrew is supposed to make a sugar solution in lab, so he adds sugar to a beaker of
water. Ooops! He didn’t measure the volume of the water OR the mass of sugar that he put
into the solution. Nooree is fuming, because he has used up all of the sugar that they were
allowed to use for the day. But little did anyone know, Andrew has been studying solutions
intensely and decides to measure the vapor pressure of the solution that he has made. It is
20.5 torr. If the vapor pressure of pure water at 25 oC is 23.8 torr.
a) What is the mole fraction of sugar in this solution?
b) What is the boiling point of this solution? (sugar = C12H22O11)
c) If the density of water is 1 g/ 1 ml, what is the osmotic pressure of this solution?