% MASS
A.
What is the percent by mass of 5.0 g of
NaCl dissolved in 100 mL of water
B.
What mass of water must be added to 400.0
g of NaCl to make a 35.0% by mass aqueous
solution?
C. A chemist dissolves 4.0 g KCl and 6.5 g of NaOH
in 800.0 g of water. What is the percent concentration
of each solute in the solution?
MOLARITY
A.How many grams of sodium chloride are there in
100.0 mL of a .5 M solution?
B. How would you prepare a 2.25 x 10 2 mL of 3.00M
solution of Calcium carbonate?
C. What is the concentration of a solution that has a
volume of 1.5 L and contains 650 grams of calcium
phosphate?
MOLALITY and MOLE FRACTION
Determine the molality of 560.0 g of acetone
(CH3COCH3) in 620 g of water.
Calculate the mole fraction of a solution containing
15.0 % by mass calcium chloride
COLLIGATIVE PROPERTIES
Solvent
Water
Benzene
CCl4
Ethanol
Boiling Point
(oC)
100.0
80.1
76.7
78.5
Kb
(oC/m)
0.512
2.53
5.03
1.22
Freezing Point
(oC)
0.0
5.5
-23
-114.1
Kf
(oC/m)
1.86
5.12
29.8
1.99
222.2 g of calcium chloride are dissolved in 500 g of
water.
a. what is the molality of the solution?
b. What is the boiling point of the solution?
c. What is the freezing point of the solution?
Dilutions and Henry’s Law
A. If you have 300.0 mL of a .3 M NaBr solution,
what will the concentration by if you add 500 mL
more water to it?
B. If you dilute 350 mL lithium hydroxide to a
volume of 800 mL, what will the concentration of
this solution be?
C. If temperature stays the same, but the pressure
above the solution increases, what happens to the
solubility of the solute?
D.The solubility of a gas in water is 0.22 g/L at 20.0
kPa of pressure. What is the solubility when the
pressure is increased to 115 kPa?
DRAW AND EXPLAIN HOW/WHY
SALT DISSOLVES IN WATER.
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