The document provides an overview of the different ways to express the concentration of solutions, including percentages by mass, volume, molarity, and mole fraction. It includes examples and calculations for various types of solution concentrations, as well as the definitions of terms like molality and parts per million. Practical problems illustrate how to calculate the concentration based on given quantities.

1. Concentration of
Solutions
WHY WOULD SOLUTIONS BE EXPRESSED IN A CORRECT CONCENTRATION
UNITS?

2. Concentration of Solution
 It is a measure of the amount of solute in a
given amount of solvent or solution.
 One type of solution may be prepared and
expressed in different concentration.

3. Concentration of Solutions
 1. Percent by Mass
 2. Percent by Volume
 3. Percent by Mass – Volume
 4. Mole Fraction
 5. Molality
 6. Molarity
 7. Parts per Million / ppm

5. Sample Problem #1
A saline solution with a mass of
355 g has 36.5 g of NaCl
dissolved in it. What is the mass
percent concentration of the
solution?

11. Sample Problem #2
A wine contains 12% of
alcohol by volume. Calculate
the volume (in mL) of alcohol
in 350 mL of the wine.

17. Percent by Mass - Volume
What is the concentration in percent by
mass/volume of 150 mL of solution
containing 30 g of solute?

21. Sample Problem #3
A 50 mL of 12% by mass –
volume solution was used in
an experiment. How many
grams of solute does the
solution contain?

22. Solution

27. Mole Fraction
 The mole fraction (x) of a component in a solution
is equal to the number of moles of the component
divided by the total number of moles of all the
components present.
 The sum of all the mole fractions of all components
in all solution will always be equal to one (1)

29. Sample Problem
25 g of Sodium Fluoride (NaF) is
mixed with 200 g of Water (H2O).
What is the mole fraction of NaF
in the solution?

39. Molality
The molality of a solution is the number of
moles of solute per kilogram of solvent.

40. Sample Problem

41. Solution

45. Molarity
Molarity of the solution is the
number of moles of solute per
liter of solution. It is especially
useful in doing stoichiometric
calculations involving solution.

47. Sample Problem
Determine the molarity of a
solution containing 2.40 g
of Sodium Chloride (NaCl)
in 40.0 mL of solution.

52. Parts per Million/Billion
 Parts per million (ppm) expresses the number of parts of
solute per one million / billion parts of solution.

53. Sample Problem