Chapter 20 Concentration. Molarity (M) Moles of solute per liter of solution. Molarity = moles of solute liters of solution.

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Presentation transcript:

Chapter 20 Concentration

Molarity (M) Moles of solute per liter of solution. Molarity = moles of solute liters of solution

What is the molarity of a solution prepared by dissolving 21.0 g of CaCl 2 in mL of solution?

0.378M CaCl 2

What is the molarity of a solution prepared by dissolving 48.4 g of CaCl 2 in mL of solution?

4.36M CaCl 2

molality (m) Moles of solute per kilogram of solvent. molality = moles of solute kg of solvent

What is the molality of a solution prepared by dissolving 92.3 g of KF in 100.0g of water?

15.9m KF

What is the molality of a solution prepared by dissolving 20.0g of NH 4 Cl in 400.0g of water?

0.935m NH 4 Cl

Mole Fraction (X) moles of component per total moles of solution. mole fraction = moles of component total moles in solution Note: The mole fractions of the solute and solvent add up to “1”

What is the mole fraction of C 4 H 10 O in a solution containing 75.6g of C 10 H 8 and 600.0g of C 4 H 10 O?

X C 4 H 10 O = 0.932

What is the mole fraction of C 2 H 6 O in a solution containing 67.4g of C 9 H 7 N and 200.0g of C 2 H 6 O?

X C 2 H 6 O = 0.893

Percent Solution by mass Represents the number of grams of solute per 100 grams of solution. % solution = mass of solute mass of solution X 100

A solution contains 130g of HCl in 750g of water. What is the percent by mass of this HCl solution?

14.8% HCl

What is the mass percent of a solution containing 67.4g of C 9 H 7 N in 200.0g of C 2 H 6 O?

25.2% C 9 H 7 N

Homework Worksheet: Concentration