molarity and molality copyright © 2011 pearson canada inc. slide 1 of 46 general chemistry: chapter...

Molarity and Molality

Copyright © 2011 Pearson Canada Inc. Slide 1 of 46General Chemistry: Chapter 13

Molarity (M) = Amount of solute (in moles)

Volume of solution (in liters)

Molality (m) = Amount of solute (in moles)

Mass of solvent (in kilograms)


• For dilute aqueous solutions the molality and molality of a solution are usually very similar.

• Why is this the case?

Class Examples

• 2. A solution is prepared by dissolving 44.6g of Cu(NO3)2

.6H2O(s) in enough water to make 825 mL of solution. What is the molar concentration of Cu2+(aq) ions and NO3

-(aq) ions in this solution?

• 3. 2.25 L of 0.400 mol.L-1 Al(NO3)3 (aq) and 2.00L of 0.350 mol.L-1 Ba(NO3)2 (aq) are mixed. What is the molar concentration of nitrate ions in the resulting solution?

Physical Properties – Concentrations: :

• The most useful concentration units for physical properties studies show the relative numbers of molecules (or ions) of each substance. The relative number of molecules (of each substance) is the same as the relative number of moles (of each substance). Often we employ mole fractions – especially for vapor pressure calculations.

Mole Fraction and Mole Percent


i = Amount of component i (in moles)

Total amount of all components (in moles)

1 + 2 + 3 + …n = 1

Mole % i = i 100%


• Molarity (mol∙L-1), does not indicate the relative amounts of solute(s) and solvent. The next slide helps demonstrate why. An alternate concentration unit, molality, does give an indication of the relative amounts of solute(s) and solvent. We can convert from molarity to molality given the solution density.



Molarity (M) = Amount of solute (in moles)

Volume of solution (in liters)

Molality (m) = Amount of solute (in moles)

Mass of solvent (in kilograms)

Class Example• 4. At 25 o C a concentrated H2SO4/water

solution has a density of 1.841 g.cm-3 and is 95.1 % H2SO4 by mass.

• Find: (a) the molarity of H2SO4.

• (b) the molarity of H2SO4

• (c) the mole fraction of H2SO4 and water in the solution.

Intermolecular Forces and the Solution Process

Copyright © 2011 Pearson Canada Inc.

General Chemistry: Chapter 13 Slide 9 of 46

FIGURE 13-2

•Enthalpy diagram for solution formation

Intermolecular Forces in Mixtures



FIGURE 13-3•Intermolecular forces in a solution

ΔHsoln = 0

Magnitude of ΔHa, ΔHb, and ΔHc depend on intermolecular forces.

Ideal solution

Forces are similar between all combinations of components.

Similar Intermolecular Forces

• Molecules with similar structures often have intermolecular forces of the same type and of similar strength. The next slide shows the structures of benzene and the slightly more complex toluene molecule. What intermolecular forces are important for these two molecules?

Two components of a nearly ideal solutionFIGURE 13-4



Formation of Ionic Solutions



FIGURE 13-6

•An ionic crystal dissolving in water

Hydrated Ions – Intermolecular Forces

• Can highly polar water molecules and ions interact? Yes. This is represented on the previous slide (2 dimensions!). The interaction is particularly important for small metal ions with larger charges – such as Mg2+(aq). (Aside: The effects of hydration are sometimes surprising – thus, e.g., lithium ions move through water more slowly than potassium ions!)

Solution Formation and Equilibrium



FIGURE 13-7

•Formation of a saturated solution

13-5 Solubility of Gases



Effect of temperature on the solubilities of gases

Effect of Temperature

•Most gases are less soluble in water as temperature increases.

•In organic solvents the reverse is often true.

Dissolved Oxygen• The oxygen that dissolves in fresh and sea

water is critical to aquatic life/food chains. The amount of dissolved oxygen decreases as water temperature increases which is an important current concern. In aquatic environments oxygen levels can drop due to agricultural runoff as well (Gulf of Mexico “dead zones”).

Henry’s Law ? – Global Warming?

Effect of Pressure


•William Henry found that the solubility of a gas increases with increasing pressure.

C = kPgas

k = C

Pgas

=23.54 mL

1.00 atm= 23.54 ml N2/atm

k

CPgas = =

100 mL= 4.25 atm

23.54 ml N2/atm

Effect of pressure on the solubility of a gasFIGURE 13-11



Henry’s Law Example• 5. What are the expected units for the Henry’s

Law constant, kH. What graph might you draw (at least mentally) to remind yourself of the form of the Henry’s Law equation and, as well, the units for kH?

• 6. The concentration of a dissolved gas with at a “surface pressure” P1 is c1. What are two ways in which we could calculate the concentration of dissolved gas , c2, at a pressure P2?

molarity and molality copyright © 2011 pearson canada inc. slide 1 of 46 general chemistry: chapter...

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