SolutionsThe story continues

Heterogeneous mixture Particles of varied size

Heterogeneous mixtures Suspension – Particles settle out if left

alone Colloids – Based on size of particles and

the action of solution (477 table 1)

Homogeneous mixtures You cannot see various parts of the

solution. (479 table 2)

Concentration Compares the amount of solute that is

in a solvent

Many ways to express this…

Concentration Percent by mass

% by mass = (mass solute/mass solvent)*100

Concentration Percent by volume

% by volume = (volume solute/volume solution)*100

Concentration Molarity

Molarity = (moles solute/liters solvent)

Concentration Molarity

Concentration Molality

Molality = (Moles solute/ Kg solution)

Solvation Surrounding solute with solvent

Solvation Soluble

Insoluble

Miscible

Immiscible

Types of Solutions Unsaturated

Saturated

Supersaturated

Factors Agitation

Surface area

Temperature

Solubility

Saturated Solutions Temperature effect

Sugar in Water

Solubility Page 493

Figure 15

Solubility of a gas Depends on:

Temperature Pressure

Higher pressure “Pushes” molecules into the solution

Solubility of a gas Solubility =

Solubility is given in g/L

Solubility 10 g of a gas dissolves in 2 L of water.

What is the solubility of this gas in water?

3 moles of H2 dissolves in 10 L of water. What is the solubility of H2?

Solubility of a gas Henry’s Law

=

Solubility of a gas The solubility of a gas is .35 g/l at S.T.P.

What is the solubility of the material if the pressure is reduced to .75 atm?

Solubility of a gas At 25°C and 1 atm, 1 g of a gas

dissolves in 2 L of water. What mass of the same gas will dissolve in 2 L of water at 25°C and 4 atm?

Find the molarity of the solution formed by dissolving 116.9 g Na Cl in .5 L solution.