Honors Chem - Chapter 18: Solutions

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Solubility

Maximum amount of solute dissolved in a given amount of solvent at a specific temperature

Dilute Solution

When there is more of the solvent than the solute

Concentrated Solution

When there is more of the solute than the solvent

Solute

The compound being dissolved

Solvent

What the solute is being dissolved in

Factors Affecting Solubility

1. Temperature (when increased, solubility of gases decreases)

2. Agitation

3. Particle Size

Henry’s Law

At constant temperatures, the solubility of a gas is directly proportional to the pressure of the gas above the liquid: S1/P1 = S2/P2

Units of Concentration

1. Molarity

2. %Mass/Volume

3. %Volume/Volume

4. Mole Fractions

5. Molality

Molarity

M = # of moles of solute/volume of solution in L

% Mass/Volume

% M/V = (mass of solute in g)/(volume of solution in mL) * 100

% Volume/Volume

% V/V = (volume of solutes in L)/(volume of solution in L) * 100

Mole Fractions

• Xsolute = mole of solute/total moles solute + solvent

• Xsolvent = mole of solvent/ total moles solute + solvent

• Xsolute + Xsolvent = 1

Making Dilutions

M1V1(dilute) = M2/V2(stock/concentrated)

Colligative Properties

1. Boiling Point Elevation

2. Freezing Point Depression

   1. Vaporizing Pressure Lowering

Boiling Point Elevation

Change in Boiling Point = (i)(Kb)(m)

Freezing Point Depression

Change in Freezing Point = (i)(Kf)(m)

Molal Constants for Water

• Kb = 0.512 C/m

• Kf = 1.86 C/m