Chapter 25

High surface tension, low vapor pressure, and high boiling points

Low vapor pressure: the hydrogen bonds holding water molecules in a liquid state must be broken before water changes from liquid to vapor. High Boiling point: it takes more heat to break the hydrogen bonds between water molecules. High surface tension:

Ice has less density than water

Agitation Temperature Particle Size of the solute

Polar solvents dissolve polar compounds (also ionic compounds) Nonpolar solvents dissolve nonpolar compounds

IonicCovalentPolarNonpolarSoluble Insoluble Soluble in nonpolar solvent Solubility in Water

Chapter 16

Saturated solution- contains the maximum amount of solute for a given quantity of solvent at a constant temperature and pressure.

Unsaturated solution- a solution that contains less solute than a saturated solution at a given temperature and pressure Supersaturated solution- contains more solute than it can theoretically hold at a given temperature.

Concentration- a measure of the amount of solute that is dissolved in a given quantity of solvent. Dilute solution Concentrated solution

The number of moles of solute dissolved in one liter of solution.

What is the molarity of a solution with.0155 moles of NaCl in.1 L of water? A solution has a volume of 0.25 L and contains 0.70 mol of NaCl. What is its molarity?

Diluting a solution reduces the number of moles of solute per unit volume, but the total number of moles of solute in solution does not change. You are just adding more volume, the number of moles of solute is staying the same.

Colligative properties- a property of solution that depends only upon the number of solute particles, not upon their identity. Freezing point depression Boiling point elevation

The freezing point of the solution is lower than the freezing point of the pure solvent. The difference between the freezing point of the solution and the freezing point of the pure solvent is freezing point depression.

The boiling point of the solution is higher than the boiling point of the pure solvent. The difference in temperature between the boiling point of the solution and the boiling point of the pure solvent is the boiling point elevation.

The number of moles of solute dissolved in 1 kilogram of solvent.

How many grams of potassium bromide must be dissolved in kg of water to produce a molal KBr solution?

Chapter 19

Donate H + (it will have a hydrogen in the formula) Common acids: hydrochloric acid, nitric acid, sulfuric acid, phosphoric acid, ethanoic acid, and carbonic acid

Accepts H + (it will have a hydroxide ion in the formula) Common bases: sodium hydroxide, potassium hydroxide, calcium hydroxide, magnesium hydroxide

HCl + Ca(OH) 2  CaCl 2 + 2H 2 O

A neutral solution of an aqueous solution will have [H + ] equal to [OH - ]. pH equation K w = [H + ] x [OH - ]= 1.0 x Practice with number 11 on page 655 in the book.

To find the pH of a solution you look at the H + or hydronium ion (H 3 O + ).