1. Chapter 25

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

3. 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:

4. Ice has less density than water

7. Agitation Temperature Particle Size of the solute

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

9. IonicCovalentPolarNonpolarSoluble Insoluble Soluble in nonpolar solvent Solubility in Water

10. Chapter 16

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

12. 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. https://www.youtube.com/watch?v=BLq5NibwV5g

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

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

16. 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?

17. 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.

18. 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

19. 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.

20. 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.

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

22. How many grams of potassium bromide must be dissolved in 0.750 kg of water to produce a 0.150 molal KBr solution?

23. Chapter 19

24. 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

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

28. HCl + Ca(OH) 2  CaCl 2 + 2H 2 O

29. A neutral solution of an aqueous solution will have [H + ] equal to [OH - ]. pH equation K w = [H + ] x [OH - ]= 1.0 x 10 -14 Practice with number 11 on page 655 in the book.

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