1. II III I II. The Nature of Solutions Ch. 13 – Liquids & Solids

2. A. Solutions MATTER Can it be physically separated? Homogeneous Mixture (solution) Heterogeneous MixtureCompoundElement MIXTUREPURE SUBSTANCE yesno Can it be chemically decomposed? noyes Is the composition uniform? noyes ColloidsSuspensions

3. Separating Mixtures: 1.Evaporation 2.Filtration 3.Decanting 4.Centrifuge – spins rapidly and separates liquids with different densities 5.Chromatography – (color) separates dyes in ink 6.Distillation - separates liquids with different boiling points using vaporization & condensation

4. A. Solutions  Solution Homogeneous mixture very small particles no Tyndall effect Tyndall Effect particles don’t settle EX: salt water, hydrogen peroxide, 3 M (molar) HCl

5. A. Definitions  Solution: Solvent Solvent - present in greater amount- does the dissolving Solute Solute - substance being dissolved

6. A. Definitions  Types of solutions: Solid Solutions: gold jewelry (gold + copper, 18k (karot) is 18/24=75% gold); alloy- brass (copper + zinc) Gas Solutions: air (78% nitrogen, 21% oxygen, <1% argon and neon) Liquid Solutions: oxygen dissolved in lakes; soda pop-CO 2 in water

7. A. Definitions Aqueous Solutions: water is the solvent (universal solvent) Salt + water Sugar + water 3% Hydrogen Peroxide NaOH (aq)

8. B. Solvation  Solvation the process of dissolving Increase rate by 3 things: stirring, increase temp. of solvent, smaller particle size. solute particles are separated and pulled into solution solute particles are surrounded by solvent particles

9. B. Solvation  1. Dissociation separation of an ionic solid into aqueous ions NaCl(s)  Na + (aq) + Cl – (aq) MgCl 2 (s) Mg +2 (aq) + 2Cl - (aq)

10. B. Solvation  2. Ionization breaking apart of some polar molecules into aqueous ions HNO 3 (aq) + H 2 O(l)  H 3 O + (aq) + NO 3 – (aq) (nitric acid)

11. B. Solvation  3. Molecular Solvation Molecules Covalently bonded stay intact C 6 H 12 O 6 (s)  C 6 H 12 O 6 (aq) (glucose, sugar)

12. B. Solvation Strong Electrolyte Non- Electrolyte solute exists as ions only - + salt - + sugar solute exists as molecules only - + acetic acid Weak Electrolyte solute exists as ions and molecules

13. B. Solvation NONPOLAR + NONPOLAR POLAR + POLAR  Detergents - exception polar “head” with long nonpolar “tail” can dissolve nonpolar grease in polar water “Like Dissolves Like”

14. C. Solubility  Solubility maximum grams of solute that will dissolve in 100 g of solvent at a given temperature and pressure varies with temp. and pressure based on a saturated solution - (maximum of solute has been dissolved)

15. C. Solubility  Polar Substances Water Salt (ionic solids) ammonia Vinegar (acetic acid) Rubbing alcohol (isopropyl) acetone  Nonpolar substance Vegetable oil Waxes Petroleum oil Gasoline Carbon tetrachloride Hexane

16. C. Solubility SolutePolar Solvent Nonpolar solvent PolarSoluble (will mix together) insoluble NonpolarInsoluble- (Not Soluble) soluble Ionicsolubleinsoluble

17. C. Solubility SATURATED SOLUTION no more solute can dissolve UNSATURATED SOLUTION more solute can dissolve SUPERSATURATED SOLUTION becomes unstable, crystals form concentration

18. C. Solubility  Solubility Curve shows the dependence of solubility on temperature

19. C. Solubility  Solids are more soluble at... high temperatures.  Gases are more soluble at... low temperatures. high pressures EX: nitrogen narcosis, the “bends,” soda