UW CHEM 120 Summer ALWAYS express any numerical value with units and significant figures. This includes intermediate values in calculations!

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1 Exam 3 Review Tips for Success on Exams: Show ALL YOUR WORK when solving numerical problems. ALWAYS express any numerical value with units and significant figures. This includes intermediate values in calculations! Be able to discriminate between necessary and extraneous information in a word problem. Bring a scientific calculator to the exam. No graphing calculators and no cell phones will be allowed. hapter 8: Solutions Types of solutes and solvents Polar and non polar interactions Strong, weak, and non electrolytes alculate equivalents Know the properties of an unsaturated and saturated solutions Know the effect of temperature on solubility Understand Henry s Law Know the solubility rules 1&2 from lecture. Know why some salts are less soluble Write double replacement reactions Determine if there is a precipitate reaction Write the ionic equation Write the net ionic equation Be able to do calculations using mass percent, volume percent, mass/volume percent, and molarity. Perform dilution calculations Know how colloids and suspensions are different from solutions of soluble salts. Perform mole ratio calculations and limiting reactant calculations for precipitation reactions. Know freezing point suppression and boiling point elevation Understand osmotic pressure Know what happens to isotonic cells if placed in a hypertonic or hypotonic medium. 1 of 5

2 Describe dialysis. hapter 9: hemical Equilibrium Describe collision theory Know how to draw a reaction diagram. Know what activation energy is Understand rates of reactions and the factors that change the rate of reaction. Understand how catalysts change reactions Show how equilibrium is established and describe equilibrium state. Write equilibrium constants for reactions. alculate equilibrium constants for reaction. alculate a concentration of a species from the equilibrium constant. Know what is left out of the equilibrium constant. Use equilibrium constants to determine whether equilibrium favors products or reactants. Perform stresses on equilibrium via Le hatelier s Principle. alculate the solubility product constant in a saturated solution alculate the solubility of a slightly soluble salt. hapter 10: Acids and Bases Describe the characteristics of acids and bases. Describe an Arrhenius acid and base. Describe a Bronsted Lowry acid and base. Name acids and bases Find conjugate acid/base pairs Know about strengths of acids and bases (know the 6 strong acids in table 10.3) Determine if an acid/base reaction favors products or reactants. Write dissociation constants Show the auto ionization of water Know the ion product constant of water Determine the concentration of acid or base with the ion product constant of water Know the concentration of acid and base when a solution is neutral and be able to tell whether a solution is acidic, neutral, or basic. Know the ph scale. hange the ph of a solution by dilution. alculate concentration of acids and bases from ph and calculate ph from concentrations of acids and bases. React acids with different bases. Balance neutralization reactions Do acid base titrations Know the acid base properties of salt solutions 2 of 5

3 Know what makes a buffer solution alculate the ph of a buffer The next page starts the information you will be given on the exam. Be sure to remember anything you may need that is not included below. I may add things you need, but I will never remove anything from this list. onversion factors: 3 of 5

4 Length 1 m = yd 1 mi = 5280 ft 1 ft = 12 in 1 mi = 1760 yd 1 Å = m 1 in = 2.54 cm Mass 1 kg = lb 1 lb = g 1 amu = x kg 1 dry oz (ounce) = g Volume 1 L = 1.06 qt 1 ft 3 = L 1 ml = 1 cm 3 1 gal = L 1 liquid oz = ml Pressure 1 atm = 760. mmhg 1 torr = 1 mmhg 1 atm = lb/in 2 (psi) 1 atm = 101,325 Pa 1 Pa = 1 N/m 2 1 bar = 100 kpa Energy 1 ev = x J 1 cal = J (exact) 1 kcal = 1 al Force 1 N = lb Radioactivity 1 i = 3.7 x Bq 1 Gy = 100 rad 1 Sv = 100 rem 1A 1 H Li Na Physical Data: 2A 4 Be Properties of Water Density, liquid = g/cm 3 Density, solid = g/cm 3 Heat of vaporization = 2260 J/g Heat of fusion = 334 J/g T boil = K T freeze = K Specific heat, solid = 2.11 J/g.K Specific heat, liquid = J/g.K Specific heat, gas = J/g.K 12 Mg B 4B 5B 6B 7B 8B 8B 8B 1B 2B 3A 4A 5A 6A 7A 5 B Al Si N P O S F l A 2 He Ne Ar K Rb s Fr (223) 20 a Sr Ba Ra Sc Y La Ac (227) 22 Ti Zr Hf V Nb Ta r Mo W Mn Tc (98) 75 Re Fe Ru Os o Rh Ir Ni Pd Pt u Ag Au Zn d Hg Ga In Tl Ge Sn Pb As Sb Bi Se Te Po (209) 35 Br I At (210) 36 Kr Xe Rn (222) onstants: 4 of 5

5 Avogadro s Number 6.02 x mole 1 Gas constant (R) L atm / mole K 62.4 L mmhg / mole K J/mole K Metric prefixes: tera (T) = peta (P) = pico (p) = femto (f) = Equations: m d V qsmt T T T T F final 1.8T 32 initial T K T cv cv ph poh + ph log[h3o ] poh log[oh ] Solubility rules for salts in water: 1. not given 2. not given 3. Most chloride, bromide, and iodide salts are soluble. Notable exceptions are salts containing the ions Ag +, Pb 2+, and Hg Most sulfate salts are soluble. Notable exceptions are BaSO 4, PbSO 4, HgSO 4, and aso Most hydroxide salts are only slightly soluble. The important soluble hydroxides are NaOH and KOH. The compounds Ba(OH) 2, Sr(OH) 2, and a(oh) 2 are marginally soluble. 6. Most sulfide, carbonate, chromate, and phosphate salts are only slightly soluble. 5 of 5

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