3. Ca(NO 3 ) 2 YES All nitrates are soluble! Zn(OH) 2 NO Hydroxides are insoluble except for sodium and potassium ions! K 3 PO 4 YES Phosphates are insoluble except for sodium, potassium, and ammonium ions!

4. Energy to boil (kJ/mol) 1100 Ion- ion 700 500 Covalent bonds 100 60 Intermolecular forces 0.1 H-bonds Polar bonds Non-polar bonds ( intramolecular forces)

5. Why so strong? -Small size of hydrogen -High electronegativity of O, N, and F What are they? -A network between H and either N, O, or F molecules

7. Name Simple Cubic Body- Centered Cubic Face- Centered Cubic # atoms/unit cell 124 Volume e = edge length r = cell radius e 3 = (2r) 3 = 8r 3 e 3 = (4r/√3) 3 (4r/√3) 3 e 3 = (4r/√2) 3 (4r/√2) 3

8. For: 3A(aq) + B(s) ↔ 2C(g) + D(l) + E(aq) ** Only gaseous and dissolved particles are expressed in the equilibrium expression because their concentrations can vary (whereas solids and liquids cannot)

9. If a dynamic equilibrium is disturbed by changing the conditions, the position of equilibrium moves to counteract the change. 3A (aq) + B (s) ↔ 2C (g) + D (l) + E (aq) If the concentration of A is raised, as the mixture returns to equilibrium a portion of all of the reactants are consumed, and as a result, the concentrations of C, D, and E will increase

10. N 2 + O 2 ↔ 2NO ICEICE 0.25 0.25 0.0042 -x -x +2x 0.25 0.25 0.0042 + 2x K c = 1.7 x 10 -3 = (0.0042 + 2x) 2 / (0.25)(0.25) Eventually… x = 0.0030 M change

11. Would a precipitate form? AgCl (s) ↔ Ag + (aq)+ Cl - (aq) K sp = 1.8 x 10 -10 Q = [Ag + ][Cl - ] 25 mL of 0.1M AgNO 3 solution is added to 100 mL of 0.0050M NaCl solution If Q<K sp, no precipitation If Q>K sp, precipiation [Ag + ] = 0.10M(25mL/125mL) [Cl - ] = 0.005M(100mL/125mL) Therefore Q>K sp, and this is expected to precipitate Q = (0.100)(0.005) = (5.0 x 10 -4 )

12. Molar Concentration “molarity” M = # moles/vol. of solution Molal Concentration “molality” m = # moles solute / mass of solvent (in kg) Mass Fraction = mass solute / mass total Ppm (parts per million) = mass solute (in mg) / mass total (in kg) Mole Fractions X A = moles A /moles A + moles B +…

13. Cd(OH) 2 K sp = 1.2 x 10 -14 Ca(OH) 2 K sp = 7.9 x 10 -6 Ca 2+ Cd 2+ 0.10 M Cd 2+ 0.10 M Ca 2+ At what concentration of OH - will one of the ions precipitate? (OH - ) is more attracted to Cd 2+, because, as the equations are similar in structure (1 cation, 2 anions) they are comparable and Cd(OH) 2 would precipitate first Cd(OH) 2  Cd 2+ (aq) + 2OH - (aq) 0.10~0 +x K sp = 1.2*10 -14 = (0.10)(x) 2 X 2 = 12*10 -12 x = 3.5*10 -6

14. Freezing Point Depression ΔT f = iK f m Boiling Point Elevation ΔT b = iK b m i = # dissociated particles in empirical formula (Van’t Hoff factor) K f or K b = boiling point elevation / freezing point depression constant m = (n mol solute / mass solvent (kg))

15. Volatile Solution P vaptotal = X A P vapA + X B P vapB +… Non-volatile Solution P vapA = X A P vapA + 0 volatile= changes to gas

16. “the solubility of a gas is proportional to the pressure of the gas” Sol g = K Henry P g Osmotic Pressure Π = (n/v)RT R = 0.082057 L · atm / K · mol C = (n / v) = (mol/L) T = temperature in Kelvin