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Chemistry 123 Review - Spring 2013

Chemistry 123 Review - Spring 2013. Final Exam Monday, June 10, 2013; 10:30-12:30 ~ 50:50 Qualitative & Quantitative Questions Final counts as 26 % of Grade. Chapter 15 – Intro to Acids & Bases. Arrhenius Definition Strong Acids/Bases (know these); M H + pH

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Chemistry 123 Review - Spring 2013

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  1. Chemistry 123 Review - Spring 2013 Final Exam Monday, June 10, 2013; 10:30-12:30 ~ 50:50 Qualitative & Quantitative Questions Final counts as 26 % of Grade

  2. Chapter 15 – Intro to Acids & Bases • Arrhenius Definition • Strong Acids/Bases (know these); M H+ pH • Weak Acids/Bases (know these); M OH- pOH • weak acids: HF, HC2H3O2, HCN, H3PO4, NH4+, HNO2 • weak bases: NH3 , HCO3-, salts of weak acids • Bronsted-Lowry Definition • Conjugate acids & bases • Lewis Definition • Auto Ionization of water • pH & pOH; 1.00x10-14 = [H+][OH-]; 14.00 = pH + pOH • Measuring Acidity: pH or M of H+ • Meters & Indicators • Significant Figures • Accuracy & Precision 15%

  3. Chapter 16 Acid-Base Equilibria(weak acids/bases) - Equilibria Expression (H2O & Solids drop out of expression) - Determination of Ka from pH - Determination of % Ionization - Determination of [H+] from Ka & M of HA (let X = M that ionizes) Approximation for simplifying the math: [HA]/Ka > 100 - Determination of [H+] or [OH-] for a Base. Ka x Kb= 1.00x10-14 - Determination of [H+] from salt of weak acid - Determination of [H+] from [HA] & [A-] (Common Ion & Buffer) - pH = pKa + log [A-]/[HA] (Henderson-Hasselbalch Equation) - Buffers: Define, Strength, Effective Range, Selection - Titrations: pH Calculations & pH Curves 20%

  4. Chapter 17 - Solubility Equilibria - Equilibria expression (solid drops out) - Calculation of Ksp from solubility - Calculation of Solubility from Ksp (let X = M that dissolves) - Calculation of Solubility in Presence of Common ion - Effect of pH & complex ion formation on solubility - Possible Separation of Ions using solubility - Prediction of Precipitation (Q compared to Ksp) - Le Chatelier’s Principle 13%

  5. Chapter 18 – Thermodynamics, pg 1 - Terms to know: State Function Enthalpy, H Entropy, S Free Energy, G Specific Heat Capacity, s Calorimeter Bond Energy Signs involved with ∆H, ∆S, ∆G, Bond Energies - Calculations / Equations: Δ H = s x m x ΔT ΔHR = ∑HoFProducts - ∑HoFReactants ΔHR = ∑HBonds Broken - ∑HBonds Formed Hess’s Law

  6. Chapter 18 – Thermodynamics, pg 2 -Calculations / Equations Continued: S = ΔH / T (only for a system at equilibrium) ΔSR = ∑∆SP - ∑∆SR ΔGR = Δ H - T Δ S ΔGR = ∑ΔGoFProducts - ∑ΔGoFReactants ΔGo = - RT Ln K ; Ln K = - ΔGo / RT or K = e-ΔG / RT - Miscellaneous: - Lewis Structures - Ni+2 Complex & Alcohol Determination labs - Beer’s Law: A = εbc@ constant λ ε = molar absorptivity c = M b = path length of cuvette in cm A = absorbance 22%

  7. Chapter 19 - Electrochemistry - Problems & Terminology: Oxidation, Reduction, Oxidation Numbers, Voltaic & Electrolytic Cells, Signs, Cathode, Anode, Voltage/emf/Potential, Half Cell Reactions - Balancing Redox Reactions in Acid 3 Rules - Voltaic Cells: Conventions for short Cell Notation: anode elec ions ionscathelec Eocell = Eooxidation + Eoreduction ΔGo = - nFEocell(Coul x Volt = Joule) Eo = (0.0592/n) Log Keq[2.303RT/nF = 0.0592/n @ 25.0 oC] E = Eo - 0.0592/n Log Q (@ 25 oC)= Nerst Equation - Electrolytic Cells: Uses Predicting Rxn using Eo values; pH & F- ISE (ion selective electrode) Calculations: Coul = amps x sec & 1F = 96,500 coul = 1 m e- 29%

  8. Equations & Constants Given on Final Exam coul = amps x sec Eocell = Eooxidation ½ Cell + Eoreduction ½ Cell

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