Chapter 9: Polyprotic Acids and Bases

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Cecil Pitts
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1 Amino acids Isoionic point Isoelectronic point 9-6 Isoelectric & Isoionic ph 9-1 Diprotic A&B Leucine: acidic & basic forms Leucine: intermediate form Monoprotic Polyprotic 9-5 Fractional compositions Chapter 9: Polyprotic Acids and Bases 9-2 Diprotic buffers Two HH equations Monoprotic case Diprotic case 9-4 Principal Species 9-3 Polyprotic A&B Multiple HH equations

2 10-9 The Levelling Effect 10-1 Titration of Strong Base with Strong Acid Procedure Equivalence Point vs. End Point ph curves Alkaline solutions Subtopic Storage 10-7 Practical Notes Primary standards (table) 10-6 Finding the End Point with Indicators Chapter 10 Acid-Base Titrations 10-2 Titration of Weak Acid with Strong Base Introduction ph curves Before addition of base 10-3 Titration of Weak Base with Strong Acid Before acid is added First and second derivatives 10-5 Finding the End Point with a ph Electrode 10-4 Titrations in Diprotic Systems ph curves Buffer region #1 B, BH+ First EP Buffer region #2 BH+, BH2+ Second EP

3 Direct Back Displacement Indirect 11-7 EDTA titration techniques 11-1 Metal-chelate complexes Glossary: Lewis acid, Lewis base, Monodentate, Bidentate, Multidentate, Chelate effect Complexometric titration Examples: naturally occurring amino carboxylic acids Masking pka values 11-6 Metal-Ion Indicators Chapter 11 EDTA Titrations 11-2 EDTA Introduction Preparation and usage Acid and base properties alpha-y4- (fraction of EDTA as chelator) EDTA complexes formation constant, Kf conditional formation constant, Kf' Examples Metal-Ligand Equilibria Titration in the presence of an ACA 11-5 Auxiliary Complexing Agents 11-3 EDTA titration curves Explicit calculation

4 oxidation and reduction charge and quantity of reaction 13-7 Biochemists and Eo' 13-1 Basic concepts current and reaction rate voltage and Gibbs energy of reaction Simple ph meter Tips for analyzing cells 13-6 Cells as Chemical Probes glossary: electric charge, Coulombs, electric current, Ampere, electrical potential, Volts, Gibbs (free) energy, Faraday constant, Ohm's Law, resistance, Ohms, power, Watts Eo and K Examples of Eo and K 13-5 Eo and the Equilibrium Constant Chapter 13 Electrochemistry 13-2 Galvanic cells glossary: batteries, fuel cells, cathode (reduction), anode (oxidation), short circuited net reaction and half reactions salt bridge Nernst equation 13-4 Nernst Equation N.E. for a complete cell/reaction Intuitive thoughts (number line) line notation for galvanic cells voltmeter/potentiometer standard reduction potential 13-3 Standard potentials standard hydrogen electrode (SHE) Subtopic

5 line notation electrode schematics glass membrane standards junctional potentials and drifts alkaline error acid error equilibration time hydration of glass temperature cleaning electrode errors in ph measurements 14-6 Ion Selective Electrodes 14-5 ph Measurement with a Glass Electrode Chapter 14 Potentiometry 14-1 Reference Electrodes 14-2 Indicator Electrodes Glossary: potentiometry, electroactive species, indicator electrode, reference electrode, cell voltage Reference electrodes Metal electrodes Ion Selective electrodes General properties Titration example Titration curve Ag AgCl electrode Calomel electrode Voltage conversion scale Pt, Au, Ag high surface area very clean semi-permeable membrane filling solution ionophore electrode schematics 14-4 How Ion-Selective Electrodes Work 14-3 Junction Potentials What are they? How do they arise? Electronic potential difference for an ISE

6 Iodometry Iodimetry Starch indicator I3- solutions 15-7 Methods Involving Iodine 15-1 The Shape of a Redox Curve Ce4+ - Fe2+ titration Shapes of Redox Curves Use of sodium thiosulphate Use with indicator Applications Primary standard: ammonium hexanitrato -cerate(iv) 15-5 Oxidation with Ce Chapter 15 Redox Titrations 15-2 Finding the Endpoint Electrodes Indicators Peroxydisulfate Silver (II) oxide Determination of suitable indicator Starch (for iodine) Preoxidation sodium bismuthate Strong acid solutions Hydrogen peroxide Neutral or alkaline solutions Strong basic solution Standardization with sodium oxalate 15-4 Oxidation with Potassium Permanganate 15-3 Adjustment of Analyte Oxidation State How to get rid of the preoxidation agents Stannous chloride Chromous chloride Prereduction Jones reductor Zinc amalgam How to get rid of the prereduction agents

7 15-A Redox titration 9-A phs of species from polyprotics 15-B Redox indicator 9-B ph and polyprotic buffers 15-M Iodine titrated with thiosulphate 9-C ph and buffers, choose species 9-D ph's of amino acids Shape of Redox Curve Adjustment of Analyte Oxidation State Redox reactions (KMnO4, Ce4+ and K2Cr2O7) Methods with Iodine Chapter 15 Chapter 9 - Polyprotic A&B Examples 9-G isoionic ph of 0.01 M lysine A&B forms Leucine Intermediate form ph of intermediate form, diprotic acid diprotic buffers triprotic system 14-A Cell voltage calculation 14-C Ion selective electrode principal species Reference electrodes Indicator electrodes Junction potentials ph measurement - glass electrode Chapter and Examples Chapters 9-15 Chapter A ph titration SA/SB 10-B ph titration WA/SB 10-C ph titration SA/WB 10-H Activity Coefficients and ph Diprotic Systems Ion selective electrodes 13-C Cell Voltages 13-D Nernst eq. and cells Finding the EP with Indicators Practical notes and levelling effect 13-F Reduction potentials Titration curves and spreadsheets 13-H Nernst and K 13-J Reducing agents 11-A EDTA titration (Zn) 11-E EDTA titration (Mn) Electricity Basic electrochemistry Galvanic cells Std. Red. Pot. and Nernst Eo and K Cells as Chemical Probes Biochemists and Eo' Chapter 13 Chapter G Iminodiacetic acid EDTA EDTA titration curves Auxiliary complexing agents Metal ion indicators EDTA titration techniques

Electrochemistry. Redox reactions. Half Reactions. Nernst Equation Ion selective electrodes

Electrochemistry. Redox reactions. Half Reactions. Nernst Equation Ion selective electrodes Electrochemistry Nernst Equation Ion selective electrodes Redox reactions oxidation - loss of electrons M n+ M n+1 + e - M is oxidized - reducing agent reduction - gain of electrons N n+ + e - N n-1 N