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# ANALYTICAL CHEMISTRY LECTURE CHEM 321

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This 104 page Class Notes was uploaded by Coty O'Hara Sr. on Monday September 28, 2015. The Class Notes belongs to CHEM 321 at Old Dominion University taught by John Donat in Fall. Since its upload, it has received 10 views. For similar materials see /class/215294/chem-321-old-dominion-university in Chemistry and Biochemistry at Old Dominion University.

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Date Created: 09/28/15

Final Review Chem 321 Upcoming Tests 0423 4th Unit Test Chapter 1416 Graded test will be available to pick up outside Rm 200 Chemistry building on April 27 Keys to be posted at the website by April 27 0430 345645 PM Comprehensive Final Examination Chapter 116 except 2 5 and 13 Graded test will be available to pick up outside Rm 200 Chemistry building on May 4 Grade available at Leoonline by May 4 Steps gt Well study all problems in the tests gt Well study all examples that we discussed in the class lecture notes and slides gt Well study all related examples in textbook gt Well study all assigned problems homework Unit Tests gtUnit Test1 Chapters 1 3 4 gtUnit Test2 Chapters 69 gtUnit Test3 Chapters 1012 gtUnit Test4 Chapters 1416 Keys to the Tests httpwww0dueduscixuchem321answershtm Unit Test1 Chapters 1 3 4 SummaryChapter 1 J Course Overview Classi m on of Analysis J Units v Molecular Weight Mole V Concentrations Stoichiometric Calculations v Preparation of Solution SummaryChapter 3 VMean Median Accuracy xPrecision Errors Absolute and Relative Errors rt Systematic or determinate errors 6 Random or indeterminate errors rt Gross errors or blunders SummaryChapter 3 Absolute standard deviation or standard deviation Relative standard deviation Standard deviation of the mean Sm Pooled standard deviation Coefficient of variation Variance s2 xSpread or range Siqnificant Fiqures SummaryChapter 4 Con dence Limit CL Con dence Interval CI Con dence Level Qtest Ttest extra credit F test extra credit Unit Test2 Chapters 69 SummaryChapter 6 V Acids and Bases concepts and strength of Acids and Bases V Equilibriumconstant expression V Types of Equilibrium constants V Pfunctions V Commonion effect V Calculation of equilibrium constants and concentrations eg V Ionproduct constant for water V Solubilityproduct constants V Acid and Base Dissociation Constants SummaryChapter 7 V Molarity V Preparation of solution V Dilution V Titration V Analytical Molarity V Equilibrium or Species Molarity V Percent concentration V PValue V Density amp speci c gravity V Understand concepts titrirnetry equivalence point end point primary standard secondary standard standardization SummaryChapter 7 Titration Curves Titration Curves for a single Anion Titration Curves for Mixtures Anion End Points for Argentometric Titration Chemical Indicators Methods Applications Standard AgNO3 Solution SummaryChapter 8A Ionic Strength Activity Coef cient Activity Types of thermodynamics Equilibrium constants Related calculation and de nition SummaryChapter 8B V Concepts of equilibrium V Equilibrium concentration of every species eg ions solubility in the solution V Equilibriumconstant expressions V Mass concentrationbalance equations V A single chargebalance equation V Calculation of Solubility by the Systematic Method Metal Hydroxides Formation of Complex Ion Separation of ions SummaryChapter 9 J How to select standard solutions and indicators for neutralization titrations J Theory of Indicator Behavior J Titration Curves J Theories Plots and shapes of plots J Parameters pH Volume of titrants equivalence point J Calculations Ka pH indicator choices halfneutralized point J Effects Concentration reaction composition temperature equilibrium constants J The titration of a strong acid with a strong base J The titration of a week acid with a strong base J The titration of a strong base with a strong acid J The titration of a week base with a strong acid J Buffer solutions J Definition and properties eg buffer capacity J Calculation of pH of the buffer solution J Applications Unit Test3 Chapters 1012 SummaryChapters 1011 Derive titration curves of complex acidbase system Mixtures of strong and weak acids or bases Polyfunctional acids and bases Buffer solution involving polyprotic acids Amphiprotic salts eg NaHCO3 General Expression for a values SummaryChapter 12 Basic concepts amp terms 39 Coordination number I Ligand and chelate 39 Unidentate bidentate tridentate 39 Formation constant 39 Conditional formation constants K My K MY Equilibrium Calculations for Complexformation titration Derive EDTA titration curves Calculation of related concentrations Effect of other complexing agents Theory and Calculation of Indicators for EDTA titration Titration Methods employing EDTA Direct titration Backtitration Unit T est4 Chapters 1416 SummaryChapters 1416 Basicconceptsandterms Oxidation and redlction agents and reactions Anode cathode electrode Halfcell reactions electrode potential Galvanic and electrolytic cells Chenical reversible and irreversible reactions Schermtic representation of cells Thermodynanic potential of electrochenical cells SIE standard potential forrral standard potential Indicator and factors of titration cu39ves Calculations Electrode potential Nernst Equation Thermodynanic potentials of electrochenical cell Keq Titration Curves Final Exam 200 points Help Sessions amp Of ce Hours gtThis Wed April 18 Class Hour 52457 PM OCNPS 200 gtNext Friday April 27 23 PM Alfriend Chemistry Building 201 Outside rny Of ce Any Questions Study Really Hard Goodluck to you Dr Nancy Xu Final Review Chem 321 Upcoming Tests 0423 4th Unit Test Chapter 1416 Graded test will be available to pick up outside Rm 200 Chemistry building on April 27 Keys to be posted at the website by April 27 0430 345645 PM Comprehensive Final Examination Chapter 116 except 2 5 and 13 Graded test will be available to pick up outside Rm 200 Chemistry building on May 4 Grade available at Leoonline by May 4 Steps gt Well study all problems in the tests gt Well study all examples that we discussed in the class lecture notes and slides gt Well study all related examples in textbook gt Well study all assigned problems homework Unit Tests gtUnit Test1 Chapters 1 3 4 gtUnit Test2 Chapters 69 gtUnit Test3 Chapters 1012 gtUnit Test4 Chapters 1416 Keys to the Tests httpwww0dueduscixuchem321answershtm Unit Test1 Chapters 1 3 4 SummaryChapter 1 J Course Overview Classi m on of Analysis J Units v Molecular Weight Mole V Concentrations Stoichiometric Calculations v Preparation of Solution SummaryChapter 3 VMean Median Accuracy xPrecision Errors Absolute and Relative Errors rt Systematic or determinate errors 6 Random or indeterminate errors rt Gross errors or blunders SummaryChapter 3 Absolute standard deviation or standard deviation Relative standard deviation Standard deviation of the mean Sm Pooled standard deviation Coefficient of variation Variance s2 xSpread or range Siqnificant Fiqures SummaryChapter 4 Con dence Limit CL Con dence Interval CI Con dence Level Qtest Ttest extra credit F test extra credit Unit Test2 Chapters 69 SummaryChapter 6 V Acids and Bases concepts and strength of Acids and Bases V Equilibriumconstant expression V Types of Equilibrium constants V Pfunctions V Commonion effect V Calculation of equilibrium constants and concentrations eg V Ionproduct constant for water V Solubilityproduct constants V Acid and Base Dissociation Constants SummaryChapter 7 V Molarity V Preparation of solution V Dilution V Titration V Analytical Molarity V Equilibrium or Species Molarity V Percent concentration V PValue V Density amp speci c gravity V Understand concepts titrirnetry equivalence point end point primary standard secondary standard standardization SummaryChapter 7 Titration Curves Titration Curves for a single Anion Titration Curves for Mixtures Anion End Points for Argentometric Titration Chemical Indicators Methods Applications Standard AgNO3 Solution SummaryChapter 8A Ionic Strength Activity Coef cient Activity Types of thermodynamics Equilibrium constants Related calculation and de nition SummaryChapter 8B V Concepts of equilibrium V Equilibrium concentration of every species eg ions solubility in the solution V Equilibriumconstant expressions V Mass concentrationbalance equations V A single chargebalance equation V Calculation of Solubility by the Systematic Method Metal Hydroxides Formation of Complex Ion Separation of ions SummaryChapter 9 J How to select standard solutions and indicators for neutralization titrations J Theory of Indicator Behavior J Titration Curves J Theories Plots and shapes of plots J Parameters pH Volume of titrants equivalence point J Calculations Ka pH indicator choices halfneutralized point J Effects Concentration reaction composition temperature equilibrium constants J The titration of a strong acid with a strong base J The titration of a week acid with a strong base J The titration of a strong base with a strong acid J The titration of a week base with a strong acid J Buffer solutions J Definition and properties eg buffer capacity J Calculation of pH of the buffer solution J Applications Unit Test3 Chapters 1012 SummaryChapters 1011 Derive titration curves of complex acidbase system Mixtures of strong and weak acids or bases Polyfunctional acids and bases Buffer solution involving polyprotic acids Amphiprotic salts eg NaHCO3 General Expression for a values SummaryChapter 12 Basic concepts amp terms 39 Coordination number I Ligand and chelate 39 Unidentate bidentate tridentate 39 Formation constant 39 Conditional formation constants K My K MY Equilibrium Calculations for Complexformation titration Derive EDTA titration curves Calculation of related concentrations Effect of other complexing agents Theory and Calculation of Indicators for EDTA titration Titration Methods employing EDTA Direct titration Backtitration Unit T est4 Chapters 1416 SummaryChapters 1416 Basicconceptsandterms Oxidation and redlction agents and reactions Anode cathode electrode Halfcell reactions electrode potential Galvanic and electrolytic cells Chenical reversible and irreversible reactions Schermtic representation of cells Thermodynanic potential of electrochenical cells SIE standard potential forrral standard potential Indicator and factors of titration cu39ves Calculations Electrode potential Nernst Equation Thermodynanic potentials of electrochenical cell Keq Titration Curves Final Exam 200 points Help Sessions amp Of ce Hours gtThis Wed April 18 Class Hour 52457 PM OCNPS 200 gtNext Friday April 27 23 PM Alfriend Chemistry Building 201 Outside rny Of ce Any Questions Study Really Hard Goodluck to you Dr Nancy Xu Final Review Chem 321 Upcoming Tests 0423 4th Unit Test Chapter 1416 Graded test will be available to pick up outside Rm 200 Chemistry building on April 27 Keys to be posted at the website by April 27 0430 345645 PM Comprehensive Final Examination Chapter 116 except 2 5 and 13 Graded test will be available to pick up outside Rm 200 Chemistry building on May 4 Grade available at Leoonline by May 4 Steps gt Well study all problems in the tests gt Well study all examples that we discussed in the class lecture notes and slides gt Well study all related examples in textbook gt Well study all assigned problems homework Unit Tests gtUnit Test1 Chapters 1 3 4 gtUnit Test2 Chapters 69 gtUnit Test3 Chapters 1012 gtUnit Test4 Chapters 1416 Keys to the Tests httpwww0dueduscixuchem321answershtm Unit Test1 Chapters 1 3 4 SummaryChapter 1 J Course Overview Classi m on of Analysis J Units v Molecular Weight Mole V Concentrations Stoichiometric Calculations v Preparation of Solution SummaryChapter 3 VMean Median Accuracy xPrecision Errors Absolute and Relative Errors rt Systematic or determinate errors 6 Random or indeterminate errors rt Gross errors or blunders SummaryChapter 3 Absolute standard deviation or standard deviation Relative standard deviation Standard deviation of the mean Sm Pooled standard deviation Coefficient of variation Variance s2 xSpread or range Siqnificant Fiqures SummaryChapter 4 Con dence Limit CL Con dence Interval CI Con dence Level Qtest Ttest extra credit F test extra credit Unit Test2 Chapters 69 SummaryChapter 6 V Acids and Bases concepts and strength of Acids and Bases V Equilibriumconstant expression V Types of Equilibrium constants V Pfunctions V Commonion effect V Calculation of equilibrium constants and concentrations eg V Ionproduct constant for water V Solubilityproduct constants V Acid and Base Dissociation Constants SummaryChapter 7 V Molarity V Preparation of solution V Dilution V Titration V Analytical Molarity V Equilibrium or Species Molarity V Percent concentration V PValue V Density amp speci c gravity V Understand concepts titrirnetry equivalence point end point primary standard secondary standard standardization SummaryChapter 7 Titration Curves Titration Curves for a single Anion Titration Curves for Mixtures Anion End Points for Argentometric Titration Chemical Indicators Methods Applications Standard AgNO3 Solution SummaryChapter 8A Ionic Strength Activity Coef cient Activity Types of thermodynamics Equilibrium constants Related calculation and de nition SummaryChapter 8B V Concepts of equilibrium V Equilibrium concentration of every species eg ions solubility in the solution V Equilibriumconstant expressions V Mass concentrationbalance equations V A single chargebalance equation V Calculation of Solubility by the Systematic Method Metal Hydroxides Formation of Complex Ion Separation of ions SummaryChapter 9 J How to select standard solutions and indicators for neutralization titrations J Theory of Indicator Behavior J Titration Curves J Theories Plots and shapes of plots J Parameters pH Volume of titrants equivalence point J Calculations Ka pH indicator choices halfneutralized point J Effects Concentration reaction composition temperature equilibrium constants J The titration of a strong acid with a strong base J The titration of a week acid with a strong base J The titration of a strong base with a strong acid J The titration of a week base with a strong acid J Buffer solutions J Definition and properties eg buffer capacity J Calculation of pH of the buffer solution J Applications Unit Test3 Chapters 1012 SummaryChapters 1011 Derive titration curves of complex acidbase system Mixtures of strong and weak acids or bases Polyfunctional acids and bases Buffer solution involving polyprotic acids Amphiprotic salts eg NaHCO3 General Expression for a values SummaryChapter 12 Basic concepts amp terms 39 Coordination number I Ligand and chelate 39 Unidentate bidentate tridentate 39 Formation constant 39 Conditional formation constants K My K MY Equilibrium Calculations for Complexformation titration Derive EDTA titration curves Calculation of related concentrations Effect of other complexing agents Theory and Calculation of Indicators for EDTA titration Titration Methods employing EDTA Direct titration Backtitration Unit T est4 Chapters 1416 SummaryChapters 1416 Basicconceptsandterms Oxidation and redlction agents and reactions Anode cathode electrode Halfcell reactions electrode potential Galvanic and electrolytic cells Chenical reversible and irreversible reactions Schermtic representation of cells Thermodynanic potential of electrochenical cells SIE standard potential forrral standard potential Indicator and factors of titration cu39ves Calculations Electrode potential Nernst Equation Thermodynanic potentials of electrochenical cell Keq Titration Curves Final Exam 200 points Help Sessions amp Of ce Hours gtThis Wed April 18 Class Hour 52457 PM OCNPS 200 gtNext Friday April 27 23 PM Alfriend Chemistry Building 201 Outside rny Of ce Any Questions Study Really Hard Goodluck to you Dr Nancy Xu Final Review Chem 321 Upcoming Tests 0423 4th Unit Test Chapter 1416 Graded test will be available to pick up outside Rm 200 Chemistry building on April 27 Keys to be posted at the website by April 27 0430 345645 PM Comprehensive Final Examination Chapter 116 except 2 5 and 13 Graded test will be available to pick up outside Rm 200 Chemistry building on May 4 Grade available at Leoonline by May 4 Steps gt Well study all problems in the tests gt Well study all examples that we discussed in the class lecture notes and slides gt Well study all related examples in textbook gt Well study all assigned problems homework Unit Tests gtUnit Test1 Chapters 1 3 4 gtUnit Test2 Chapters 69 gtUnit Test3 Chapters 1012 gtUnit Test4 Chapters 1416 Keys to the Tests httpwww0dueduscixuchem321answershtm Unit Test1 Chapters 1 3 4 SummaryChapter 1 J Course Overview Classi m on of Analysis J Units v Molecular Weight Mole V Concentrations Stoichiometric Calculations v Preparation of Solution SummaryChapter 3 VMean Median Accuracy xPrecision Errors Absolute and Relative Errors rt Systematic or determinate errors 6 Random or indeterminate errors rt Gross errors or blunders SummaryChapter 3 Absolute standard deviation or standard deviation Relative standard deviation Standard deviation of the mean Sm Pooled standard deviation Coefficient of variation Variance s2 xSpread or range Siqnificant Fiqures SummaryChapter 4 Con dence Limit CL Con dence Interval CI Con dence Level Qtest Ttest extra credit F test extra credit Unit Test2 Chapters 69 SummaryChapter 6 V Acids and Bases concepts and strength of Acids and Bases V Equilibriumconstant expression V Types of Equilibrium constants V Pfunctions V Commonion effect V Calculation of equilibrium constants and concentrations eg V Ionproduct constant for water V Solubilityproduct constants V Acid and Base Dissociation Constants SummaryChapter 7 V Molarity V Preparation of solution V Dilution V Titration V Analytical Molarity V Equilibrium or Species Molarity V Percent concentration V PValue V Density amp speci c gravity V Understand concepts titrirnetry equivalence point end point primary standard secondary standard standardization SummaryChapter 7 Titration Curves Titration Curves for a single Anion Titration Curves for Mixtures Anion End Points for Argentometric Titration Chemical Indicators Methods Applications Standard AgNO3 Solution SummaryChapter 8A Ionic Strength Activity Coef cient Activity Types of thermodynamics Equilibrium constants Related calculation and de nition SummaryChapter 8B V Concepts of equilibrium V Equilibrium concentration of every species eg ions solubility in the solution V Equilibriumconstant expressions V Mass concentrationbalance equations V A single chargebalance equation V Calculation of Solubility by the Systematic Method Metal Hydroxides Formation of Complex Ion Separation of ions SummaryChapter 9 J How to select standard solutions and indicators for neutralization titrations J Theory of Indicator Behavior J Titration Curves J Theories Plots and shapes of plots J Parameters pH Volume of titrants equivalence point J Calculations Ka pH indicator choices halfneutralized point J Effects Concentration reaction composition temperature equilibrium constants J The titration of a strong acid with a strong base J The titration of a week acid with a strong base J The titration of a strong base with a strong acid J The titration of a week base with a strong acid J Buffer solutions J Definition and properties eg buffer capacity J Calculation of pH of the buffer solution J Applications Unit Test3 Chapters 1012 SummaryChapters 1011 Derive titration curves of complex acidbase system Mixtures of strong and weak acids or bases Polyfunctional acids and bases Buffer solution involving polyprotic acids Amphiprotic salts eg NaHCO3 General Expression for a values SummaryChapter 12 Basic concepts amp terms 39 Coordination number I Ligand and chelate 39 Unidentate bidentate tridentate 39 Formation constant 39 Conditional formation constants K My K MY Equilibrium Calculations for Complexformation titration Derive EDTA titration curves Calculation of related concentrations Effect of other complexing agents Theory and Calculation of Indicators for EDTA titration Titration Methods employing EDTA Direct titration Backtitration Unit T est4 Chapters 1416 SummaryChapters 1416 Basicconceptsandterms Oxidation and redlction agents and reactions Anode cathode electrode Halfcell reactions electrode potential Galvanic and electrolytic cells Chenical reversible and irreversible reactions Schermtic representation of cells Thermodynanic potential of electrochenical cells SIE standard potential forrral standard potential Indicator and factors of titration cu39ves Calculations Electrode potential Nernst Equation Thermodynanic potentials of electrochenical cell Keq Titration Curves Final Exam 200 points Help Sessions amp Of ce Hours gtThis Wed April 18 Class Hour 52457 PM OCNPS 200 gtNext Friday April 27 23 PM Alfriend Chemistry Building 201 Outside rny Of ce Any Questions Study Really Hard Goodluck to you Dr Nancy Xu

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