Course Code: CHEM4441 Course Title: Analytical Chemistry II

Transcription

1 College of Science Department of Chemistry Course Code: CHEM4441 Course Title: Analytical Chemistry II General Inmation Number of Credits: 3. Instructional Format: hours Lectures + 3 hours lab Contact Hours/Week: 5 Prerequisite: CHEM 3341 Analytical Chemistry I. Assessment: Homework, Lab, Tests, Final examination Grading (A F, Pass/Fail): Grading (A F) Textbook: Quantitative Chemical Analysis, by D. C. Harris, 8 th Edition. References (optional): Fundamentals of Analytical Chemistry, by D. A. Skoog, D. M. West, F. J. Holler, S. R. Crouch, 8 th Edition. 1. Course Description The course is a continuation of CHEM 3341 intended Chemistry majors. Analytical techniques studied in CHEM 3341 will be developed furr and some more advanced techniques, including some instrumental methods, will be introduced... Course Objective At end of course, you will be able to: 1. Apply statistics in reporting and analyze data, be familiar with classical techniques such as gravimetric, combustion and methods.. Introduce students to basic concepts of electrochemistry,, titrants and applications of s. 3. Expose students to spectrophotometric techniques, its application and instrumentation. 4. Motivate students to acquire critical thinking and problem solving ability. 5. Equip students with skills to write scientific report. 3. Learning Outcomes (a) Knowledge and Understanding On successful completion of course, you will be able to: 1. Express data using techniques and apply basic quality control methods.. Distinguish correct calibration methods a given chemical analysis problem. 3. Apply redox equilibria and Nernest equation to develop electro methods. 4. Identify essential components of spectrophotometers, errors in spectrochemical analysis and areas of applications of spectrophotometry. 5. Identify and apply advanced gravimetric and rmogravimetric techniques. 1

2 6. Recognize proper procedures and regulations safe handling and use of chemicals. (b) Skills On successful completion of course, you will be able to: 1. Use modern instrumentation and classical techniques, to design experiments.. Practice applying scientific methods in collection of data, and to use modern techniques in analysis and results. 3. Be skilled in problems solving, critical thinking and reasoning. 4. Interpret and communicate results of chemical analysis. 5. Practice processes and procedures creating and completing successful writing in chemistry. (c) Attitudes On successful completion of course, you will be able to: 1. Think independently and logically.. Be a good team player in order to achieve to achieve common goals 4. Assessment Assessment Criteria Learning outcomes: By end of course, students will be able to: Recognize notion least square methods and apply se method in chemistry Interpret quality assurance methods and employ methods to validate methods Use gravimetric methods to compute concentrations of analytes and to solve problems. Assessment criteria A B C D F least square method and its Excellent use techniques to determine and explain basic quality parameters and to validate methods Mastery use of calculations and proper interpretation of results. An all-round least square Good methods determination and explanation of basic quality validation of Good application calculations and to properly interpret calculation results. An acceptable least square method and its Acceptable explanation of basic quality parameters and validation of Acceptable use of calculations. A bare knowledge least square Less than satisfactory explanation of basic quality validation of Limited evidence of skill to use calculations. basics least square Unrelated explanation of basic quality validation of Evidence of lack of acquired skills to.

3 Learning outcomes: Recognize and explain basics of electrochemistry and use of galvanic cells and Nernst equation Employ redox titrations, interpret titration curves and iate Recognize and explain basics of spectrophotomet ry and apply spectrophotomet ric methods to solve problems. Describe components of spectrohpotomet rs and explain ir operation principles. Assessment criteria A B C D F of good basics exhibit a Demonstration Satisfactory Barely able to of electrochemistry basics of basics of basics of and acceptable skills basics of electrochemistry. electrochemist electrochemistr in using Nernst electrochemistry ry and mastery y and good use concept. use of of Nernst Nernst concept. concept. Accurate and well thought interpretation of redox titration Differentiation redox reactions Showing a clear mastery of spectrophotom etry and its knowledge in structure of ir operation. Appropriate Differentiation redox reactions. Having a good grasp of spectrophotome tric techniques and ir An all-round knowledge in structure of ir operation. Satisfactory Differentiation of redox reactions A satisfactory grasp of spectrophotometric techniques. Acceptable knowledge in structure of ir operation Limited evidence of grasp of Differentiation of redox reactions. Less than satisfactory grasp of spectrophotometri c techniques. Limited knowledge in structure of ir operation Inability to interpret redox titration systems and to e redox reactions. basics spectrophotometr y. knowledge in structure of ir operation 5. Course Structure The course is designed to be delivered in one semester of 15 weeks with 5 contact hours per week ( hours ory and 3 hours lab). The course weight is 3 credit hours. 6. Topics Chapter Topics Sections Weeks 4 Least square methods 4.7 The method of least square Calibration curves 4.9 A spread sheet least squares. 5 Quality Assurance and 5.1 Basics of quality assurance Calibration methods 5. Method validation 5.3 Standard addition methods 5.4 Internal standards 6 Gravimetric Analysis, 6.1 Examples of gravimetric analysis 3

4 Precipitation Titration, and Combustion Analysis 6. Precipitation 6.3 Examples of gravimetric calculations 6.4 Combustion analysis Chapter Topics Sections Weeks 13 Fundamentals of Electrochemistry 13.1 Basic concepts 13. Galvanic cells 13.3 Standard potentials 13.4 Nernst equation 13.5 E 0 and equilibrium constant 13.6 Cells as chemical probes 13.7 Biochemists use E 0' 15 Redox Titration 15.1 The shape of a titration curve 15. Finding end point 15.3 Adjustment of analyte oxidation state 15.4 Oxidation with potassium permanganate 15.5 Oxidation with Ce(IV) 15.6 Oxidation with potassium dichromate 15.7 Methods involving iodine 17 Fundamentals of Spectrophotometry 18 Application of spectrophotometry 17.6 What happens when a molecule absorbs light? 17.7 Luminescence 18.1 Analysis of a mixture 18. Measuring an equilibrium constant 18.3 The method of continuous variation 18.4 Flow injection analysis 18.5 Immunoassays and aptamers 18.6 sensors based on luminescence 19 Spectrophotometers 19.1 Lamps and lasers 19. Monochromators 19.3 Detectors 19.4 Optical sensors 19.5 Fourier transm infrared spectroscopy 7. Lab/Tutorial/Homework content Week/Lab# Contents /1 EXPERIMENT 1: An exercise in volumetric analysis 3/ EXPERIMENT : Determination of chloride by gravimetric analysis 5/3 EXPERIMENT 3: Redox titration 6/4 EXPERIMENT 4: Determination of ascorbic acid vitamin C tablets 8/5 EXPERIMENT 5: Beer's law and determination of iron in water 9/6 EXPERIMENT 5: Determination of phosphate in detergents. 10/7 EXPERIMENT 7: Determination of iron by Jone's reductor 11/8 EXPERIMENT 8: Simultaneous spectrophotometric determination 13/9 EXPERIMENT 9: Optimization of separation using normal and reversed phase chromatography. 4

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