This course covers the fundamentals of an Analytical Chemistry course that one might take as a Chemistry major or minor. Ideally, students should have taken a year of General Chemistry as a prerequisite, as much of the material covered relies on a knowledge of equilibrium chemistry.
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This course covers the fundamentals of an Analytical Chemistry course that one might take as a Chemistry major or minor. Ideally, students should have taken a year of General Chemistry as a prerequisite, as much of the material covered relies on a knowledge of equilibrium chemistry.
This course covers the fundamentals of an Analytical Chemistry course that one might take as a Chemistry major or minor. Ideally, students should have taken a year of General Chemistry as a prerequisite, as much of the material covered relies on a knowledge of equilibrium chemistry.
Students in this course have access to ample supplemental material, all of which will be found in the Resource Folders. In addition to the 23 hours of lectures, downloadable audio mp3 files of each lecture are included. For many lectures, a Practice Assignment where you can test your understanding of the material can be found in the Resource Folder. Also included is an answer key for each Practice Assignment. Any graphs, figures or tables presented in the lectures are also available as downloadable files. The content of this course is as extensive as all of my other Chemistry courses are that are also available on Udemy.
This course assumes that you have completed General Chemistry I and ideally General Chemistry II college courses. While you will not need to be familiar with all topics covered in those courses, you should have a good understanding of equilibrium Chemistry. As with my other intermediate courses that I have posted on Udemy, I have review sections for important chemical concepts that are needed for this course. Since this course covers the fundamentals of Analytical Chemistry, most instrumental techniques such as Atomic Absorption, UV-Visible Spectrophotometry, Infrared Spectroscopy, Chromatography and Nuclear Magnetic Resonance are not covered. Section 15 is an introduction to Instrumental Analysis where I introduce colorimetric analysis and Beer's Law, which is the basis for most Instrumental methods. Anyone who is interested in learning about various aspects of Analytical Chemistry may find this course beneficial, especially if you had no prior exposure to Analytical Chemistry in your studies.
What's inside
Learning objectives
- Basic topics of analytical chemistry typically covered in a quantitative analysis university course.
- Understanding the difference between qualitative analysis and quantitative analysis.
- The general steps followed when performing a chemical analysis.
- How units and dimensional analysis applies to calculations in analytical chemistry.
- Solution concentrations used in analytical chemistry.
- How to prepare a specific volume of solution to a desired concentration.
- The specific lab materials for successful analytical results: analytical balance, volumetric glassware, burets, pipets, filtration devices, desiccator and more.
- The difference between random and systematic errors and how to minimize them.
- The difference between accuracy and precision.
- Statistics as they relate to analytical chemistry, i.e., gaussian distribution and how to test for an outlier in a set of results.
- Definition and principles of volumetric analysis.
- Stoichiometric calculations for titrations.
- How to standardize a solution by titration.
- The requirements for a chemical to be a primary standard.
- Definition and steps involved with a gravimetric analysis.
- Stoichiometric calculations for gravimetric analysis.
- The conditional solubility product for gravimetric analysis.
- How to calculate the mass loss of the precipitate in a gravimetric determination.
- Defining ionic strength and how it affects the solubility of slightly soluble salts.
- Activity and activity coefficients and how they affect gravimetric analyses.
- How to form precipitates in the lab with minimal contamination and why this is important.
- The difference between strong and weak acids and bases and how to calculate the ph of their solutions.
- Buffer solutions.
- The applications of the henderson-hasselbalch equation.
- Calculate the ph of amphiprotic species.
- How to calculate the change in ph when an acid or base is added to a buffer solution.
- Buffer capacity.
- How to make a buffer solution to a specific ph.
- Determining the predominant species in an acidic or basic solution.
- Derivation of fractional composition equations for monoprotic and polyprotic acids.
- Application of fractional composition equations.
- Stoichiometric calculations for a chemical analysis by titration.
- How to construct a titration curve for neutralization reactions.
- Indicators used in acid-base titrations, the titration error and how to calculate it.
- Choice of indicator for an acid-base titration.
- Complexometric titrations.
- Fractional composition equations for the ligand edta.
- The conditional formation constant for complexometric titrations.
- How to construct complexometric titration curves.
- Auxiliary complexing agents and how and why they may be used in a complexometric titration.
- Chemical analysis by complexometric titration.
- Indicators used in complexometric titrations.
- Back titrations.
- How to construct titration curves for redox titrations.
- Redox titration indicators.
- Requirements of colorimetric analysis.
- How to construct and interpret a beer's law graph.
- How to prepare standard solutions for colorimetric analysis.
- Steps involved in a colorimetric determination.
- Chemical analysis by colorimetric analysis.
- Show more
- Show less
- Basic topics of analytical chemistry typically covered in a quantitative analysis university course.
- Understanding the difference between qualitative analysis and quantitative analysis.
- The general steps followed when performing a chemical analysis.
- How units and dimensional analysis applies to calculations in analytical chemistry.
- Solution concentrations used in analytical chemistry.
- How to prepare a specific volume of solution to a desired concentration.
- The specific lab materials for successful analytical results: analytical balance, volumetric glassware, burets, pipets, filtration devices, desiccator and more.
- The difference between random and systematic errors and how to minimize them.
- The difference between accuracy and precision.
- Statistics as they relate to analytical chemistry, i.e., gaussian distribution and how to test for an outlier in a set of results.
- Definition and principles of volumetric analysis.
- Stoichiometric calculations for titrations.
- How to standardize a solution by titration.
- The requirements for a chemical to be a primary standard.
- Definition and steps involved with a gravimetric analysis.
- Stoichiometric calculations for gravimetric analysis.
- The conditional solubility product for gravimetric analysis.
- How to calculate the mass loss of the precipitate in a gravimetric determination.
- Defining ionic strength and how it affects the solubility of slightly soluble salts.
- Activity and activity coefficients and how they affect gravimetric analyses.
- How to form precipitates in the lab with minimal contamination and why this is important.
- The difference between strong and weak acids and bases and how to calculate the ph of their solutions.
- Buffer solutions.
- The applications of the henderson-hasselbalch equation.
- Calculate the ph of amphiprotic species.
- How to calculate the change in ph when an acid or base is added to a buffer solution.
- Buffer capacity.
- How to make a buffer solution to a specific ph.
- Determining the predominant species in an acidic or basic solution.
- Derivation of fractional composition equations for monoprotic and polyprotic acids.
- Application of fractional composition equations.
- Stoichiometric calculations for a chemical analysis by titration.
- How to construct a titration curve for neutralization reactions.
- Indicators used in acid-base titrations, the titration error and how to calculate it.
- Choice of indicator for an acid-base titration.
- Complexometric titrations.
- Fractional composition equations for the ligand edta.
- The conditional formation constant for complexometric titrations.
- How to construct complexometric titration curves.
- Auxiliary complexing agents and how and why they may be used in a complexometric titration.
- Chemical analysis by complexometric titration.
- Indicators used in complexometric titrations.
- Back titrations.
- How to construct titration curves for redox titrations.
- Redox titration indicators.
- Requirements of colorimetric analysis.
- How to construct and interpret a beer's law graph.
- How to prepare standard solutions for colorimetric analysis.
- Steps involved in a colorimetric determination.
- Chemical analysis by colorimetric analysis.
- Show more
- Show less
Syllabus
Introduction
In this lecture I define Analytical Chemistry and discuss the three general methods of analysis.
In this lecture, I discuss the general steps taken in a chemical analysis: Sampling, Sample Preparation and Analyzing the Sample.
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Syllabus
In this lecture I define Analytical Chemistry and discuss the three general methods of analysis.
In this lecture, I discuss the general steps taken in a chemical analysis: Sampling, Sample Preparation and Analyzing the Sample.
In this lecture I do a quick review of the 7 SI Base Units, Derived Units and prefixes used with the metric system.
In this lecture I show how to apply dimensional analysis to converting units.
In this lecture, I review what is a solution and the concentration units of mass percent, parts per million and billion, molarity and formality.
We this lecture we see how density of the solution is needed to convert between these two concentration units going in either direction.
In this lecture I explain how to prepare solutions for analytical work and how to do the calculations.
In this lecture I discuss the differences between a top-loading balance and an analytical balance, when to use each, and the rules for using an analytical balance.
Items included in volumetric glassware, the two types and rules for using are discussed in this lecture.
In this lecture we discuss how to use and read a buret.
A few more details about volumetric flasks are added in this lecture.
Details about the pipet are given in this lecture.
In this lecture, three types of filtration devices are discussed.
In this lecture, the parts of a desiccator and use are explained.
A review of significant figures with emphasis on significant figures in measurements and when zeroes are significant.
In this lecture, I explain how to round your answer to the correct number of significant figures when adding or subtracting.
In this lecture, I explain how to round your answer to the correct number of significant figures when multiplying or dividing.
In this lecture the definition and difference between random and systematic lab errors is discussed. Examples of both are given.
In this lecture, I discuss what is meant by precision, accuracy, absolute error, relative error and how to minimize random error.
In this lecture, the Gaussian Distribution and standard deviation are defined and discussed.
In this lecture, I discuss how to identify a data point that might need to be rejected and how to go about determining that.
In this lecture, I describe the requirements of volumetric analysis, list the requirements for a successful titration and discuss the two types of titrations: direct titrations and back titrations.
In this lecture, I show how to calculate the mass % of an analyte in a sample by a titration.
In this lecture, I explain how a solution is standardized to a known concentration, then used to determine the molarity of another reagent and the mass % of an analyte in an unknown sample.
In this lecture, I review how to set up the equilibrium constant equation for insoluble salts, weak acids and bases, and complex ions.
In this lecture, I list and discuss the steps involved in a gravimetric determination.
Calculations for two examples of gravimetric analysis are given in this lecture.
In this lecture I explain how to calculate the mass and % loss of the precipitate from the slight dissolving of the slightly soluble precipitate.
In this lecture I define ionic strength and explain why a high solution ionic strength increases the solubility of slightly soluble salts.
In this lecture, activity and activity coefficients are defined and explained and several applications are given.
In this lecture, I show how to calculate mass and % loss of a precipitate taking activity into account.
In this lecture, I discuss the theory of precipitation, how impurities can contaminate your precipitate and steps you can take to form the purest precipitate.
In this lecture, I define Bronsted-Lowry acids and bases as well as explaining how to determine acid-base conjugate pairs.
In this lecture, I review how to calculate hydronium ion concentrations and hydroxide ion concentrations from the Kw equation and then a quick review of pH calculations.
In this lecture, I explain the difference between strong and weak acids and bases and how to recognize them. I also discuss the relationship between Ka and Kb for acid-base conjugate pairs.
In this lecture, I review how to calculate the pH of strong acid and base solutions given their molar concentration.
In this lecture, I review how to calculate the pH of a weak acid solution.
In this lecture, I review how to calculate the pH of a weak base solution.
In this lecture, I define buffer solutions, explain what they consist of and how they react to added acids and bases.
In this lecture, I review pKa and the Henderson-Hasselbalch equation showing how it is used to calculate the pH of buffer solutions and its limitations.
In this lecture, I explain how to make buffer solutions using polyprotic acids.
In this lecture, I derive the equation needed to calculate the pH of amphiprotic species solutions. We also see how it can be simplified in most cases.
In this lecture, I show how to calculate the change in pH of a buffer solution if an acid or base is added to it.
In this lecture, I define buffer capacity and show how to determine which solutions have higher buffer capacity.
In this lecture, I discuss several different ways to make a buffer to a specific pH.
In this lecture, I show how you can determine the predominant species in a weak acid or weak base equilibrium system.
In this lecture, I derive the fractional composition equations for a monoprotic acid and show what a graph of these equations would look like.
In this lecture, I derive the fractional composition equations for a polyprotic acid and show what a graph of these equations would look like.
In this lecture, I explain how to calculate the molar concentrations of all species in a solution knowing the formal concentration of the acid or base and alpha values of each species.
In this lecture, I explain how to calculate the percent amount of analyte in a sample by titration
In this lecture, I define a titration curve and explain why it is important.
In this lecture, I construct a titration curve for a titration of a strong acid with a strong base.
In this lecture, I construct a titration curve for a titration of a strong base with a strong acid.
In this lecture, I construct a titration curve for a titration of a weak acid with a strong base.
In this lecture, I construct a titration curve for a titration of a weak base with a strong acid.
In this lecture, I construct a titration curve for a titration of a diprotic base with a strong acid.
In this lecture, I explain why a titration of a weak acid with a weak base (or vice versa) won't work.
In this lecture, I explain the chemistry of indicators and show why it's important to add no more than 2-3 drops in indicator to the solution.
In this lecture, I show by calculation, how to choose the correct indicator for a titration knowing the analyte and titrant.
In this lecture, I explain complexometric titrations, the formation constant equilibrium equation and the beta equations for complex ion formation.
In this lecture, I show how to address the hexaprotic EDTA molecule and calculate the fractional amount of the totally deprotonated form of the molecule using fractional compositional equations covered in Section 10.
Inn this lecture, I show how to calculate the conditional formation constant and why it is necessary.
In this lecture, I explain the calculations necessary for constructing a titration curve for Mg(2+) with EDTA.
In this lecture, I define an auxiliary complexing agent, why it is used and how it enters into equilibrium calculations.
In this lecture, I explain the calculations necessary for constructing a titration curve for Cd(2+) with EDTA and using NH3 an auxiliary complexing agent.
In this lecture, I explain how to calculate the percent amount of analyte in a sample by complexometric titration.
In this lecture, I discuss metal ion indicators, how they are similar, how they are different from acid-base indicators and how to select the correct indicator for a particular complexometric titration.
In this lecture, I explain what a back titration is, when it might be used, its requirements and the calculations involved.
In this lecture, I review oxidation and reduction, half-reactions and standard reduction potentials.
In this lecture, I review the Nernst equation and show its application.
In this lecture, I explain the calculations necessary for constructing a redox titration curve for Fe(2+) with Ce(4+).
In this lecture, I explain the calculations necessary for constructing a redox titration curve when there is an unequal number of electrons transferred between the two half-reactions.
In this lecture, I explain how redox titration indicators work and how to select the correct one for a particular titration.
In this lecture, I define colorimetric analysis and give an overview on how the method works.
In this lecture, I discuss the schematics of a spectrophotometer, give the Beer's Law equation and explain how it is used in a colorimetric analysis.
In this lecture, I describe each step involved in a Colorimetric Analysis
In this lecture, I give a detailed example of how a colorimetric analysis would be performed and how the calculations would be done.
This video supplements Lecture 8 on the use of the Analytical Balance.
This video supplements Lecture 10 on the use of Burettes.
This video supplements Lecture 12 on the use of Pipettes.
This video supplements Lecture 13 on the use of Filters.
This video supplements Lecture 13 on the filtering processes.
This video supplements Lecture 14 on the use of Desiccators.
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Reviews summary
Foundational analytical chemistry for students
Excellent for review or supplementing studies.
Supplemental materials reinforce learning.
Lectures are well-explained and engaging.
Covers fundamental theory and calculations.
Activities
Review General Chemistry Concepts
Show steps
Reinforce your understanding of fundamental chemistry principles, particularly equilibrium, to better grasp analytical chemistry concepts.
Browse courses on
General Chemistry
Show steps
-
Review notes and textbooks from your General Chemistry courses.
-
Work through practice problems related to equilibrium, acids, and bases.
-
Identify areas where your understanding is weak and focus your review there.
Read 'Quantitative Chemical Analysis' by Daniel C. Harris
Show steps
Supplement the course material with a comprehensive textbook that provides in-depth explanations and examples.
View
Student Solutions Manual for the 10th Edition...
on Amazon
Show steps
-
Obtain a copy of 'Quantitative Chemical Analysis' by Daniel C. Harris.
-
Read the chapters relevant to the course syllabus, focusing on areas where you need more clarification.
-
Work through the example problems and end-of-chapter exercises to test your understanding.
Practice Titration Calculations
Show steps
Reinforce your understanding of titration calculations through repetitive practice.
Show steps
-
Find practice problems online or in textbooks related to acid-base, complexometric, and redox titrations.
-
Work through the problems step-by-step, paying attention to stoichiometry and equilibrium constants.
-
Check your answers and review the solutions to understand any mistakes you made.
Four other activities
Expand to see all activities and additional details
Show all seven activities
Tutor other students
Show steps
Reinforce your understanding of the course material by helping other students.
Show steps
-
Offer to tutor classmates who are struggling with the material.
-
Prepare explanations and examples to help them understand the concepts.
-
Answer their questions and provide feedback on their work.
Create a Titration Curve Visualization
Show steps
Solidify your understanding of titration curves by creating a visual representation of the data.
Show steps
-
Choose a specific type of titration (e.g., strong acid-strong base, weak acid-strong base).
-
Calculate the pH at various points during the titration.
-
Use a spreadsheet program or graphing software to plot the pH versus the volume of titrant added.
-
Annotate the graph with key features, such as the equivalence point and buffer region.
Explore 'Analytical Chemistry: A Modern Approach to Analytical Science' by Kenneth A. Rubinson and Judith F. Rubinson
Show steps
Broaden your understanding of analytical techniques and applications with a modern textbook.
View
Melania
on Amazon
Show steps
-
Obtain a copy of 'Analytical Chemistry: A Modern Approach to Analytical Science' by Kenneth A. Rubinson and Judith F. Rubinson.
-
Browse the chapters on instrumental techniques and applications that are not covered in detail in the course.
-
Focus on understanding the basic principles and instrumentation of each technique.
Design a Gravimetric Analysis Experiment
Show steps
Apply your knowledge of gravimetric analysis by designing a hypothetical experiment.
Show steps
-
Choose an analyte and a precipitating agent for a gravimetric determination.
-
Develop a detailed procedure for the experiment, including sample preparation, precipitation, filtration, drying, and weighing.
-
Calculate the expected yield and error for your experiment.
-
Identify potential sources of error and suggest ways to minimize them.
Review General Chemistry Concepts
Show steps
Reinforce your understanding of fundamental chemistry principles, particularly equilibrium, to better grasp analytical chemistry concepts.
Browse courses on
General Chemistry
Show steps
- Review notes and textbooks from your General Chemistry courses.
- Work through practice problems related to equilibrium, acids, and bases.
- Identify areas where your understanding is weak and focus your review there.
Read 'Quantitative Chemical Analysis' by Daniel C. Harris
Show steps
Supplement the course material with a comprehensive textbook that provides in-depth explanations and examples.
View
Student Solutions Manual for the 10th Edition...
on Amazon
Show steps
- Obtain a copy of 'Quantitative Chemical Analysis' by Daniel C. Harris.
- Read the chapters relevant to the course syllabus, focusing on areas where you need more clarification.
- Work through the example problems and end-of-chapter exercises to test your understanding.
Practice Titration Calculations
Show steps
Reinforce your understanding of titration calculations through repetitive practice.
Show steps
- Find practice problems online or in textbooks related to acid-base, complexometric, and redox titrations.
- Work through the problems step-by-step, paying attention to stoichiometry and equilibrium constants.
- Check your answers and review the solutions to understand any mistakes you made.
Tutor other students
Show steps
Reinforce your understanding of the course material by helping other students.
Show steps
- Offer to tutor classmates who are struggling with the material.
- Prepare explanations and examples to help them understand the concepts.
- Answer their questions and provide feedback on their work.
Create a Titration Curve Visualization
Show steps
Solidify your understanding of titration curves by creating a visual representation of the data.
Show steps
- Choose a specific type of titration (e.g., strong acid-strong base, weak acid-strong base).
- Calculate the pH at various points during the titration.
- Use a spreadsheet program or graphing software to plot the pH versus the volume of titrant added.
- Annotate the graph with key features, such as the equivalence point and buffer region.
Explore 'Analytical Chemistry: A Modern Approach to Analytical Science' by Kenneth A. Rubinson and Judith F. Rubinson
Show steps
Broaden your understanding of analytical techniques and applications with a modern textbook.
View
Melania
on Amazon
Show steps
- Obtain a copy of 'Analytical Chemistry: A Modern Approach to Analytical Science' by Kenneth A. Rubinson and Judith F. Rubinson.
- Browse the chapters on instrumental techniques and applications that are not covered in detail in the course.
- Focus on understanding the basic principles and instrumentation of each technique.
Design a Gravimetric Analysis Experiment
Show steps
Apply your knowledge of gravimetric analysis by designing a hypothetical experiment.
Show steps
- Choose an analyte and a precipitating agent for a gravimetric determination.
- Develop a detailed procedure for the experiment, including sample preparation, precipitation, filtration, drying, and weighing.
- Calculate the expected yield and error for your experiment.
- Identify potential sources of error and suggest ways to minimize them.
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