Chemical Equilibria and Acid-Base Chemistry (Undergraduate Foundation)

This course provides a complete guide to chemical equilibria, the state where the rates of forward and reverse reactions are equal. It covers the law of mass action, the definition and calculation of the equilibrium constant, and the factors that can cause a shift in the equilibrium position. The course then applies these principles to the study of aqueous equilibria, including the properties of acids, bases, and salts, and the calculation of pH. The principles of equilibrium govern the outcomes of all reversible reactions, from industrial synthesis to biological processes. A command of this topic is essential for chemists and chemical engineers to maximise the yield of a desired product, for environmental scientists to understand natural water systems, and for biochemists to analyse metabolic pathways. By the end of this course, you will be able to write the expression for the equilibrium constant for any reversible reaction, use Le Chatelier's principle to predict how a system at equilibrium will respond to changes in concentration, pressure, or temperature, and perform calculations involving the pH of acidic and basic solutions. This course is for students who have a solid foundation in stoichiometry. It is a mandatory course for all students of chemistry and chemical engineering and is a direct prerequisite for the study of analytical chemistry, biochemistry, and environmental science.

8 hrs

Enrolment valid for 12 months

This course is also part of the following learning track. You may join the track to gain comprehensive knowledge across related courses.

CHM 101: General Chemistry I

This learning track delivers the complete NUC CCMAS curriculum for General Chemistry I. It is a comprehensive programme designed to build a robust, university-level foundation in modern chemistry. The track systematically covers all essential topics, from atomic theory, chemical bonding, and the states of matter, to the quantitative principles of stoichiometry, equilibrium, thermodynamics, and kinetics. This programme is for first-year undergraduates in science, technology, engineering, and mathematics (STEM) faculties who are required to take CHM 101. It is also essential for any student or professional globally who needs a rigorous and complete foundation in first-year university chemistry for further study or career development. This track delivers a full skill set in chemical theory and quantitative problem-solving. Graduates will be able to determine molecular structures, calculate reaction quantities, analyse the energetics and rates of reactions, and solve complex equilibrium problems. This programme provides the non-negotiable prerequisite knowledge for all subsequent chemistry courses and for any degree in the physical sciences, engineering, or medicine.

Course Chapters

1. Introduction

This chapter provides the roadmap for the course. It introduces the concept of a dynamic, reversible chemical reaction and outlines the progression from the principles of equilibrium to their application in acid-base chemistry. Key learning objectives include: understanding the overall course structure and appreciating the importance of equilibrium in controlling the outcomes of chemical reactions.

Concept Overviews

1 Lesson

4:29

2. Chemical Equilibrium

This chapter establishes the foundational mechanics of reversible reactions and the dynamic state of equilibrium. Mastering these principles is vital for quantifying reaction yields and predicting the behaviour of chemical systems in industrial and biological environments. You will master five objectives: defining the dynamic equilibrium state; interpreting rate and concentration graphs; deriving Kc expressions via the law of mass action; differentiating phase-dependent equilibria; and calculating Kp for gaseous systems.

Concept Overviews

5 Lessons

40:48

3. Stoichiometric Relations

This chapter examines the mathematical dependence of the equilibrium constant on the stoichiometry of the chemical equation. Understanding these correlations is essential for correctly modifying Kc values when reversing reactions, scaling coefficients, or combining multiple elementary steps in industrial process design. You will master four objectives: calculating the reciprocal constant for reversed reactions; determining new Kc values for scaled stoichiometric coefficients; applying the rule of multiple equilibria for multi-step reactions; and establishing consistent units for the equilibrium constant.

Concept Overviews

1 Lesson

10:15

Problem Walkthroughs

3 Lessons

29:52

4. Le Chatelier's Principle

This chapter covers the qualitative analysis of equilibrium shifts in response to external stresses. Mastering Le Chateliers principle is mandatory for predicting and controlling the direction of reversible reactions in industrial and biological systems. You will master the mechanical prediction of directional shifts caused by concentration changes; the resolution of gaseous equilibria under varying pressure or volume; the effect of temperature on exothermic and endothermic reactions; and the role of catalysts in kinetic acceleration.

Concept Overviews

5 Lessons

41:56

Problem Walkthroughs

3 Lessons

31:20

5. Acids, Bases, and Salts

This chapter applies equilibrium principles to acid-base chemistry, a critical area for understanding chemical reactivity in industrial and biological systems. You will master the quantitative tools needed to predict and control the behaviour of aqueous solutions. By the end, you will define acids and bases using Arrhenius, Bronsted-Lowry, and Lewis theories; calculate pH and pOH for strong and weak electrolytes; predict salt hydrolysis outcomes; and design buffer systems to resist pH changes.

Concept Overviews

10 Lessons

1:25:00

Problem Walkthroughs

11 Lessons

1:25:29

6. Solubility and Solubility Products

This chapter bridges chemical equilibria with the practical solubility of salts in water. It explains why some substances dissolve while others form precipitates, providing the tools needed to predict reaction outcomes in industrial and environmental chemistry. You will master the solubility product constant, the common ion effect, and the use of the reaction quotient to determine if a precipitate will form. You will also learn to calculate molar solubility and understand how pH influences the dissolving process.

Concept Overviews

2 Lessons

4:30

Problem Walkthroughs

6 Lessons

22:16

7. Solubility Equilibria and Precipitation

This chapter explains how solids dissolve in water until they reach a balance. It is vital for understanding how scale forms in pipes, how bones grow, and how to remove pollutants from liquid waste. You will learn to predict if a solid will settle out of a liquid and how to control this process in the lab or industry. By the end, you will master writing solubility product expressions, calculating molar solubility from constants, and predicting precipitate formation using the ion product.

Concept Overviews

1 Lesson

3:39

Problem Walkthroughs

3 Lessons

21:03