Acids-Bases Course

Lesson 1 • Brønsted-Lowry Proton Transfer Model

Extends acid-base behavior to any proton-transfer reaction regardless of solvent. Introduces conjugate acid-base pairs as a central organizing concept.

Lesson 2 • Lewis Electron-Pair Model

Defines acids as electron-pair acceptors and bases as electron-pair donors, broadening scope beyond proton transfer. Connects acid-base behavior to coordination chemistry.

Lesson 3 • Arrhenius Definition and Scope

Defines acids as proton donors and bases as hydroxide donors in aqueous solution. Establishes the simplest model as a baseline for comparing later frameworks.

Lesson 4 • Comparing and Selecting Theoretical Models

Evaluates the predictive power and appropriate context for each model. Equips students to choose the correct framework for a given chemical scenario.

Lesson 1 • Measuring pH in Practice

Covers instrumental and indicator-based methods for determining pH experimentally. Links measurement accuracy to proper calibration and sample handling.

Lesson 2 • Calculating pH of Strong Acids and Bases

Applies complete dissociation assumption to calculate pH directly from concentration. Builds computational fluency before tackling partial dissociation.

Lesson 3 • The pH and pOH Scales

Defines pH and pOH as logarithmic measures of ion concentration. Connects the two scales through the water ion-product constant.

Lesson 1 • Polyprotic Acids and Stepwise Dissociation

Extends equilibrium analysis to acids that donate more than one proton. Shows how successive Ka values govern each dissociation step.

Lesson 2 • Equilibrium Constants for Weak Bases

Defines the base dissociation constant and connects it to the acid dissociation constant of the conjugate acid. Extends the equilibrium framework to basic solutions.

Lesson 3 • Factors Affecting Acid and Base Strength

Connects molecular structure—bond polarity, electronegativity, resonance—to Ka and Kb values. Enables prediction of relative acid-base strength from structure.

Lesson 4 • Equilibrium Constants for Weak Acids

Defines the acid dissociation constant and explains its relationship to acid strength. Establishes the mathematical framework used throughout weak-acid calculations.

Lesson 1 • Biological and Industrial Buffer Applications

Surveys how buffers maintain pH in blood, cell culture, food processing, and manufacturing. Connects design principles to real-world performance requirements.

Lesson 2 • Henderson-Hasselbalch Equation

Derives and applies the Henderson-Hasselbalch equation for rapid pH estimation. Links component ratio to buffer pH for design and analysis.

Lesson 3 • Buffer Composition and Mechanism

Explains how a weak acid and its conjugate base neutralize added acid or base. Establishes the chemical logic underlying buffer resistance.

Lesson 4 • Buffer Capacity and Range

Quantifies how much acid or base a buffer can absorb before pH shifts significantly. Defines the effective pH range as pKa plus or minus one unit.

Lesson 1 • Hydrolysis of Salts

Explains how dissolved salts produce acidic or basic solutions through ion hydrolysis. Predicts solution pH from the nature of the parent acid and base.

Lesson 2 • Acid-Base Reactions in Non-Aqueous Media

Extends acid-base concepts to solvents other than water using the Brønsted-Lowry and Lewis frameworks. Highlights how solvent choice affects reaction outcomes.

Lesson 3 • Amphoteric Species and Zwitterions

Identifies species that act as both acids and bases depending on conditions. Introduces amino acids as biologically relevant amphoteric molecules.

Lesson 1 • Weak Acid–Strong Base Titration Curves

Extends titration curve analysis to weak acid systems where buffer regions appear. Connects half-equivalence point to pKa determination.

Lesson 2 • Polyprotic Acid Titration Curves

Analyzes titration curves with multiple equivalence points for polyprotic acids. Demonstrates how each step corresponds to successive proton removal.

Lesson 3 • Titration Fundamentals and Setup

Defines titration as a volumetric technique for quantitative acid-base analysis. Covers equipment, standardization of titrant, and proper technique.

Lesson 4 • Strong Acid–Strong Base Titration Curves

Calculates pH at each stage of a strong acid–strong base titration. Identifies the sharp equivalence-point inflection and its significance.

Lesson 1 • Quality Control in Acid-Base Analysis

Applies statistical tools and standard reference materials to validate analytical results. Ensures measurements meet regulatory and professional accuracy standards.

Lesson 2 • Potentiometric Methods and Ion-Selective Electrodes

Explains how electrochemical cells measure pH and ion activity in solution. Covers electrode types, calibration, and common interferences.

Lesson 3 • Spectrophotometric pH Determination

Uses absorbance of pH-sensitive indicators to determine solution pH quantitatively. Connects Beer-Lambert law to indicator equilibrium for calibration.

Lesson 1 • Computational Approaches to Acid-Base Problems

Introduces software tools and iterative numerical methods for solving complex equilibrium systems. Prepares students to handle multi-component acid-base problems beyond manual calculation.

Lesson 2 • Physiological Acid-Base Balance

Examines how the body maintains blood pH through respiratory and renal compensation. Introduces acidosis and alkalosis as clinical acid-base disorders.

Lesson 3 • Industrial Acid-Base Processes

Surveys large-scale industrial processes that depend on precise acid-base control. Includes synthesis, neutralization, and waste treatment applications.

Lesson 4 • Acid-Base Chemistry in Environmental Systems

Analyzes ocean acidification, acid rain, and soil pH as consequences of acid-base equilibria. Connects atmospheric chemistry to aquatic and terrestrial pH changes.