CU-204 Acids, Bases & Buffers

Unit · year 2

CU-204 · Acids, Bases & Buffers

Threads equilibrium24 lectures5 results

Proton transfer, the pH scale, and the chemistry of buffered solutions.

PREREQUISITES

L01	Arrhenius, Brønsted, and Lewis Definitions The Bronsted-Lowry theory
L02	Conjugate Acid–Base Pairs The Bronsted-Lowry theory
L03	Strength of Acids and Bases The Bronsted-Lowry theory
L04	Autoionisation of Water Autoionisation of water and pH
L05	The pH Scale Autoionisation of water and pH
L06	pH of Strong Acids and Bases Autoionisation of water and pH
L07	Ka, Kb, and pKa The Bronsted-Lowry theory
L08	pH of Weak Acid Solutions —
L09	Percent Ionisation and Dilution —
L10	Salt Hydrolysis —
L11	Buffer Solutions: How They Work The Henderson-Hasselbalch equation
L12	The Henderson–Hasselbalch Equation The Henderson-Hasselbalch equation
L13	Buffer Capacity and Useful Range The Henderson-Hasselbalch equation
L14	Preparing a Buffer at a Target pH The Henderson-Hasselbalch equation
L15	Biological Buffer Systems The Henderson-Hasselbalch equation
L16	Acid–Base Titration: The Setup Titration curves
L17	Strong Acid–Strong Base Curves Titration curves
L18	Weak Acid–Strong Base Curves Titration curves
L19	The Half-Equivalence Point Titration curves, The Henderson-Hasselbalch equation
L20	Indicators and Endpoint Selection Titration curves
L21	Polyprotic Acids Polyprotic acids
L22	Stepwise Dissociation Constants Polyprotic acids
L23	Speciation Diagrams Polyprotic acids
L24	Synthesis: Proton Transfer, Quantified Autoionisation of water and pH, The Henderson-Hasselbalch equation

Acids and bases as proton donors and acceptors.

Kw and the definition of the pH scale.

Buffer pH from the acid-to-base ratio.

Equivalence points and the choice of indicator.

Stepwise dissociation and successive constants.