Lecture
This lecture covers the concept of buffer solutions, which are resistant to pH changes upon addition of acids or bases. The equilibrium between a weak acid and its conjugate base determines the buffer capacity. Examples and calculations of buffer solutions are provided, along with the Henderson-Hasselbalch equation. The lecture also discusses the importance of pH in various buffer systems, such as blood. Polyprotic acids and bases, as well as their equilibrium constants, are explained. The session concludes with a discussion on the properties of solutions and solubility equilibria in chemistry.