7: Buffers, Titrations and Solubility Equilibria
-
- 7.1: Acid-Base Buffers
- A solution containing a mixture of an acid and its conjugate base, or of a base and its conjugate acid, is called a buffer solution. Unlike in the case of an acid, base, or salt solution, the hydronium ion concentration of a buffer solution does not change greatly when a small amount of acid or base is added to the buffer solution. The base (or acid) in the buffer reacts with the added acid (or base).
-
- 7.2: Practical Aspects of Buffers
- Buffers are solutions that resist a change in pH after adding an acid or a base. Buffers contain a weak acid ([latex]HA[/latex]) and its conjugate weak base ([latex]A^−[/latex]). Adding a strong electrolyte that contains one ion in common with a reaction system that is at equilibrium shifts the equilibrium in such a way as to reduce the concentration of the common ion. Buffers are characterized by their pH range and buffer capacity.
-
- 7.3: Acid-Base Titrations
- The shape of a titration curve, a plot of pH versus the amount of acid or base added, provides important information about what is occurring in solution during a titration. The shapes of titration curves for weak acids and bases depend dramatically on the identity of the compound. The equivalence point of an acid–base titration is the point at which exactly enough acid or base has been added to react completely with the other component.
-
- 7.4: Solving Titration Problems
- The shape of a titration curve, a plot of pH versus the amount of acid or base added, provides important information about what is occurring in solution during a titration. The shapes of titration curves for weak acids and bases depend dramatically on the identity of the compound. The equivalence point of an acid–base titration is the point at which exactly enough acid or base has been added to react completely with the other component.
-
- 7.5: Solubility Equilibria
- The solubility product (Ksp) is used to calculate equilibrium concentrations of the ions in solution, whereas the ion product (Q) describes concentrations that are not necessarily at equilibrium. The equilibrium constant for a dissolution reaction, called the solubility product (Ksp), is a measure of the solubility of a compound. Whereas solubility is usually expressed in terms of mass of solute per 100 mL of solvent, Ksp is defined in terms of the molar concentrations of the component ions.
-
- 7.E: Buffers, Titrations and Solubility Equilibria (Exercises)
- These are homework exercises for Chapter 17 “Additional Aspects of Aqueous Equilibria” of the Brown et al. Textmap, which addresses more complex equilibria with solutions containing more than one solute.
-
- 7.S: Buffers, Titrations and Solubility Equilibria (Study Guide)
- This is the summary for Chapter 17 “Additional Aspects of Aqueous Equilibria” of Brown et al. Textmap, which addresses more complex equilibria with solutions containing more than one solute.