2.4: 4. AB2- Quantitative Properties of Acid/Base Systems
- Page ID
- 436099
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Summary of AB1 and AB2:
Acid and base chemistry has so many applications and so many essential properties throughout chemistry that it is broken down into two Core Goals:
AB1: Equilibrium Acids and Bases - focused on the qualitative nature of acid/base chemistry and the equilibrium between them.
AB2: Quantitative understanding of the various properties of complex acid/base systems.
AB2: Quantitative Properties of Acid/Base Systems
- Recall how to use Ka, pKa, Kb, or pKb, to predict the extent of an acid-base reaction and the value of the equilibrium constant for a reaction such as the mixture of a weak acid with a weak base.
- Perform quantitative calculations related to water solutions of acids, bases, and salts (Ka, pKa, Kb, pKb, [H+], pH, [OH-], pOH, and % ionization) including polyprotic acids, mixtures of weak acids or bases, and very dilute solutions of acids or bases
- In terms of Le Chatelier’s Principle, explain why the addition of a salt containing the conjugate base of a weak acid, or the conjugate acid of a weak base, suppresses the ionization of the acid or base respectively.
- Distinguish between a solution that is buffered and one that is not in terms of composition and response to addition of small quantities of a strong acid or strong base
- Describe two distinctly different methods of preparing a buffered solution and the decisions one must make in preparing a buffered solution.
- Define and apply the following concepts to buffered solutions: buffer capacity, buffer range, acidic buffer, and basic buffer
- From a molecular perspective, use chemical reaction equations to describe what happens when small quantities of a strong acid or strong base is added to a buffered solution
- Calculate the initial pH of a buffered solution and the pH after addition of a strong acid or base
- Compare and contrast acid-base titrations:
- strong acid-strong base
- weak acid-strong base
- weak base-strong acid
- polyprotic acids with strong base
- Explain why the pH at the equivalence point in an acid-base titration is not always 7 even though the acid has been completely neutralized
- Interpret titration curves:
- initial pH
- equivalence point
- end-point
- buffered region and
- pKa values
- Calculate the pH at any point in an acid-base titration, especially:
- initially
- at 50% of the equivalence point (the midpoint)
- near the midpoint point
- at the equivalence point and
- much beyond the equivalence point
- Explain the role of acid-base indicators in a titration, how they work, their limitations, and the factors that one must consider in the selection of an appropriate indicator for a titration