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💧AP CHEMISTRY STUDY GUIDE
Unit 8: Acids and Bases
Review acid-base models, pH, strong and weak species, buffers, titrations, and molecular structure for AP Chemistry Unit 8.
8 key ideas8 flashcards5 practice questions
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pH equals pKa for a weak acid
stoichiometric amounts have reacted
Key ideas to know
Start with the relationships between ideas. Then close the notes and explain each one from memory.
- 01
A Brønsted-Lowry acid donates a proton, while a Brønsted-Lowry base accepts a proton.
- 02
Conjugate acid-base pairs differ by one proton.
- 03
Strong acids and bases ionize nearly completely in dilute aqueous solution.
- 04
Weak acids and bases establish equilibria with water.
- 05
pH is the negative base-ten logarithm of hydrogen ion activity, often approximated with concentration in course calculations.
- 06
The acid and base ionization constants quantify weak-species equilibria.
- 07
A buffer contains a weak acid-base pair that consumes added acid or base.
- 08
A titration curve connects solution pH with added titrant volume.
PART OF THE AP CHEMISTRY GUIDE
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Open the full AP Chemistry guide →Two ideas worth correcting now
NOT QUITE
→A strong acid is always highly concentrated
USE THIS INSTEAD
Strength describes extent of ionization, while concentration describes amount per volume.
NOT QUITE
→A buffer keeps pH perfectly fixed
USE THIS INSTEAD
A buffer limits a pH shift but has finite capacity.
Flashcards
Answer before opening each card. The effort to retrieve is part of the learning.
1What is a Brønsted-Lowry acid?Show answer ＋
A proton donor.
2What is a Brønsted-Lowry base?Show answer ＋
A proton acceptor.
3How are a conjugate acid and base related?Show answer ＋
They differ by one proton.
4What is pH?Show answer ＋
The negative base-ten logarithm of hydrogen ion activity, often approximated by concentration.
5What does a larger Ka indicate?Show answer ＋
A greater extent of acid ionization in water.
6What makes a buffer?Show answer ＋
Appreciable amounts of a weak acid and its conjugate base, or a weak base and its conjugate acid.
7At the half-equivalence point of a weak-acid titration, how are pH and pKa related?Show answer ＋
They are equal under the standard approximation because acid and conjugate-base concentrations are equal.
8What is amphiprotic behavior?Show answer ＋
Ability to donate or accept a proton.
Explain it in your own words
Use the answer as a check after you have written or spoken your response.
01Why does diluting a strong acid raise its pH?
Dilution lowers the hydrogen ion concentration even though the acid remains nearly fully ionized.
02How does a buffer respond to added strong acid?
Its weak-base member consumes much of the added proton, limiting the pH shift.
03Why is the equivalence-point pH above seven in a weak-acid, strong-base titration?
The conjugate base formed at equivalence reacts with water to produce hydroxide ions.
04How can molecular structure affect acid strength?
Bond polarity, bond strength, atom size, and stabilization of the conjugate base affect proton donation.
05Why is an indicator endpoint only an estimate of equivalence?
The indicator shifts color across a pH interval, while equivalence is defined by stoichiometry.
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