Chemistry: Acids & Bases Flashcards
7 cards from real AP practice questions. Tap to flip, then mark Knew It or Still Learning — missed cards come back until you master them.
Read the first 7 Chemistry: Acids & Bases flashcards as text
A buffer solution is typically made from:
Answer: A weak acid and its conjugate base
Buffers consist of a weak acid and its conjugate base (or weak base and conjugate acid).
Using the Henderson-Hasselbalch equation, the pH of a buffer equals pKa when:
Answer: [A-] = [HA]
When [A-] = [HA], the log term is zero, so pH = pKa.
How many moles of NaOH are needed to neutralize 0.5 mol of H2SO4 completely?
Answer: 1.0 mol
H2SO4 has two acidic protons, so 0.5 mol requires 1.0 mol NaOH.
The titration curve of a weak acid with a strong base has an equivalence point pH that is:
Answer: Greater than 7
The conjugate base formed makes the equivalence-point solution basic, so pH > 7.
What volume of 0.10 M HCl is required to neutralize 25.0 mL of 0.10 M NaOH?
Answer: 25.0 mL
Equal concentrations and a 1:1 ratio require equal volumes, so 25.0 mL.
Adding a small amount of strong acid to a buffer causes the buffer to:
Answer: Resist large pH change
The conjugate base neutralizes added acid, so the pH changes only slightly.
The percent ionization of a weak acid increases as the solution becomes:
Answer: More dilute
Dilution shifts the dissociation equilibrium toward more ionization.