Unit 8.4 - Acid-Base Reactions and Buffers - Part II

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10 Terms

1
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What is a weak acid that was mentioned in the lecture?
Acetic acid.
2
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What is the pH of a weak acid solution when titrated with a strong base at the start (zero base added)?
2.72.
3
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At what point in a titration does the pH equal the pKa?
At the halfway point, or half equivalence point.
4
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What equation can be used to calculate the pH of a buffer system?
The Henderson-Hasselbalch equation.
5
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In a titration involving acetic acid and KOH, which species is the limiting reactant at 50 mL of KOH added?
OH-.
6
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What is the outcome when equal amounts of weak acid and strong base react in a titration?
Both reactants are completely consumed, resulting in a conjugate base and water.
7
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What does a WOMEX problem signify in the context of acid-base reactions?
Water is a reactant and we use molarities in the ICE table.
8
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At the equivalence point, what is left in the solution after titration?
Only the conjugate base of the weak acid.
9
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What is indicated if the pH at the equivalence point is above 7?
The solution contains a weak acid and a strong base.
10
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How is the pOH calculated when you have excess strong base?
By finding the concentration of OH- and using pOH = -log[OH-].