Revise later
SpaceTo flip
If confident
All Flashcards
Define 'Titrant'.
Solution with a known concentration, usually in the burette.
Define 'Analyte'.
Solution with an unknown concentration, usually in the Erlenmeyer flask.
Define 'Equivalence Point'.
The point where moles of titrant = moles of analyte; reaction is complete.
Define 'Endpoint'.
The point where the indicator changes color, ideally close to the equivalence point.
Define 'Titration Curve'.
Graph showing pH change of the analyte as titrant is added.
Define 'Acid (Bronsted-Lowry)'.
A proton (H⁺) donor.
Define 'Base (Bronsted-Lowry)'.
A proton (H⁺) acceptor.
Define 'Conjugate Base'.
The species remaining after an acid has donated a proton.
Define 'Conjugate Acid'.
The species formed when a base accepts a proton.
Define 'Amphiprotic'.
A substance that can act as both an acid and a base.
Label the main components of a titration setup.
1: Burette (Titrant), 2: Erlenmeyer Flask (Analyte), 3: Indicator
What is the difference between the 'Equivalence Point' and the 'Endpoint' in a titration?
Equivalence Point: Moles of acid equals moles of base (theoretical). Endpoint: Indicator changes color (experimental).
What are the key differences between a strong acid/strong base titration curve and a weak acid/strong base titration curve?
Strong Acid/Strong Base: No buffer region, sharp equivalence point. Weak Acid/Strong Base: Buffer region present, equivalence point at pH > 7.
Compare and contrast an acid and its conjugate base.
Acid: Proton donor. Conjugate Base: What remains after the acid donates a proton. Differ by one proton.