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What are the steps of an acid-base titration?
1. Fill burette with titrant. 2. Measure analyte into flask. 3. Add indicator. 4. Slowly add titrant, swirling, until indicator changes color.
How do you determine the concentration of an unknown solution using titration?
React a known volume of the unknown solution (analyte) with a solution of known concentration (titrant) until the reaction reaches the equivalence point, then use stoichiometry to calculate the unknown concentration.
What is the process for identifying conjugate acid-base pairs?
1. Identify the pairs in the reaction. 2. The compound with the extra hydrogen is the acid; the other is the base.
What is the process of using the equation $M_aV_a = M_bV_b$?
1. Identify knowns. 2. Use the equation $M_aV_a = M_bV_b$. 3. Plug in and solve, remembering to convert volumes to liters and account for mole ratios.
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.
What is the effect of adding titrant to the analyte during titration?
The pH of the analyte changes as the titrant neutralizes it, eventually leading to the endpoint.
What happens if the endpoint is significantly different from the equivalence point?
The calculated concentration of the analyte will be inaccurate.
What is the effect of using an inappropriate indicator for a titration?
The endpoint will not accurately reflect the equivalence point, leading to inaccurate results.
What happens if the mole ratio of acid to base is not 1:1 in a titration reaction?
The $M_aV_a = M_bV_b$ equation must be adjusted to account for the mole ratio to calculate the correct concentration.
What happens when a strong acid donates a proton?
It forms its conjugate base, which has a weaker affinity for protons.