In AP Chemistry, the titrant is the solution of known concentration that you add (usually from a buret) during a titration; it reacts specifically and quantitatively with the analyte, so the volume of titrant needed to reach the equivalence point lets you calculate the analyte's unknown concentration.
The titrant is the solution you already know everything about. You know its concentration, and you know exactly how it reacts with the substance you're testing. During a titration, you slowly drip titrant from a buret into a flask containing the analyte, the solution whose concentration you're trying to find.
The whole technique works because the titrant reacts specifically and quantitatively with the analyte (that's the CED's exact language in Topic 4.6). "Quantitatively" means the reaction goes essentially to completion with no side reactions, so every mole of titrant you add consumes a predictable amount of analyte. When the analyte is totally used up, you've hit the equivalence point. Since you tracked the volume of titrant delivered and you know its molarity, you can calculate moles of titrant, use the balanced equation's mole ratio, and back out the analyte's concentration. The titrant is the measuring stick; the analyte is the mystery.
Titrant shows up in two places in the CED. In Topic 4.6 (Introduction to Titration), learning objective 4.6.A asks you to identify the equivalence point based on the amounts of titrant and analyte, assuming the reaction goes to completion. In Topic 8.5 (Acid-Base Titrations), learning objective 8.5.A has you explain titration results, and the CED specifically defines a titration curve as a plot of pH versus volume of titrant added. That x-axis label matters. Every titration curve question is really asking what happens chemically as more titrant pours in.
The key stoichiometric fact (essential knowledge 8.5.A.2) is that at the equivalence point of a monoprotic titration, moles of titrant added equal moles of analyte originally present. That single relationship powers most titration math on the exam, and it works the same whether the acid or base is strong or weak.
Keep studying AP Chemistry Unit 8
Burette (Unit 4)
The buret is the titrant's delivery device. It dispenses titrant drop by drop and measures the exact volume added, which is the number you plug into M × V to get moles of titrant. No precise volume, no usable titration.
End Point and Acid-Base Indicators (Units 4 & 8)
The equivalence point is the invisible chemical moment when the titrant has exactly consumed the analyte. The endpoint is the visible signal, like an indicator changing color, that tells you to stop adding titrant. A good indicator makes the endpoint land as close to the equivalence point as possible, but they're not guaranteed to be identical.
Molarity and Solution Stoichiometry (Unit 4)
Titration math is just solution stoichiometry in lab form. Moles of titrant equals molarity times volume, then the balanced equation's mole ratio converts that to moles of analyte. A titrant only works as a measuring tool because its molarity is known precisely.
Titration Curves and Buffers (Unit 8)
Plot pH against volume of titrant added and you get a titration curve. For a weak acid titrated with a strong-base titrant, the region before equivalence is a buffer, and the half-equivalence point (where pH = pKa) happens when you've added exactly half the titrant needed to reach equivalence.
Multiple-choice questions love the steep part of the titration curve. A classic stem gives you 25.0 mL of 0.100 M HCl titrated with 0.100 M NaOH and asks where pH changes most dramatically per drop of titrant (answer: right at the equivalence point). Other MCQs test whether you can explain why the endpoint and equivalence point might occur at slightly different titrant volumes, or what determines the equivalence point in the first place (stoichiometry, not the indicator).
On FRQs, titrants aren't limited to acids and bases. The 2017 short FRQ asked students to choose between two redox titrants (dichromate vs. cobalt(II) ion) for finding H₂O₂ concentration, and the 2019 short FRQ used dark purple KMnO₄ as a self-indicating titrant for oxalic acid. Expect to do the full calculation chain (titrant volume → moles of titrant → mole ratio → analyte concentration), justify titrant choice, or explain what the persistent color of excess titrant tells you about reaching the endpoint.
These are the two players in every titration, and mixing them up wrecks your setup. The titrant is the known solution you add from the buret. The analyte is the unknown solution sitting in the flask, the thing you're actually trying to measure. A quick memory hook: you ANALyze the ANALyte using the titrant. On a titration curve, the x-axis is always volume of titrant added, never analyte.
The titrant is the solution of known concentration added from a buret, and it reacts specifically and quantitatively with the analyte.
At the equivalence point of a monoprotic titration, moles of titrant added equal moles of analyte originally present, which is the relationship you use to solve for the unknown concentration.
A titration curve plots pH on the y-axis against volume of titrant added on the x-axis, with the steepest jump occurring at the equivalence point.
The endpoint (the observable signal, like a color change) and the equivalence point (the exact stoichiometric moment) are close but not necessarily identical volumes of titrant.
Titrants aren't always acids or bases; released FRQs have used redox titrants like KMnO₄ and dichromate ion to find concentrations of species like H₂O₂ and oxalic acid.
The titrant is the solution with a precisely known concentration that you add from a buret during a titration. It reacts completely and predictably with the analyte, so the volume of titrant used lets you calculate the analyte's unknown concentration.
No. The titrant is the known solution in the buret, and the analyte is the unknown solution in the flask that you're trying to measure. The CED defines the equivalence point as the moment the titrant has totally consumed the analyte.
No. While Topic 8.5 focuses on acid-base titrations, redox titrants appear on the exam too. The 2019 FRQ used KMnO₄ to titrate oxalic acid, and the 2017 FRQ asked students to compare dichromate and cobalt(II) ions as titrants for H₂O₂.
Multiply the titrant's molarity by the volume delivered to get moles of titrant, then use the balanced equation's mole ratio to find moles of analyte, and finally divide by the analyte's original volume. For a 1:1 monoprotic titration, moles of titrant at equivalence equal moles of analyte exactly.
The equivalence point is the exact stoichiometric moment, but the endpoint is just the observable signal, usually an indicator's color change. If the indicator changes color at a pH slightly above or below the equivalence-point pH, you'll see the endpoint a few drops of titrant early or late.