Titration
High School
Definition
A laboratory technique for finding an unknown concentration by reacting a solution with a measured volume of another solution of known concentration. An indicator or pH meter signals the endpoint, when the reactants have combined in exact proportions.
Worked examples
\(25.0\,\)mL NaOH\( + 18.3\,\)mL\(\) of \(0.100\,\)M HCl\(\) reaches endpoint
The measured volume of acid neutralizes the base; we can now calculate the unknown NaOH concentration.
Phenolphthalein turns from pink to colorless at pH 8.2
The indicator color change signals the endpoint when the acid has exactly neutralized the base.
Common mistakes
- recording the final burette reading as the titrant volume → subtracting initial from final burette reading to get volume delivered The volume used is the difference, not the final mark on the burette.
- assuming endpoint and equivalence point are always identical → endpoint is when indicator changes; equivalence point is the exact stoichiometric moment A good indicator changes color very close to, but not exactly at, the equivalence point.
- using any indicator for any titration → choosing an indicator whose color change matches the pH at equivalence Strong acid–strong base needs a different indicator than weak acid–strong base titrations.
Where you'll use it next
Titration is essential for quantitative analysis in chemistry labs, calculating molarity and reaction stoichiometry, and prepares you for analytical chemistry, biochemistry, and real-world quality control in pharmaceuticals and environmental testing.
Found in 1 StudyPug lesson
Acid-Base Titration: Mastering the Math Behind Chemistry
10th Grade10thGCSE Chemistry
Dive into the world of acid-base titration math! Learn to calculate concentrations, find equivalence points, and apply your skills to real-world scenarios. Our expert guidance makes complex concepts clear.
See also
Reviewed by Pat Cheng, M.Ed. — StudyPug Curriculum Lead · Last updated June 6, 2026