standardization
/ stan-der-dy-ZAY-shun /
Imagine buying a tape measure with no markings and first checking it against a ruler you trust, so you know exactly how long each section really is. Standardization does the same for a solution: before relying on it, you measure its true concentration against something dependable.
Technically, standardization is the procedure of finding the exact concentration of a titrant by reacting it with a precisely weighed primary standard — a very pure, stable substance whose amount is known to high accuracy. The measured volume of titrant needed reveals its real concentration.
It matters because many useful titrants (like sodium hydroxide or hydrochloric acid solutions) cannot be made up accurately just by weighing, since they absorb water, gas, or impurities. Standardizing them pins down the true value; skipping it means trusting a number that may be quietly wrong.
A roughly made sodium hydroxide solution is standardized by titrating it against weighed potassium hydrogen phthalate, a primary standard; the result might show its true concentration is 0.1023 mol/L rather than the intended 0.1000.
Pin down a titrant's real concentration against a trusted primary standard.
A solution standardized against a primary standard becomes a secondary standard. Concentrations from standardization drift over time, so titrants are usually re-standardized periodically rather than trusted indefinitely.