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Neutralisation reaches its end point when the moles of donated protons equal the moles of hydroxide supplied. Moles of acid come from concentration times volume, multiplied by the protons each molecule can donate, so a diprotic acid needs twice the base a monoprotic one does at the same concentration. 25 mL of 0.1 M monoprotic acid needs 20 mL of 0.125 M base.
Proton balance
C(acid) x V(acid) x protons = C(base) x V(base)
Base volume
V(base) = moles of H+ / C(base)
Only for a strong acid with a strong base. A weak acid neutralised by a strong base reaches equivalence above pH 7 because the conjugate base hydrolyses.
Sulfuric acid donates two protons per molecule, so 0.1 M sulfuric acid neutralises twice as much base as 0.1 M hydrochloric acid.