= Equivalence point
{title2=$V_{\mathrm{eq}}$}
{wiki}
The <equivalence point> is the composition at which added <titrant> and the initial sample inventory match the specified <chemical reaction>'s <stoichiometry>. It is a theoretical inventory condition; the <titration endpoint> is an observed stopping criterion. For a <monoprotic acid> consuming one <hydroxide> per acid unit, initial acid <molar concentration> $c_A$, sample <volume (thermodynamics)> $V_A$, and base <titrant> <molar concentration> $c_B$ give
$$
n_A=c_AV_A=c_BV_{\mathrm{eq}},\qquad V_{\mathrm{eq}}=\frac{c_AV_A}{c_B}.
$$
The proof is <amount of substance> conservation with one-to-one <neutralization>; a different <stoichiometry> requires its coefficients. All <volumes> must use compatible units. Since $1\,\mathrm{mL}=10^{-3}\,\mathrm L$, $0.100\,\mathrm{mol\,L^{-1}}\times10.00\,\mathrm{mL}=0.001000\,\mathrm{mol}$, not $1\,\mathrm{mol}$.
An <equivalence point> does not prescribe <pH> $7$. A <weak acid> titrated with a <strong base> leaves its <conjugate base>, which reacts with <water>; the corresponding <chemical equilibrium> can make the <chemical solution> alkaline. The neutral <strong acid>/<strong base> case additionally depends on <temperature>, through <self-ionization of water>.<Chemistry 2e by Paul Flowers and others/14.7 Acid-Base Titrations>[Chemistry 2e, §14.7, Example 14.21(c), Example 14.22(b), and Figure 14.18: different equivalence-point pH values]{ref}
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