= Solution
Two neutral <carboxylic acids> can form a <carboxylic acid dimer> with \b[two reciprocal O–H···O=C <hydrogen bonds>]. In water, each acid group already makes favourable solvent contacts. Association must displace some of those contacts and loses translational freedom, so the extra stabilization of the dimer may be small. Any ionized carboxylate population also cannot form the same neutral two-donor <carboxylic acid dimer>.
A nonpolar, weakly hydrogen-bond-accepting solvent such as dry <toluene> or a compatible hydrocarbon generally favours this dimerization relative to water, provided the acid dissolves. The solvent competes less strongly for the donor and acceptor sites. Dilution still disfavors the dimer because $K=[(\mathrm{HA})_2]/[\mathrm{HA}]^2$: the dimer fraction depends on concentration even in a favourable solvent. Thus trace dimer in the aqueous sample is not evidence that the acid lacks hydrogen-bonding ability.
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