Do carboxylic acids have permanent dipole to permanent dipole intermolecular bonds?

Sometimes folks fixate on hydrogen bonding, but remember that ALL molecules exhibit London dispersion forces. Carboxylic acids are asymmetrical and have a net dipole moment, and therefore exhibit dipole-dipole attraction, and then there is hydrogen bonding. All of these intermolecular forces contribute to the total van der Waals attraction. The same is true of alcohols. What you will notice in both acids and alcohols is that these are more noticeable for molecules with small numbers of carbon atoms (1-5).. In terms of intermolecular attractions, as the number of carbon atoms increases, the molecules behave more like nonpolar alkanes and less like polar acids or alcohols. This is why water solubility decreases as the carbon count increases.