Results are reported for measurements leading to the calculation of standard thermodynamic properties for temperatures from T = 250 K to T = 560 K for the methylpyridines (Chemical Abstracts registry numbers: 4-methylpyridine, 108-89-4; 2-methylpyridine, 109-06-8; 3-methylpyridine, 108-99-6). The standard state is defined as the ideal gas at the pressure p = p(O) = 101.325 kPa. Vapor pressures were measured by comparative ebulliometry for the pressure range p approximate to 4 kPa to p = 270 kPa. Two-phase (liquid + vapor) heat capacities were measured for the temperature range approximate to 310 (T/K) approximate to 590 with a differential scanning calorimeter (d.s.c.), and saturation heat capacities C-sat were derived. The critical temperature T, was determined experimentally by d.s.c., and the critical pressure and critical density were derived. Densities for the liquid phase of 3-methylpyridine at saturation pressure were measured with a vibrating-tube densimeter for the temperatures 323 (T/K) < 473. The enthalpy of combustion for 3-methylpyridine was determined to resolve a discrepancy in the literature. Enthalpies of vaporization were calculated for all compounds. Literature values for enthalpy increments and entropies for the condensed phases by adiabatic heat-capacity calorimetry and the energies of combustion were combined with the present results to derive standard entropies, enthalpy increments, and molar Gibbs free energies of formation for temperatures between T = 250 K and T = 560 K. Comparisons with standard entropies calculated statistically provide corroboration for the calorimetrically derived values and are used to demonstrate thermodynamic consistency for properties related through identities and correlations. Isomerization distributions derived with standard molar Gibbs free energies of formation are used to aid interpretation of literature fossil fuel characterization and pyridine methylation catalysis studies.