<Tr> <Td> Naphthalene </Td> <Td> 217.9 </Td> <Td> 5.8 </Td> </Tr> <Tr> <Td> Phenol </Td> <Td> 181.75 </Td> <Td> 3.04 </Td> </Tr> <Tr> <Td> Water </Td> <Td> 100 </Td> <Td> 0.512 </Td> </Tr> <P> Together with the formula above, the boiling - point elevation can in principle be used to measure the degree of dissociation or the molar mass of the solute . This kind of measurement is called ebullioscopy (Greek "boiling - viewing"). However, since superheating is difficult to avoid, precise ΔT measurements are difficult to carry out, which was partly overcome by the invention of the Beckmann thermometer . Furthermore, the cryoscopic constant that determines freezing - point depression is larger than the ebullioscopic constant, and since the freezing point is often easier to measure with precision, it is more common to use cryoscopy . </P>

The value of the boiling-point-elevation constant (kb) depends on the identity of the solvent