<Table> Conjugate acids of bases <Tr> <Th> Compound </Th> <Th> Equilibrium </Th> <Th> pK </Th> <Th> ΔH (kJ mol) </Th> <Th> − TΔS (kJ mol) </Th> </Tr> <Tr> <Td> B = Ammonia </Td> <Td> HB ⇌ B + H </Td> <Td> 9.245 </Td> <Td> 51.95 </Td> <Td> 0.8205 </Td> </Tr> <Tr> <Td> B = Methylamine </Td> <Td> HB ⇌ B + H </Td> <Td> 10.645 </Td> <Td> 55.34 </Td> <Td> 5.422 </Td> </Tr> <Tr> <Td> B = Triethylamine </Td> <Td> HB ⇌ B + H </Td> <Td> 10.72 </Td> <Td> 43.13 </Td> <Td> 18.06 </Td> </Tr> </Table> <Tr> <Th> Compound </Th> <Th> Equilibrium </Th> <Th> pK </Th> <Th> ΔH (kJ mol) </Th> <Th> − TΔS (kJ mol) </Th> </Tr> <Tr> <Td> B = Ammonia </Td> <Td> HB ⇌ B + H </Td> <Td> 9.245 </Td> <Td> 51.95 </Td> <Td> 0.8205 </Td> </Tr> <Tr> <Td> B = Methylamine </Td> <Td> HB ⇌ B + H </Td> <Td> 10.645 </Td> <Td> 55.34 </Td> <Td> 5.422 </Td> </Tr>

Determination of the dissociation constant of weak acids