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The licl boiling point is the temperature at which LiCl becomes liquid. This is the highest possible temperature that a solution can reach under a given pressure. It is determined by the dipole-dipole forces between ions. These forces are dependent on the charge of the cation or anion and their ionic radius. In the case of LiCl, the cation is alkali metal and its ionic radius is small. Hence the dipole-dipole force is strong. This makes the ionic bonds stronger and harder to break. This can explain why LiCl has a higher boiling point than HCl. But it doesn’t explain why HF has a lower boiling point than H2O. The melting and boiling points of a chemical increase as they go down the group because the molecules get larger, which means more electrons are available to form temporary dipoles. These dipoles create more attraction and therefore require more energy to break their bonds, which increases the energy required to melt or boil a liquid. Similarly, the thermal conductivity of a liquid solution also increases as the molecules get larger. The increase in the thermal conductivity is also caused by the formation of temporary dipoles, which causes more electrons to move between the molecules and therefore requires more energy to conduct heat. The enthalpy change of a liquid is also related to the dilution of the solvent from r1 to r2. It depends on the mass fraction of the solvent, the dilution enthalpy and other required parameters.