Typically, you get what are called Integral tables for heat of dilution. Such a table (as the one linked above) lists enthalpy changes (relative to infinite dilution, where h = 0) as a function of molality. So the heat of dilution to go from molality M1 to molality M2 is simply the difference between two values in the table, namely h(M1) - h(M2) and it would have units of say, kJ.ritunesh said:I want to know what's difference between heat of mixing and differential heat of dilution. I am working on calcium chloride solution. I need to know also from where i can get heat of mixing of calcium chloride solution.
Thanking you
The heat of mixing, also known as the enthalpy of mixing, is the amount of heat released or absorbed when two or more substances are mixed together. It is a measure of the energy changes that occur when the molecules of different substances interact with each other.
The heat of mixing can be calculated using the following formula: ΔHmix = ΣniΔHi, where ΔHmix is the heat of mixing, ni is the number of moles of each component, and ΔHi is the enthalpy of each component.
The heat of mixing is affected by the types of molecules being mixed, their concentrations, and the temperature at which the mixing occurs. It can also be influenced by intermolecular forces, such as hydrogen bonding, between the molecules.
The differential enthalpy of dilution is a measure of the change in enthalpy when a solute is added to a solvent to create a solution. It is the difference between the enthalpy of the solution and the enthalpy of the pure components at the same temperature and pressure.
The differential enthalpy of dilution is related to the heat of mixing because it is a measure of the energy changes that occur when a solute is mixed with a solvent. In other words, it is a specific type of heat of mixing that only applies to solutions and takes into account the enthalpy changes of the pure components.