Enthalpy OF neutralization,lattice enthalpy & its calculation

Order of lattice enthalpy is as

Calorific Value || Enthalpy of Neutralization || Enthalpy of Fusion, Vaporization,Sublimation,Transition,Enthalpy of Hydration

Enthalpy OF Neutrilisation and Its Calculation || Lattice Enthalpy & Born Haber Cycle

Enthalpy OF Hydrogenation || Enthalpy OF Isomerization || Enthalpy OF Neutralization - Case I :- SASB (Strong Acid Strong Base)

Introduction || Enthalpy of Reaction || Enthalpy of Formation || Calculation of Enthalpy of Reaction from Enthalpies of Formation || Hess’s Law || Enthalpy of Combustion

The solubility of a crystalline compound in water is influenced by two factors. These are lattice enthalpy and hydration enthalpy. Lattice enthalpy is needed to separate the ions from the crystal lattice. At the same time hydration enthalpy is released when the ion are dissolved in water. The resultant of these two opposing tendencies guides the solubility of the compound in water. If lattice enthalpy has a greater magnitude, the compound has low solubility. In case hydration enthalpy is more, then the compound is highly soluble in water. The hydroxide which is maximum soluble in water is :

The solubility of a crystalline compound in water is influenced by two factors. These are lattice enthalpy and hydration enthalpy. Lattice enthalpy is needed to separate the ions from the crystal lattice. At the same time hydration enthalpy is released when the ion are dissolved in water. The resultant of these two opposing tendencies guides the solubility of the compound in water. If lattice enthalpy has a greater magnitude, the compound has low solubility. In case hydration enthalpy is more, then the compound is highly soluble in water. A metal M readily forms a water soluble sulphate MSO_(4) water insoluble hydroxide M(OH)_(2) and oxide MO which becomes inert upon heating. The hydroxide is soluble in NaOH. The metal M is

The solubility of a crystalline compound in water is influenced by two factors. These are lattice enthalpy and hydration enthalpy. Lattice enthalpy is needed to separate the ions from the crystal lattice. At the same time hydration enthalpy is released when the ion are dissolved in water. The resultant of these two opposing tendencies guides the solubility of the compound in water. If lattice enthalpy has a greater magnitude, the compound has low solubility. In case hydration enthalpy is more, then the compound is highly soluble in water. A chemical compound 'A' is used for water softening to remove temporary hardness 'A' reacts with Na_(2)CO_(3) to form caustic soda. When CO_(2) is bubbled through 'A' it becomes cloudy. The chemical formula of 'A' is :

Among the alkali metal halides, lattice enthalpy is maximum for LiF and least for CsI.

Enthalpy OF reaction, enthalpy OF formation, enthalpy OF combustion