For example if I have a table with these data data

How can those data be compared with each other to find heat of solution of $\ce{KI}$?


The enthalpy of solution is equal to the difference in the enthalpy of hydration minus the lattice energy of the material.

Enthalpy of solution = Enthalpy of hydration− Lattice energy.

Maybe you should look up the KI hydration energy value somewhere, like the NIST website.

  • $\begingroup$ But I need to use the table only. I guess, enthalpy of hydration can't be calculated from this table. $\endgroup$
    – Abrar
    Jul 28 at 15:42
  • $\begingroup$ Here is an idea. Replacing $\ce{Na}$ by $\ce{K}$ should be the same in chloride and in iodide. So, in chloride, this change in the heat of solution is accompanied by an increase of $13.2$ kJ/mol. In iodides, the heat of solution of KI maybe obtained by the same change, and this gives $-5.1 + 13.2 = + 8.1$ kJ/mol. I am not sure of the validity of my reasoning, because it does not take into account the lattice energy. I would be happy to know more. $\endgroup$
    – Maurice
    Aug 27 at 16:42

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