0
$\begingroup$

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 $\ce{KI}$?

$\endgroup$
0
$\begingroup$

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.

$\endgroup$
2
  • $\begingroup$ 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

Your Answer

By clicking “Post Your Answer”, you agree to our terms of service, privacy policy and cookie policy

Not the answer you're looking for? Browse other questions tagged or ask your own question.