[rg16]

Hi! For an experimental investigation I'm doing, I need to find the literature enthalpies of solution of CuCl₂ and Cu(NO₃)₂. I've found literature values for all the other compounds I'm testing except for these copper compounds. I am trying to figure out if I can determine these through Hess's Law, but I'm really confused on what reactions to use and add up.

So far, I just have the reactions written out:
CuCl₂ (s) --> CuCl₂ (aq), and then the same with the nitrate compound.
I've tried using things like: CuO + 2HCl --> CuCl₂ (aq) + H₂O, but it doesn't seem to work when I add these reaction equations. Any guidance on which reaction equations to use or any alternative ways to find heat of solution non-experimentally would be appreciated!
Thanks!

[mjc123]

Try looking up enthalpies of formation of the compounds. You should be able to find it for e.g. CuCl₂(s); maybe not for CuCl₂(aq), but you should find values for Cu²⁺(aq) and Cl^-(aq).

[rg16]

Thanks for replying! So I found the enthalpies of formation for CuCl₂ (s) and both the aqueous ions. Now, I just do the sum of products (the aqueous ions) - the sum of reactants/the solid, (multiplying the enthalpy of Cl- by 2) correct? Also, for copper (II) nitrate, I wasn't able to find a heat of formation for it in the solid state in any sort of database; I was only able to find the enthalpy in problems about its decomposition reaction in worksheets posted online from college courses. Would you happen to know of any more reliable place/way I can find that enthalpy of formation? Again, thank you!

[mjc123]

Try this: https://www.update.uu.se/~jolkkonen/pdf/CRC_TD.pdf. I found it googling "copper nitrate enthalpy of formation".

[CelticKhemist2000]

How can you have CuCl2 in solid and aqueous form?