it has been a while since ive done these so i just need a refresher. im looking for the heat of hydration of lithium chloride and sodium chloride.

compound Lattice Energy deltaH soln
LiCl -834 kj/mol -37.0 kj/mol
NaCl -769 kj/mol +3.88 kj/mol

what is delta H hydration?

See your post below

oh okay thanks!

Delta H hydration refers to the enthalpy change that occurs when one mole of a compound dissolves in water, leading to the formation of an aqueous solution. In this case, you are specifically interested in the heat of hydration for lithium chloride (LiCl) and sodium chloride (NaCl).

To calculate the delta H hydration, you need to subtract the lattice energy (delta H lattice) from the enthalpy change of solution (delta H soln). The equation to calculate delta H hydration is as follows:

Delta H hydration = Delta H soln - Delta H lattice

For lithium chloride (LiCl), the given values are:
Lattice Energy (Delta H lattice) = -834 kJ/mol
Enthalpy Change of Solution (Delta H soln) = -37.0 kJ/mol

Substituting these values into the equation:
Delta H hydration (LiCl) = -37.0 kJ/mol - (-834 kJ/mol)
= -37.0 kJ/mol + 834 kJ/mol
= 797 kJ/mol

Therefore, the heat of hydration for lithium chloride (LiCl) is 797 kJ/mol.

For sodium chloride (NaCl), the given values are:
Lattice Energy (Delta H lattice) = -769 kJ/mol
Enthalpy Change of Solution (Delta H soln) = +3.88 kJ/mol

Substituting these values into the equation:
Delta H hydration (NaCl) = +3.88 kJ/mol - (-769 kJ/mol)
= +3.88 kJ/mol + 769 kJ/mol
= 772.88 kJ/mol

Therefore, the heat of hydration for sodium chloride (NaCl) is 772.88 kJ/mol.

Please note that the heat of hydration is typically expressed in kilojoules per mole (kJ/mol).