I was told that the more exothermic the solution, the more soluble the salt. Is this statement wrong? I was also told that $$\Delta H(\text{solution}) = \Delta H(\text{hydration}) - \Delta H(\text{lattice E})$$

However, for $\Delta H(\text{solution})$ to be exothermic, it has to have a negative value &lt;0. Which means lattice energy is going to have to be greater than $\Delta H(\text{solution})$ to produce a negative value, based on the equation above.

Yet I am also told that hydration energy released needs to be enough to compensate for the lattice energy required to break down the solid. So it can't be lesser than $\Delta H(\text{lattice E})$.

Isn't this contradictory? I am confused.

I have read a similar question at   Enthalpy of solution
but the answer given is that dissolving is dependent on Gibb's free energy instead.
Does that mean that I should disregard the statement "the more exothermic the solution, the more soluble the salt."?
Does that mean that I should disregard the statement "the more exothermic the solution, the more soluble the salt."? 


No, based on the Gibbs free energy equation $$\Delta G = \Delta H -T \Delta S$$ and the condition that $\Delta G&lt;0$ for spontaneous dissolution, if you assume $\Delta S$ is constant then the statement is true.

The point of that other post is that as a general rule you should not simply ignore the $\Delta S$ term since sometimes it is the decisive factor determining solubility (such as in the case of endothermic dissolution reaction).