Why does the solubility of a solute (like table salt) increase with increasing temperature of the solution?

Dissolution of a salt in water is a bond breaking reaction. For salts, this involves the breaking of strong ionic bonds between the counterions and the formation of aquated ions, which we represent as $N {a}^{+} \left(a q\right)$, i.e. $N a {\left(O {H}_{2}\right)}_{6}^{+}$, for example. Since this is a bond-breaking reaction, dissolution of ionic salts should indeed be enhanced at higher temperatures, in that the higher temperatures allow disruption of ion-ion bonds. Likewise, dissolution of non-ionic solutes should be greater at higher temperature, as solute-solute interactions still have to be overcome.