I'm considering the following reaction:
$\ce{ZnSO4} + 2 \ce{KCl} \ce{->} \ce{ZnCl2} + \ce{K2SO4}$
The high solubility of $\ce{ZnCl2}$ would favour the $\ce{ZnSO4}$ & $\ce{KCl}$ direction of the reaction, but I'm wondering if I could turn this around by making the reaction occur in a flow of boiling hot water.
The idea would be to subject (initially dry) $\ce{ZnSO4}$ & $\ce{KCl}$ stationary phase to a flow of water in the 80-100°C range. The comparative solubility of $\ce{ZnCl2}$ at this temperature being high, I'm wondering if it being comparatively flushed away more than the other species could help drive the reaction forwards in the opposite direction?
I wouldn't get pure $\ce{ZnCl2}$ of course but I'd be happy if I could get a 90% $\ce{ZnCl2}$ solution from dry $\ce{ZnSO4}$ & $\ce{KCl}$.