If the dissolving of #NH_4Cl# [aq] is an endothermic process, how does the decrease/increase in temperature affect its solubility?

1 Answer
anor277
May 16, 2018

Well, consider the equilibrium....

Explanation:

#NH_4Cl(s) +DeltarightleftharpoonsNH_4^+ + Cl^(-)#

This is a bond breaking process, and so reasonably we would expect that an increase in temperature should bring MORE of the salt into solution, i.e. to drive the equilibrium to the right as we face the page.

This page displays some data, and as chemists, as physical scientists, our argument should also address the data, and at higher temperatures ammonium chloride increases its aqueous solubility.

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