Write an equation to represent the enthalpy change of solution of zinc chloride.

The enthalpies of solution of some metal halides are given below. What do these values tell you about the relative solubilities of these four compounds?
sodium chloride, $∆{\mathrm{H}}_{\mathrm{sol}}^{⊝} =+3.9 \mathrm{kJ} {\mathrm{mol}}^{-1}$
silver chloride, $∆{\mathrm{H}}_{\mathrm{sol}}^{⊝} =+65.7 \mathrm{kJ} {\mathrm{mol}}^{-1}$
sodium bromide, $∆{\mathrm{H}}_{\mathrm{sol}}^{⊝} =-0.6 \mathrm{kJ} {\mathrm{mol}}^{-1}$
silver bromide, $∆{\mathrm{H}}_{\mathrm{sol}}^{⊝} =+84.5 \mathrm{kJ} {\mathrm{mol}}^{-1}$

Why is the enthalpy change of hydration always exothermic?

Write equation to represent the hydration of a sodium ion.

Write equation to represent the hydration of a chloride ion.

Draw diagram to show four water molecules hydrating a magnesium ion. Show the dipole on each water molecule.

Draw diagram to show two water molecules hydrating a bromide ion. Show the dipole on each water molecule.

Explain why the value of $∆{\mathrm{H}}_{\mathrm{hyd}}^{⊝}$ for magnesium ions is much more exothermic than $∆{\mathrm{H}}_{\mathrm{hyd}}^{⊝}$ for potassium ions.

Name the change associated with the equation below:

$\mathrm{KBr}\left(\mathrm{s}\right) + \mathrm{aq} \to \mathrm{KBr}\left(\mathrm{aq}\right)$ (for $1 \mathrm{mole}$ of $\mathrm{KBr}$)