Which equation represents an acid–base reaction according to the Lewis theory but not the Bronsted–Lowry theory?

The equilibrium reached when ethanoic acid is added to water can be represented by the following equation:

${\mathrm{CH}}_3\mathrm{COOH}\left(\mathrm{l}\right)+{\mathrm{H}}_2\mathrm{O}\left(1\right)\rightleftharpoons {\mathrm{CH}}_3{\mathrm{COO}}^{-}\left(\mathrm{aq}\right)+{\mathrm{H}}_3{\mathrm{O}}^{+}\left(\mathrm{aq}\right)$

Define the terms Brønsted–Lowry acid and Lewis base, and identify two examples of each of these species in the equation.

Deduce the two acids and their conjugate bases in the following reaction:

${\mathrm{H}}_2\mathrm{O}\left(\mathrm{l}\right)+{\mathrm{NH}}_3\left(\mathrm{aq}\right)\rightleftharpoons {\mathrm{OH}}^{-}\left(\mathrm{aq}\right)+{\mathrm{NH}}_4^{+}\left(\mathrm{aq}\right)$

Explain why the following reaction can also be described as an acid–base reaction.

${\mathrm{F}}^{-}\left(\mathrm{g}\right)+{\mathrm{BF}}_3\left(\mathrm{g}\right)\rightleftharpoons {\mathrm{BF}}_4^{-}\left(\mathrm{s}\right)$

When these $1.0 \mathrm{mol} {\mathrm{dm}}^3$ acidic solutions are arranged in order of increasing strength (weakest first), what is the correct order?

Acid in solution X : ${\mathrm{K}}_{\mathrm{a}}=1.74\times {10}^{-5} \mathrm{mol} {\mathrm{dm}}^{-3} \mathrm{at} 298 \mathrm{K}$ 

Acid in solution Y : ${\mathrm{K}}_{\mathrm{a}}=1.38\times {10}^{-3} \mathrm{mol} {\mathrm{dm}}^{-3} \mathrm{at} 298 \mathrm{K}$ 

Acid in solution Z : ${\mathrm{K}}_{\mathrm{a}}=1.78\times {10}^{-5} \mathrm{mol} {\mathrm{dm}}^{-3} \mathrm{at} 298\mathrm{K}$