The equilibrium constant \(K_{\mathrm{a}}\) for the reaction

is \(6.0 \times 10^{-3}\).

a. Calculate the \(\mathrm{pH}\) of a \(0.10 \mathrm{M}\) solution of \(\mathrm{Fe}\left(\mathrm{H}_{2} \mathrm{O}ight)_{6}{ }^{3+}\).

b. Calculate the \(\mathrm{pH}\) necessary for \(99.90 \%\) of the iron(III) to be in the form \(\mathrm{Fe}\left(\mathrm{H}_{2} \mathrm{O}ight)_{6}{ }^{3+}\).

c. Will a \(1.0 \mathrm{M}\) solution of iron(II) nitrate have a higher or lower \(\mathrm{pH}\) than a \(1.0 \mathrm{M}\) solution of iron(III) nitrate? Explain.

Transcribed Image Text:

3+ Fe(HO)6+ (aq) + HO(l) Fe(HO)(OH)2+ (aq) + H3O+ (aq)