`K_(a)` for the ionisation of `Fe^(3+)` to `Fe(OH)^(2+)` and `H^(o+)` is `6.5 xx 10^(-3)`, what is the maximum `pH` value which could be used so that at least `95%` of the total `Fe^(3+)` in a dilute solution exists as `Fe^(3+)`?

K_(a) for the reaction, Fe^(3+)(aq)+H_(2)O(l)hArr Fe(OH)^(2+)(aq) +H_(3)O^(o+)(aq) is 6.5 xx 10^(-3) , what is the maximum pH value which could be used so that at least 80% of the total iron (III) in a dilute solution exsists as Fe^(3+) ?

K_(a) for the reaction, Fe^(3+)(aq)+H_(2)O(l)hArr Fe(OH)^(2+)(aq) +H_(3)O^(o+)(aq) is 6.5 xx 10^(-3) , what is the maximum pH value which could be used so that at least 80% of the total iron (III) in a dilute solution exsists as Fe^(3+) ?

K_(a) for the reaction, Fe^(3+)(aq)+H_(2)O(l)hArr Fe(OH)^(2+)(aq) +H_(3)O^(o+)(aq) is 6.5 xx 10^(-3) , what is the maximum pH value which could be used so that at least 80% of the total iron (III) in a dilute solution exsists as Fe^(3+) ?

Find the oxidation number of Fe in [Fe(H_2O)_6]^(3+)

Hybridization of Fe in K_(3)Fe(CN)_(6) is

Iron oxide has formula Fe_(0.94)O . What fraction of Fe exists as Fe^(+3) ?

Calculate magnetic moment of Fe^(3+) in [Fe(CN)_(6)]^(3+) and in [Fe(H_(2)O)_(6)]^(3+)

Iron oxide has formula Fe_"0.94"O. What fraction of Fe exists as Fe^(+3) ?