Under strongly basic conditions

CHEMISTRY · Multi-part · CBSE · Chemistry · Redox Reactions · Redox Reactions

Problem

Under strongly basic conditions, iodate ion can oxidize arsenite ion according to the following unbalanced equation: IO3−\mathrm{IO_3^-} (aq) + AsO33−\mathrm{AsO_3^{3-}} (aq) → I−\mathrm{I^-} (aq) + AsO43−\mathrm{AsO_4^{3-}} (aq) Water and hydroxide ions participate in the reaction. (a) Balance the equation in basic solution, using the smallest whole-number coefficients and explicitly showing H2O\mathrm{H_2O} and OH−\mathrm{OH^-} where they appear. (b) The coefficient in front of IO3−\mathrm{IO_3^-} in the balanced equation contains a fractional value before fractions are cleared to whole numbers. State that fractional coefficient and explain why such fractions can arise during balancing. (c) After balancing, determine the mass (in grams) of IO3−\mathrm{IO_3^-} required to deliver exactly 4.50 mol of electrons to the reaction. (d) A current of 1.25 A is passed through a solution in which the balanced reaction is occurring. Calculate the time, in minutes, required for the current to provide the 4.50 mol of electrons used in part (c). (Faraday constant = 96 485 C mol−1 e−96\,485\,\text{C}\,\text{mol}^{-1}\,\mathrm{e^-})

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