The iron content of an iron supplement must be determined. The manufacturer stat

Question

The iron content of an iron supplement must be determined. The manufacturer states that each tablet contains 1 000.0 mg of iron. A tablet with a mass of 4.9283 grams is digested in nitric acid to release Fe^3+ into solution. After filtration to remove non-soluble components, the iron in solution is precipitated with sodium bicarbonate. What mass of sodium bicarbonate must be added to precipitate the iron in solution assuming a 50% excess of precipitant is used? Assume no sources of interfering metals are present.

Explanation / Answer

Mass of iron =1g

Atomic weight of iron = 55.845 u

No of moles of iron = mass/atomic mass

= 1/55.845 = 0.179 moles

Precipitate is Fe(OH)3

Required sodium bicarbonate = 1.5 x 3 x 0.0179 = 0.08055 moles

Wt of sodium bicarbonate = 0.08055 × 84 =6.7662 g

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