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The reduction reaction in this experiment uses up ions. This produces ions in solution. What you see as rust is a precipitate that forms between Iron(III) ions and hydroxide ions. Write this reaction below.

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Related questions

a solution containing only hydroxide group ions forms a colored solid on addition of excess ammonia. This solid reacts with hydrogen peroxide in alkaline solution to form a yellow solution and a rust red solid. This red solid dissolves in hydrochloric acid and forms a red solution upon addition of potassium thiocyanate.

Which ions are present?

What ions are absent?

Which ions are undetermined based on the information provided?

When solutions of iron(III) nitrate and sodium hydroxide are mixed, a red precipitate forms.

(a) Write a balanced net ionic equation for the reaction that occurs.

(b) What is the mass of the precipitate when 10.00 g of iron(III) nitrate in 135 mL of solution is combined with 100.0 mL of 0.2255 M NaOH?

(c) What is the molarity of the ion in excess? (Ignore spectator ions and assume volumes are additive.)


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