When aqueous solutions of iron (III) sulfate (Fe2(SO4)3) and sodkum hydroxide were mixed, a precipitate formed. What is the precipitate?

Could it be Fe(OH)3?

about 5 years late, but yes, it is Fe(OH)3

To determine the precipitate formed when aqueous solutions of iron (III) sulfate (Fe2(SO4)3) and sodium hydroxide (NaOH) are mixed, we need to consider the balanced chemical equation for the reaction.

The balanced equation for the reaction can be written as follows:

Fe2(SO4)3 + 6 NaOH -> 2 Fe(OH)3 + 3 Na2SO4

From the equation, we can see that iron (III) sulfate reacts with sodium hydroxide to form iron (III) hydroxide as a precipitate, and sodium sulfate as a soluble compound.

Therefore, the precipitate formed when the two solutions are mixed is iron (III) hydroxide (Fe(OH)3).

To determine the precipitate formed when aqueous solutions of iron (III) sulfate (Fe2(SO4)3) and sodium hydroxide (NaOH) are mixed, we need to understand the reaction that takes place between these compounds.

The chemical equation for the reaction is:

Fe2(SO4)3 + 6NaOH → 2Fe(OH)3 + 3Na2SO4

This equation shows that iron (III) sulfate reacts with sodium hydroxide to form iron (III) hydroxide and sodium sulfate as the products.

The precipitate formed in this reaction is iron (III) hydroxide (Fe(OH)3). It appears as a brownish solid, which indicates the presence of iron.

So, in summary, when aqueous solutions of iron (III) sulfate and sodium hydroxide are mixed, the precipitate formed is iron (III) hydroxide (Fe(OH)3).