Final answer:
Iron ions with different oxidation states (iron(II) and iron(III)) exhibit distinct chemical reactivity. This can result in the formation of different compounds, like iron(II) chloride or iron(III) chloride, each with unique properties. Solubility rules, including the insolubility of hydroxides like Fe(OH)3, are used to predict precipitate formation in reactions.
Step-by-step explanation:
When iron(II) sulfate and iron(III) nitrate are combined with the same substance or substances and only the iron ions react, we can conclude that the different oxidation states of iron lead to different chemical behaviors. This is observed through the names given to the iron compounds, which reflect the charge on the iron ion, such as iron(II) chloride or iron(III) chloride. In the reaction provided, when iron(III) reacts with hydroxide ions, an insoluble product Fe(OH)3 is formed according to solubility rules. We can expect different compounds to form when iron(II) is involved instead of iron(III) due to the different charges resulting in different reactivities.
The solubility rules help predict the formation of a precipitate in a reaction. For instance, sodium nitrate remains soluble in water because all nitrates are soluble, while hydroxides are generally insoluble unless they are bound to certain cations like Na+, which is not the case for iron. The subscripts in a compound's chemical formula indicate the mole ratio of the elements present in the compound, and these ratios are critical for understanding the stoichiometry of a reaction and the resultant properties of the substance.