What are the oxidizing agents for Formic acid and Ferrous ammonium sulphate?
To determine the oxidizing agents for formic acid and ferrous ammonium sulfate, we need to understand the concept of oxidation and reduction reactions.
Oxidation refers to the process where a substance loses electrons, while reduction refers to the process where a substance gains electrons. In a redox reaction, one species is oxidized (loses electrons) while another species is reduced (gains electrons).
For formic acid (HCOOH), the oxidizing agent will be the substance that accepts electrons from formic acid, causing it to be oxidized. One common oxidizing agent for formic acid is potassium permanganate (KMnO4). In this reaction, formic acid is oxidized to carbon dioxide (CO2), while potassium permanganate is reduced to manganese dioxide (MnO2).
The balanced equation for this reaction is:
HCOOH + 2KMnO4 -> CO2 + 2H2O + 2MnO2 + 2KOH
For ferrous ammonium sulfate ((NH4)2Fe(SO4)2), the oxidizing agent will be the substance that accepts electrons from ferrous ammonium sulfate, causing it to be oxidized. One common oxidizing agent for ferrous ammonium sulfate is potassium dichromate (K2Cr2O7). In this reaction, ferrous ammonium sulfate is oxidized to ferric ammonium sulfate ((NH4)2Fe(SO4)2), while potassium dichromate is reduced to chromium(III) sulfate (Cr2(SO4)3).
The balanced equation for this reaction is:
(NH4)2Fe(SO4)2 + K2Cr2O7 + H2SO4 -> (NH4)2Cr2(SO4)3 + Fe2(SO4)3 + K2SO4 + H2O
In summary, potassium permanganate is an oxidizing agent for formic acid, while potassium dichromate is an oxidizing agent for ferrous ammonium sulfate.