why should FeSO4 be acidified ?
I don't know that it does. How is it being used. What are the circumstances? What's the experiment? How are you using FeSO4.
How much heat energy is needed to change 3g of
ice at 0C to steam at 100C(Specific latent heat of
fusion of ice=336kj/kg, specific latent of
vapourization of water=2260kj/kg, specific heat
capacity of water=4.2kj/kgk)?
FeSO4 (ferrous sulfate) is a common chemical compound that is often used in laboratory experiments or industrial processes. However, when it comes in contact with air, it is prone to oxidization, transforming into Fe2O3 (iron oxide) and H2SO4 (sulfuric acid). This reaction is commonly observed as the formation of a brownish precipitate.
To prevent this oxidation reaction from occurring, FeSO4 can be acidified. Acidification refers to the addition of an acid, such as sulfuric acid (H2SO4), to a solution. Acidifying FeSO4 serves two main purposes:
1. Preventing Oxidation: Adding acid to FeSO4 helps create an acidic environment, which lowers the pH of the solution. A lower pH limits the availability of oxygen and slows down or prevents the oxidation reaction mentioned earlier. By acidifying FeSO4, you ensure that it remains in its original form, rather than transforming into iron oxide and sulfuric acid.
2. Stabilizing the Solution: Acidifying FeSO4 also helps to stabilize the solution by preventing the formation of hydroxide precipitates. Hydroxide ions (OH-) can react with Fe2+ ions present in FeSO4, leading to the formation of Fe(OH)2, which results in a greenish precipitate. However, by adding acid, the hydroxide ions are neutralized, preventing the formation of Fe(OH)2.
To acidify FeSO4, you can simply add a few drops of sulfuric acid (H2SO4) to the solution. However, it is crucial to exercise caution when handling acids, as they can be corrosive and pose a safety risk.