ferusamoniumsulphate reaction with sulphuric acid
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The reaction between ferric ammonium sulfate and sulfuric acid is also known as the iron(III) ammonium sulfate titration. This reaction is commonly used in analytical chemistry as a way to determine the concentration of various substances in a solution.
To perform this reaction, you will need the following materials and equipment:
1. Ferric Ammonium Sulfate (Fe(NH4)2(SO4)2·6H2O): This is a green crystalline compound that is commonly available.
2. Sulfuric Acid (H2SO4): This is a highly corrosive and dangerous compound, so handle it with care.
3. Distilled Water: This is used to prepare solutions and rinse equipment.
4. Burette and Burette Stand: This is used to measure and add solutions in controlled amounts.
5. Pipettes: These are used to measure precise volumes of solutions.
6. Indicator Solution: This is a chemical compound that changes color depending on the pH of the solution. Common indicators for this reaction include potassium dichromate (K2Cr2O7) or potassium permanganate (KMnO4).
Now, let's go through the steps involved in this reaction:
1. Preparation of Sulfuric Acid Solution: In a clean beaker, measure a known volume of sulfuric acid with a pipette. You can use a 1 M (Molar) or 0.1 M solution depending on the concentration of the ferric ammonium sulfate you want to determine.
2. Dilution of Ferric Ammonium Sulfate: In another beaker, dissolve a known mass of ferric ammonium sulfate in distilled water. The concentration will depend on the reaction's purpose. Stir the solution thoroughly to ensure complete dissolution of the compound.
3. Titration: Transfer the diluted ferric ammonium sulfate solution into a clean flask. Add a few drops of the indicator solution to the flask. The solution will turn from its original color towards the desired endpoint.
4. Burette Setup: Fill the burette with the sulfuric acid solution, ensuring there are no air bubbles. Record the initial volume of the sulfuric acid in the burette.
5. Titration Process: Slowly add the sulfuric acid solution from the burette into the flask with the diluted ferric ammonium sulfate solution. Vigorously swirl the flask during this process to ensure complete reaction.
6. Endpoint Determination: Continue adding the sulfuric acid solution slowly until the color change of the indicator shows that the reaction has reached its endpoint. The color will indicate that all the ferric ammonium sulfate has reacted and excess sulfuric acid is present.
7. Final Volume Determination: Record the final volume of sulfuric acid solution used from the burette. This volume will be used to calculate the concentration of ferric ammonium sulfate.
After obtaining the volume used, you can calculate the concentration of the ferric ammonium sulfate solution using stoichiometry and the balanced chemical equation. Note that the balanced equation for this reaction is:
Fe(NH4)2(SO4)2 + 6H2SO4 -> 2Fe2(SO4)3 + (NH4)2SO4 + 6H2O
Remember to always follow proper lab safety guidelines when working with potentially hazardous chemicals.