What's the aim of titrating potassium tetraoxomaganate(vii) with ammonium iron (ii) tetraoxosulphate (vi)

The KMnO4 oxidizes the Fe(NH4)2(SO4)2 from iron(II) to iron(III) and is reduced from Mn(VII) to Mn(II) in acid solution

The aim of titrating potassium permanganate (KMnO4) with ammonium iron (II) sulfate ((NH4)2Fe(SO4)2) is to determine the concentration of the iron (II) ions in the solution.

Here are the step-by-step instructions for titrating potassium permanganate with ammonium iron (II) sulfate:

1. Prepare the solutions:
- Dilute the ammonium iron (II) sulfate solution to the desired volume and concentration.
- Weigh a known amount of potassium permanganate.

2. Standardize the potassium permanganate solution:
- Pipette a measured volume of the ammonium iron (II) sulfate solution into a conical flask.
- Add a few drops of dilute sulfuric acid (H2SO4) to the flask to acidify the solution.
- Titrate the iron (II) ions in the solution with the potassium permanganate solution while stirring the flask.
- The reaction can be represented as follows:
5Fe2+ + MnO4- + 8H+ → 5Fe3+ + Mn2+ + 4H2O
- Observe the endpoint of the titration, which is indicated by a permanent pink color that persists for about 30 seconds.

3. Calculation:
- Use the volume and concentration of the potassium permanganate solution and the volume of ammonium iron (II) sulfate solution used in the titration to calculate the concentration of the iron (II) ions.

Note: It is important to perform the titration multiple times to obtain accurate and reproducible results.

To understand the aim of titrating potassium tetraoxomanganate(VII) with ammonium iron(II) tetraoxosulphate(VI), it is important to know that titration is a technique used in chemistry to accurately determine the concentration of a substance in a solution. In this specific titration, the aim is to determine the concentration of potassium tetraoxomanganate(VII) (commonly known as potassium permanganate) by reacting it with ammonium iron(II) tetraoxosulphate(VI) (commonly known as Mohr's salt) in a redox reaction.

The primary objective of this titration is to determine the concentration of potassium permanganate. By measuring the volume of Mohr's salt solution required to completely react with a known volume of potassium permanganate solution, the stoichiometry between the two substances can be used to calculate the concentration of the permanganate solution.

The reaction between the two compounds is a redox reaction, where the permanganate ion (MnO4-) is reduced to manganese(II) ion (Mn^2+), while the iron(II) ion (Fe^2+) is oxidized to iron(III) ion (Fe^3+). The reaction can be represented by the following equation:

MnO4- + 8H+ + 5Fe^2+ → Mn^2+ + 4H2O + 5Fe^3+

By carefully titrating the potassium permanganate solution with Mohr's salt solution until the equivalence point is reached, where all the reactants have reacted completely, the volume of Mohr's salt solution required can be used to calculate the concentration of the permanganate solution.

During the titration, a suitable indicator is often used to detect the end point of the reaction, which is the point at which the stoichiometric equivalence between the two reactants is obtained.

In summary, the aim of titrating potassium tetraoxomanganate(VII) with ammonium iron(II) tetraoxosulphate(VI) is to determine the concentration of potassium permanganate solution by measuring the volume of Mohr's salt solution required for a complete reaction.