What will happen if ammonium chloride solution is used to standardize the potassium tetraoxomangate(vii)solution?
I don't believe there is a reaction between NH4Cl and KMnO4.
If ammonium chloride solution is used to standardize the potassium tetraoxomangate(VII) solution, the following reaction will occur:
2MnO4^- + 16H+ + 10Cl^- → 2Mn^2+ + 8H2O + 5Cl2
Here, potassium tetraoxomangate(VII) (KMnO4) is reduced to Mn^2+ ions by ammonium chloride (NH4Cl) in an acidic solution.
To standardize the potassium tetraoxomangate(VII) solution using ammonium chloride, we need to determine the concentration of the KMnO4 solution. This involves a titration process:
1. Prepare a solution of an accurately known concentration of ammonium chloride (NH4Cl).
2. Measure a known volume of the KMnO4 solution using a burette.
3. Add the measured volume of KMnO4 solution to a flask.
4. Add a few drops of concentrated sulfuric acid (H2SO4) to the flask to provide the acidic medium.
5. Titrate the KMnO4 solution by adding the ammonium chloride solution from a burette until a color change occurs.
6. The color change indicates the oxidation of the ammonium chloride solution, and the endpoint is reached when the color change becomes permanent.
7. Record the volume of ammonium chloride solution used.
From the volume of ammonium chloride used and its known concentration, we can calculate the number of moles of NH4Cl. Since the stoichiometry of the reaction is known (2:10), we can determine the number of moles of MnO4^- oxidized.
Finally, we can calculate the concentration of the KMnO4 solution using the formula:
Concentration of KMnO4 solution = moles of MnO4^- / volume of KMnO4 solution used
This standardized KMnO4 solution can then be used for various analytical purposes.