Why one test tube of 2m sulphuric acid is required in permanganate titration

The titration is between oxalic acid and potassium permanganate, with $\ce$ play in this titration. The question came to me while reading a book (Advanced Chemistry by Philip Matthews - Cambridge university press), I was reading about titrations and this question came to me, but it isn't mentioned in the book. The used analytical reaction of purple permanganate to colourless $\ce$). Sulfuric acid is used because it is stable towards oxidation; whereas, for example, hydrochloric acid would be oxidized to chlorine by permanganate. Sulfuric acid acts as a catalyst in the reaction $\ce$ is consumed. H2SO4 increase the acidic content of the solution so as to prevent MnO4 (purple) to reduced to MnO2(dark brow). Hence sulfuric acid is stable in the present of strong oxidising agent. If HCl acid is use it will be oxidised to Cl and make the end point much higher. Furtherore sulfuric acid increase the H+ as it consume.

[ "article:topic", "authorname:nicholsl", "Beilstein Test", "Benedict\'s Test", "Bicarbonate Test", "Brady\'s Test", "Chromic Acid (Jones) Test", "Ferric Hydroxamate Test", "showtoc:no", "license:ccbyncnd", "transcluded:yes", "source[1]-chem-95742", "source@https://organiclabtechniques.weebly.com/" ] \( \newcommand\) • • • • • • • • • • • • • • • Beilstein Test The Beilstein test confirms the presence of a halogen in solution, although it does not distinguish between chlorine, bromine, or iodine. A copper wire is dipped into the halogen-containing solution and thrust into a flame. The copper oxide on the wire reacts with the organic halide to produce a copper-halide compound that gives a blue-green color to the flame. Procedure: In the fume hood, clean a looped copper wire by thrusting it into the tip of the blue cone of a Bunsen burner flame until it glows (Figure 6.46a). Be sure to "burn off" any residual liquid on the wire (make sure any green flames from previous tests are gone before you begin). Allow the copper to cool to room temperature, then dip it into a test tube containing 5-10 drops of your sample, coating it as much as possible (Figure 6.46b). If the sample is a solid, adhere some of the solid to the copper wire by first wetting the wire with distilled water then touching it to the solid. Immediately plunge the wire with sample into the blue cone of the flame. A positive result is a green flame, although it might be short-lived and faint (it may be easier to ...

For a titration of potassium permanganate into a standard acidified solution of hydrated iron (II) ammonium sulfate, the solution seems to end up brown (due to the formation of manganese dioxide) during the titration unless the titration is carried out extremely slowly. How can I minimise this? Adding sulfuric acid to the solution seemed to help, but is there a physical way to prevent manganese dioxide forming when the titrant is added too rapidly? Adding a large excess of acid helps greatly as the reduction to $\ce$.

For the Determination of iron by Redox Titration experiment, I am finding the role of sulphuric acid and phosphoric acid. Then I found that other than $\ce$? Titration against KMnO4 My understanding is that acidic solutions have a lower potential for the oxidation of ferrous ion by O2 so sulfuric will increase the oxidizing ability of permanganate and not accelerate side reactions. Phosphoric acid complexes ferric ion and has 3 effects. It increases the overall potential change at the equivalence point making endpoints easier to determine both potentiometrically and using a redox indicator and removes the ferric ion color. It should also hasten oxidation by O2. Phosphoric acid is more useful using dichromate oxidant than permanganate since permanganate is its own indicator. The best way to avoid reaction with O2 is to purge with N2 or add a pinch of sodium bicarbonate to the acidic solution and fill the flask with CO2, then add the phosphoric acid.