How many moles of kmno4 are reacted with one mole of ferrous oxalate

• Course • NCERT • Class 12 • Class 11 • Class 10 • Class 9 • Class 8 • Class 7 • Class 6 • IIT JEE • Exam • JEE MAINS • JEE ADVANCED • X BOARDS • XII BOARDS • NEET • Neet Previous Year (Year Wise) • Physics Previous Year • Chemistry Previous Year • Biology Previous Year • Neet All Sample Papers • Sample Papers Biology • Sample Papers Physics • Sample Papers Chemistry • Download PDF's • Class 12 • Class 11 • Class 10 • Class 9 • Class 8 • Class 7 • Class 6 • Exam Corner • Online Class • Quiz • Ask Doubt on Whatsapp • Search Doubtnut • English Dictionary • Toppers Talk • Blog • Download • Get App Doubtnut is No.1 Study App and Learning App with Instant Video Solutions for NCERT Class 6, Class 7, Class 8, Class 9, Class 10, Class 11 and Class 12, IIT JEE prep, NEET preparation and CBSE, UP Board, Bihar Board, Rajasthan Board, MP Board, Telangana Board etc NCERT solutions for CBSE and other state boards is a key requirement for students. Doubtnut helps with homework, doubts and solutions to all the questions. It has helped students get under AIR 100 in NEET & IIT JEE. Get PDF and video solutions of IIT-JEE Mains & Advanced previous year papers, NEET previous year papers, NCERT books for classes 6 to 12, CBSE, Pathfinder Publications, RD Sharma, RS Aggarwal, Manohar Ray, Cengage books for boards and competitive exams. Doubtnut is the perfect NEET and IIT JEE preparation App. Get solutions for NEET and IIT JEE previous years papers, along with chapter wise NEET MCQ solutions. G...

More • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • •

A redox titration is a titration in which the analyte and titrant react through an oxidation–reduction reaction. As in acid–base titrations, the endpoint of a redox titration is often detected using an indicator. Potassium permanganate (KMnO₄) is a popular titrant because it serves as its own indicator in acidic solution. Created by Jay. This may be a simplistic argument, but the Mn in MnO₄⁻ is in the +7 oxidation state. No atom "wants" to give up its electrons; after all, it takes almost 3000 kJ/mol to remove the electron from Fe²⁺ and convert it to Fe³⁺. But Mn " is desperate" to get electrons to reach a lower oxidation state. Like the bully it is, it grabs electrons from as many Fe²⁺ ions as it can find to get to a +2 state. It takes 10Fe²⁺ ions to produce enough electrons to reduce 2 Mn(VII) to 2Mn²⁺ ions. The Mn might take even more electrons from Fe, but it takes a whopping 5300 kJ/mol to convert Fe³⁺ to Fe⁴⁺, and few things are able to supply that much energy. - [Voiceover] We've already seen how to do an acid-base titration. Now let's look at a redox titration. Let's say we have a solution containing iron two plus cations. We don't know the concentration of the iron two plus cations, but we can figure out the concentration by doing a redox titration. Let's say we have 10 milliliters of our solution, and let's say it's an acidic solution. You could have some sulfuric acid in there. In solution, we have iron two plus cations and a source of protons from our acid. To ...

Solution: The number of moles of K M n O 4 ​ that will be needed to react completely with one mole of ferrous oxalate in acidic solution is 5 3 ​ . Potassium permangante is a very strong oxidizing agent. It oxidizes iron(II) ion as well as the oxalate ion. Oxalate oxidation: 2 M n O 4 ​ − + 16 H + + 5 C 2 ​ O 4 2 − ​ → 2 M n 2 + + 8 H 2 ​ O + 10 C O 2 ​ Iron(II) oxidation: M n O 4 − ​ + 8 H + + 5 F e 2 + → M n 2 + + 4 H 2 ​ O + 5 F e 3 + Hence, moles of K M n O 4 ​ that will be needed to react completely with one mole of ferrour oxalate F e ( C 2 ​ O 4 ​ ) is 5 3 ​ ( 2 moles for oxalate and 1 mole for iron (II)).