What specific name is given to the permanganate titration

Mohr Salt Titration It is possible to do redox titration by titrating potassium permanganate (KMnO4) against Mohr salt, as shown in the figure. In oxidation-reduction (redox) titrations, the action of the indicator is identical to that of the other forms of visual colour titrations when the endpoint is in close proximity to the indicator. To compare the strength of a specific potassium permanganate solution to a standard ferrous ammonium sulphate (Mohr’s salt) solution in order to assess its potency. In the presence of sulfuric acid, potassium permanganate is a powerful oxidant, according to theory. Mohr salt is a double salt that forms a single crystalline structure and has the formula (NH 4 ) 2 . FeSO 4 . 6H 2 O. It is also known as Mohr’s salt. Mohr’s salt is referred to by its chemical name as ferrous ammonium sulphate. It should be noted that in this titration, Mohr salt serves as a reducing agent and potassium permanganate serves as an oxidising agent. The reaction between Mohr’s salt and potassium permanganate is therefore classified as a redox reaction. The process takes place because the ferrous ion from Mohr’s salt is oxidised, and the pink manganese contained in potassium permanganate, which is in the +7 oxidation state, is reduced to the colourless manganese ion (Mn 2+ ). This titration is based on oxidation-reduction titrations, which are performed in a laboratory. When sulfuric acid is used to titrate ferrous ammonium sulphate solution against potassium perma...

Chemistry Practical Class 12 Determination of Concentration/Molarity of KMnO4 Solution by Titrating it against a Standard Solution of Oxalic Acid Viva Questions with Answers Q1. How to convert M/10 oxalic acid solution into N/10 oxalic acid solution? Answer. To make the conversion add an equal volume of water so that the solution converted to N/10. Q2. What is the formula and basicity of oxalic acid? Answer. The formula for oxalic acid is (COOH) 2.2H 2O. The basicity of oxalic acid is 2 means it is a dibasic acid. Q3. In this titration of KMnO 4 vs oxalic acid, what is the indicator used? Answer. Potassium permanganate itself is purple in colour and acts as a self indicator. Q4. What is meant by redox titration? Answer. In redox titrations, both oxidation and reduction reactions take place simultaneously. During titration, one will get oxidised at the same time the other reactant will get reduced also called a redox reaction Q5. What specific name is given to the permanganate titrations? Answer. Permanganometric titrations are redox titrations that involve potassium permanganate. Q6. Which indicator is used in the permanganate titration? Answer. No indicator is used. This is because KMnO 4 acts as a self-indicator. Q7. Why isn’t an indicator used in permanganometry? Answer. An indicator is not required for titration of colourless or slightly coloured solutions because 0.01 mL of 0.02M potassium permanganate imparts a pale-pink colour to 100 mL of water. Q8. In KMnO 4 titra...

\( \newcommand\) • • • • • • • • • • • • • • • Analytical titrations using redox reactions were introduced shortly after the development of acid–base titrimetry. The earliest Redox titration took advantage of the oxidizing power of chlorine. In 1787, Claude Berthollet introduced a method for the quantitative analysis of chlorine water (a mixture of Cl 2, HCl, and HOCl) based on its ability to oxidize indigo, a dye that is colorless in its oxidized state. In 1814, Joseph Gay-Lussac developed a similar method for determining chlorine in bleaching powder. In both methods the end point is a change in color. Before the equivalence point the solution is colorless due to the oxidation of indigo. After the equivalence point, however, unreacted indigo imparts a permanent color to the solution. The number of redox titrimetric methods increased in the mid-1800s with the introduction of MnO 4 –, Cr 2O 7 2–, and I 2 as oxidizing titrants, and of Fe 2 + and S 2O 3 2– as reducing titrants. Even with the availability of these new titrants, redox titrimetry was slow to develop due to the lack of suitable indicators. A titrant can serve as its own indicator if its oxidized and reduced forms differ significantly in color. For example, the intensely purple MnO 4 – ion serves as its own indicator since its reduced form, Mn 2 +, is almost colorless. Other titrants require a separate indicator. The first such indicator, diphenylamine, was introduced in the 1920s. Other redox indicators soon foll...

This problem has been solved! You'll get a detailed solution from a subject matter expert that helps you learn core concepts. See Answer See Answer See Answer done loading Question:Experiment No. 06 ExperimentName: Standardization of potassium permanganate solution (KMnO4) with a standard sodium oxalate (Na2C2O4) solution. Preparation of Standard sodium oxalate solution: Weigh out accurately 0.67 g of sodium oxalate salt in a 100 ml volumetric flask. Dissolve by adding a little amount of distilled water and make up to mark with Experiment No. 06 ExperimentName: Standardization of potassium permanganate solution (KMnO4) with a standard sodium oxalate (Na2C2O4) solution. Preparation of Standard sodium oxalate solution: Weigh out accurately 0.67 g of sodium oxalate salt in a 100 ml volumetric flask. Dissolve by adding a little amount of distilled water and make up to mark with distilled water. Working Procedure (i) Take the supplied potassium permanganate (KMnO4) solution into the burette and note the initial reading. (ii) Pipette out exactly 10 ml of sodium oxalate (Na2C_04) solution by a volumetric pipette into a conical flask. (iii) Add about 50 ml of 1M Sulphuric acid solution to the conical flask. (iv) Carry out the titration rapidly at the ordinary temperature until the first point pink color appears throughout the solution. Allow to stand until the color disappears and the solution becomes colorless. Warm the solution to 50-60°C and continue titration to a first perman...

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Learning Objectives • To use titration methods to analyze solutions quantitatively. To determine the amounts or concentrations of substances present in a sample, chemists use a combination of chemical reactions and stoichiometric calculations in a methodology called quantitative analysis. Suppose, for example, we know the identity of a certain compound in a solution but not its concentration. If the compound reacts rapidly and completely with another reactant, we may be able to use the reaction to determine the concentration of the compound of interest. In a titration, a carefully measured volume of a solution of known concentration, called the titrant, is added to a measured volume of a solution containing a compound whose concentration is to be determined (the unknown). The reaction used in a titration can be an acid–base reaction, a precipitation reaction, or an oxidation–reduction reaction. In all cases, the reaction chosen for the analysis must be fast, complete, and specific; that is, only the compound of interest should react with the titrant. The equivalence point is reached when a stoichiometric amount of the titrant has been added—the amount required to react completely with the unknown. Determining the Concentration of an Unknown Solution Using a Titration The chemical nature of the species present in the unknown dictates which type of reaction is most appropriate and also how to determine the equivalence point. The volume of titrant added, its concentration, an...

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 ...

Specific Learning Objectives • Define oxidation, reduction, oxidizing agent and reducing agent. • Define oxidation state and oxidation number. • Have a knowledge of the oxidation state rules and assign oxidation numbers to atoms in molecules and ions. • Identify a redox reaction by assigning oxidation numbers to each element. • Write the oxidation and reduction half reactions for a redox reaction. • Distinguish between a redox reaction and a non-redox reaction. • Write balanced Oxidation/Reduction Equations. • Apply the Nernst equation in all directions to determine missing quantities. • Describe and discuss Redox titrations. • Carry out redox-type titrations and associated calculations. Summary of learning activity #3 Chemical reactions in which there is a transfer of electrons from one substance to another are known as oxidation-reduction reactions or redox reactions. In this unit, we will consider the class of reactions called oxidation- reduction, or redox and examine the oxidation-reduction process and use the oxidation state and oxidation number concepts to not only identify redox reactions but also keep track of electrons transferred in a chemical reaction. The introductory sections of the unit explains the fundamental principles of galvanic cells, the thermodynamics of electrochemical reaction. Some applications of the concept of redox equilibria in explaining oxidation-reduction titrations as a technique for volumetric chemical analysis are also discussed. Key Con...