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Addition of concentrated sulfuric acid to potassium permanganate gives Mn 2 O 7. [76] Although no reaction may be apparent, the vapor over the mixture will ignite paper impregnated with alcohol. Potassium permanganate and sulfuric acid react to produce some ozone, which has a high oxidizing power and rapidly oxidizes the alcohol, causing it to ...
A permanganate can oxidize an amine to a nitro compound, [7] [8] an alcohol to a ketone, [9] an aldehyde to a carboxylic acid, [10] [11] a terminal alkene to a carboxylic acid, [12] oxalic acid to carbon dioxide, [13] and an alkene to a diol. [14] This list is not exhaustive. In alkene oxidations one intermediate is a cyclic Mn(V) species: [15]
Manganate is formally the conjugate base of hypothetical manganic acid H 2 MnO 4, which cannot be formed because of its rapid disproportionation. However, its second acid dissociation constant has been estimated by pulse radiolysis techniques: [3] HMnO − 4 ⇌ MnO 2− 4 + H + pK a = 7.4 ± 0.1
Permanganic acid (or manganic(VII) acid) is the inorganic compound with the formula H MnO 4 and various hydrates. [3] This strong oxoacid has been isolated as its dihydrate. It is the conjugate acid of permanganate salts. It is the subject of few publications and its characterization as well as its uses are very limited.
In weak acidic medium MnO − 4 can not accept 5 electrons to form Mn 2+. Instead, it accepts only 3 electrons and forms solid MnO 2 by the following reaction: MnO − 4 + 4 H + + 3 e − → MnO 2 + 2 H 2 O; E° = +1.69 V. In a strongly basic solution, with the concentration c (NaOH) >1 mol dm −3, only one electron is accepted to produce ...
Permanganic acid can be prepared by the reaction of dilute sulfuric acid with a solution barium permanganate, the insoluble barium sulfate byproduct being removed by filtering: [3] Ba(MnO 4) 2 + H 2 SO 4 → 2 HMnO 4 + BaSO 4. The sulfuric acid used must be dilute; reactions of permanganates with concentrated sulfuric acid yield the anhydride ...
It is the sodium salt of oxalic acid. It contains sodium cations Na + and oxalate anions C 2 O 2− 4. It is a white, crystalline, odorless solid, that decomposes above 290 °C. [2] Sodium oxalate can act as a reducing agent, and it may be used as a primary standard for standardizing potassium permanganate (KMnO 4) solutions.
pH sensitive polymers can be broken into two categories: those with acidic groups (such as -COOH and -SO 3 H) and those with basic groups (-NH 2). The mechanism of response is the same for both, only the stimulus varies. The general form of the polymer is a backbone with functional "pendant groups" that hang off of it.