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It is a redox titration that involves the use of permanganates to measure the amount of analyte present in unknown chemical samples. [1] It involves two steps, namely the titration of the analyte with potassium permanganate solution and then the standardization of potassium permanganate solution with standard sodium oxalate solution. The ...
Potassium manganate is the inorganic compound with the formula K 2 MnO 4. This green-colored salt is an intermediate in the industrial synthesis of potassium permanganate (KMnO 4), a common chemical. [1] Occasionally, potassium manganate and potassium permanganate are confused, but each compound's properties are distinct.
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 (/ p ər ˈ m æ ŋ ɡ ə n eɪ t, p ɜːr-/) [1] is a chemical compound with the manganate(VII) ion, MnO − 4, the conjugate base of permanganic acid. Because the manganese atom has a +7 oxidation state, the permanganate(VII) ion is a strong oxidising agent. The ion is a transition metal ion with a tetrahedral structure. [2]
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
Measurements, first and second derivative in a potentiometric titration. In analytical chemistry, potentiometric titration is a technique similar to direct titration of a redox reaction. It is a useful means of characterizing an acid. No indicator is used; instead the electric potential is measured across the analyte, typically an electrolyte ...
Typically, a titration is performed with one or more reactants in the titration vessel and one or more reactants in the burette. Knowing the analytical concentrations of reactants initially in the reaction vessel and in the burette, all analytical concentrations can be derived as a function of the volume (or mass) of titrant added.
The chemical chameleon reaction shows the process in reverse, by reducing violet potassium permanganate first to green potassium manganate and eventually to brown manganese dioxide: [1] [2] [5] KMnO 4 (violet) → K 2 MnO 4 (green) → MnO 2 (brown/yellow suspension) Blue potassium hypomanganate may also form as an intermediate. [6]