A dilute ferrous sulphate solution was gradually added to a beaker containing acidified potassium permanganate solution. The light purple colour of the solution faded and finally disappeared.

A dilute ferrous sulphate solution was gradually added to thebeaker containing acidified permanganate solution. The lightpurple colour of the solution fades and finally disappears.Which of the following is the correct explanation for theobservation?(a) KMnO4 is an oxidising agent, it oxidises FeSO4(b) FeSO4 acts as an oxidising agent and oxidises KMnO4(c) The colour disappears due to dilution; no reaction is involved(d) KMnO4 is an unstable compound and decomposes in presenceof FeSO4 to a colourless compound.

To an aqueous solution of a salt, acidified potassium permanganate is added and the purple colour of potassium permanganate is discharged. It indicates that the solution may containFe2+NO3–Be2+Sn2+

of potassium sulphate dissolves in  75gm . Water at  60∘C . Its Solubility at  60∘C .

Why does the colour of copper sulphate solution change when

Potassium permanganate (KMnO4) is a highly reactive inorganic salt that appears as granular dark purple crystals, nearly black in color.  Due to its useful chemical properties and the fact that its reactions typically do not produce compounds that are toxic, KMnO4 is employed in a variety of applications, including use as a topical skin disinfectant, an antifungal agent, a fire starter, and a disinfectant for drinking water.KMnO4 is widely used as an alternative water treatment agent both to disinfect drinking water and to remove undesirable dissolved iron and sulfur compounds.  The crystals are highly soluble in water and form bright pink aqueous solutions that provide a visual indication of the presence of KMnO4 treatment residual.  As a drinking water disinfectant, a KMnO4 concentration of 1 mg/L is recommended unless higher levels of contamination are indicated by the absence of a pink residual.Industrial production of potassium permanganate is accomplished in two steps.  In step 1, manganese(IV) oxide (MnO2) is heated with potassium hydroxide in the presence of oxygen to produce potassium manganate (K2MnO4), as outlined in Reaction 1.2 MnO2 + 4 KOH + O2 → 2 K2MnO4 + 2 H2OReaction 1In step 2, the potassium manganate is then converted into potassium permanganate electrochemically according to Reaction 2.2 K2MnO4 + 2 H2O → 2 KMnO4 + 2 KOH + H2Reaction 2 Question 43In Reaction 1 shown in the passage, the oxidizing agent is:A.K2MnO4, because potassium loses electrons.B.MnO2, because manganese gains electrons.C.KOH, because hydrogen loses electrons.D.O2, because oxygen gains electrons.