What should the pH be to remove iron impurities from wastewater?
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What should the pH be to remove iron impurities from wastewater?
What happens at pH 4.4? Transform into divalent? Or precipitation? Precipitation seems impossible; in that case it would have to be converted to a divalent form, but this wouldn’t serve the purpose of removing impurities.
Last time I went to a ferroalloy plant to do experiments, it seemed that precipitation could occur when the pH was above 10; both copper and ferrous iron gave a green color. The engineers from the engineering company said it was ferrous iron, copper, and nickel.
Is it to remove other impurities with iron? Is iron the impurity that needs to be removed? For example: if you are removing iron impurities from the electrolyte, the sodium ferricyanide method is generally used – it’s a proven technique; I think those who have worked with this know about it ； If iron is used to remove other pollutants, such as arsenic from wastewater, there are two mechanisms: one is a reaction mechanism that depends on pH conditions, and the other is a flocculation mechanism involving ferric hydroxide formed by trivalent iron, which also relies on different pH conditions. In short, it depends on your goals and the path you choose.
Iron is an impurity that needs to be removed. First, oxidize ferrous iron to ferric iron, then use lime, alkalis, etc. to adjust the pH for precipitation and flocculation, thereby converting it into iron oxide precipitate
Use Na2S; it gives better results.