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Alkali sulfates are formed from sulfur trioxide and sodium-containing compounds. As the formation of vanadates is preferred, sulfates are formed only if the amount of alkali metals is higher than the corresponding amount of vanadium. [3] The same kind of attack has been observed for potassium sulfate and magnesium sulfate.
[11] [12] During combustion, sodium sulfate is reduced to sodium sulfide by the organic carbon in the mixture: 1. Na 2 SO 4 + 2 C → Na 2 S + 2 CO 2. This reaction is similar to thermochemical sulfate reduction in geochemistry. The molten salts ("smelt") from the recovery boiler are dissolved in a process water known as "weak wash".
The following chart shows the solubility of various ionic compounds in water at 1 atm pressure and room temperature (approx. 25 °C, 298.15 K). "Soluble" means the ionic compound doesn't precipitate, while "slightly soluble" and "insoluble" mean that a solid will precipitate; "slightly soluble" compounds like calcium sulfate may require heat to precipitate.
Sodium sulfate is a typical electrostatically bonded ionic sulfate. The existence of free sulfate ions in solution is indicated by the easy formation of insoluble sulfates when these solutions are treated with Ba 2+ or Pb 2+ salts: Na 2 SO 4 + BaCl 2 → 2 NaCl + BaSO 4. Sodium sulfate is unreactive toward most oxidizing or reducing agents.
Toggle the table of contents. Sodium sulfate (data page) ... This page provides supplementary chemical data on sodium sulfate. Material Safety Data Sheet
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2 O and NaOH to precipitate Fe(OH) 2 then immediately adding sodium sulfate Na 2 SO 4 and proceeding to the air oxidation step. [8] [34] A more direct method combines a solution of iron(II) sulfate FeSO 4 with NaOH, and proceeding to the oxidizing step. [18] The suspension must have a slight excess of FeSO 4 (in the ratio of 0.5833 Fe 2+ for ...
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