We are continuing our series of testing oxidants and their experimental results in scavenging hydrogen sulfide. Hydrogen sulfide is a harmful byproduct found within multiple industries with the oilfield being one of the most common. Utilizing an optimal oxidizer can remove these harmful sulfides. Previously surveyed chemicals included Bleach, Peracetic Acid, and Hydrogen Peroxide, and today’s experimental study looks at the difference between sodium chlorite (Chlorite Ion) versus chlorine dioxide.

Dr. Greg Simpson, PhD., surveyed an unbuffered pH sodium chlorite. The results suggested that there was minimal reaction between chlorite and sulfide at a pH of 10. The pH was subsequently reduced to about 4, in which the chlorite became very reactive. There was ample chlorite to consume all of the sulfide tested; the solution remained clear for the entire test, and no elemental sulfur was formed. It took 32.25 ppm sulfide to consume 73.8 ppm chlorite ion, or 2.3 ppm chlorite ion per ppm of sulfide.

When compared with chlorine dioxide, the results yielded a range of 2.9 – 3.4 ppm of chlorine dioxide needed to reduce the sulfide to zero at an unbuffered pH, while 3.7 ppm chlorine dioxide was needed to reduce the sulfide at a pH of 5.

To read more of the study conducted by Dr. Simpson, view the paper below.

Sodium Chlorite vs Chlorine Dioxide

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