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Destroying sodium cyanide / potassium cyanide in the lab



A discussion started in 2004 and continuing through 2017 . . .

(2004)

Q. In my laboratory I have a flask containing 100 grs. of potassium cyanide that broke its cover. I want to destroy that cyanide to throw it away but I don't know how to do it. Can you help me?

Ana Honório
- Coimbra, Coimbra, Portugal


Hydrogen Cyanide Detector

(2004)

A. It's best to be trained in this, and it's also considered inadvisable to neutralize concentrated cyanides because of the generation of cyanogen chloride; but assuming you have lab skills and a lab hood, this one is not difficult. Slowly add bleach (sodium hypochlorite, NaOCl) while stirring. Have caustic soda on hand (sodium hydroxide, NaOH) and add it is necessary to keep the pH above 10.5. Proceed slowly and carefully. When starch paper [linked by editor to product info at Amazon] (potassium iodide) turns dark blue, indicating an excess of bleach,the amenable cyanide will be gone, converted to cyanate.

Next, it's best to oxidize the cyanate to nitrogen and carbon dioxide. This takes time, more bleach, and careful pH control, held at 8.5.

Accidental or inadvertent acidification of cyanide releases poisonous hydrogen cyanide gas, so you need pH instrumentation that works well.

Ted Mooney, finishing.com
Teds signature
Ted Mooney, P.E. RET
finishing.com
Pine Beach, New Jersey


(2004)

A. Best disposal method is to sell that 100 g of KCN to needy people in industries.

Regards,

PKM Dinesh
- Chennai, India


thumbs up signExactly, PKM. Thanks for saying it.

Ted Mooney, finishing.com
Teds signature
Ted Mooney, P.E. RET
finishing.com
Pine Beach, New Jersey



Using Oxygen gas for Cyanide oxidation

(2006)

Q. We are currently looking for ways to lower our chemical costs. We currently use chlorine bleach for oxidation and sodium bisulfite for dechlorination. Is it possible to use oxygen gas, injected into a carrier stream, to oxidize the cyanide in the first stage of the process? The first stage is accomplished in a separate tank from the second stage, where several first stage tanks are combined to second stage.

David M. Shook
helicopters - Grand Prairie, Texas


(2006)

A. Do not think that O2 will work well at all. It probably will take ozone or peroxide (diluted for safety)

James Watts
- Navarre, Florida


simultaneous (2006)

A. Oxygen may work some if you also use a UV light.

paul morkovsky
Paul Morkovsky
- Shiner, Texas, USA


(2006)

A. Yes, you can oxidize cyanide with oxygen gas. In fact, you can hydrolyze it with just water. At 50 atm pressure, and 200 °C, that is. There are some proprietary cyanide destruct processes that operate this way, mainly used by centralized waste disposal facilities that treat concentrated cyanide wastes that other people generate.

This is a good example of the "thermodynamics vs kinetics" problem. Whether a reaction *can* occur, and, how fast it *will* occur, are two separate issues.

Another example are the two cyanide treatment chemicals that Mr. Watts mentions - hypochlorite and peroxide. Hypochlorite, or chlorine gas, reacts with cyanide very rapidly at pH 10 - 11.5. It will also oxidize cyanate - with enough chlorine you can take cyanide all the way down to nitrogen gas and carbon dioxide. Peroxide, on the other hand, is slow to react even in the presence of catalysts with cyanide, and will not oxidize cyanate at all. And, it is very tough, under normal conditions, to get the cyanide below about 25 ppm with peroxide alone.

My approach to concentrated cyanide wastes (2 - 5 g/l) is to take the pH down to about 11 with sodium bicarbonate, add copper ions as a catalyst, then peroxide over a period of hours to bring the cyanide down to about 50 ppm. The endpoint of this treatment stage is signaled by a color change to green, as copper is liberated from its colorless cyanide complex. Then, I use hypochlorite to bring it down the rest of the way. The advantages of this are: 1) little cyanogen chloride is generated and 2) the volume of the waste is not increased as much as it would be if hypochlorite alone was used. Peroxide is "stronger" in the sense that it contains more equivalents of oxidizer per gallon.

Hope this is of some help.

dave wichern
Dave Wichern
Consultant - The Bronx, New York


(2006)

A. I have seen a process described in which you add sodium chloride and then pass a current through two electrodes. Chlorine is produced at the anode and destroys cyanide. To be effective there are several practical details you will need:- Presumably some agitation will be necessary. The anode current density. The anode material, presumably carbon. The pH.

Nick Clatworthy
- Whitstable, Kent, Great Britain



Need help with disposal of new unused Sodium Cyanide

February 24, 2017

Q. Hi, I currently have 5 pounds of unused sodium cyanide. How can I get rid of this safely?

Rick N [last name deleted for privacy by Editor]
- Brick, New Jersey


February 2017

A. Hi. If the container is unopened it should be relatively easy to sell it to a jeweler or plating shop. If it's open, it will probably be much harder. You didn't note your qualifications or where you got this, but if you haven't had haz-mat training, and otherwise know your way around a lab, and have a proper lab to work in, you'll need to pay to have it disposed of if you can't sell it. Good luck.

Regards,

pic of Ted Mooney
Teds signature
Ted Mooney, P.E. RET
finishing.com
Pine Beach, New Jersey
Striving to live "Aloha"

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