In large doses, the body's ability to change cyanide into thiocyanate is overwhelmed. Large doses of cyanide prevent cells from using oxygen and eventually these cells die. The heart, respiratory system, and central nervous system are most susceptible to cyanide poisoning.
In large doses, the body's ability to change cyanide into thiocyanate is overwhelmed. Large doses of cyanide prevent cells from using oxygen and eventually these cells die. The heart, respiratory system, and central nervous system are most susceptible to cyanide poisoning.
I’m not a chemist, but hydrochloric acid, based on the name, has already reacted with chlorine. Id be surprised if anything happened, maybe a slight reaction with impurities in the acid to create more?
I’m not a chemist, but hydrochloric acid, based on the name, has already reacted with chlorine. Id be surprised if anything happened, maybe a slight reaction with impurities in the acid to create more?
Yes, prussic acid is the acid corresponding to the cyanides. If you add concentrated sulphuric acid to sodium cyanide, you get hydrogen cyanide gas, aka prussic acid.
Yes, prussic acid is the acid corresponding to the cyanides. If you add concentrated sulphuric acid to sodium cyanide, you get hydrogen cyanide gas, aka prussic acid.
Assuming you do this in aqueous medium (e.g. in water), you may generate gaseous hydrogen cyanide, which is quite poisonous if inhaled. (It shuts down your body’s ability to respire, and your body starves for energy promptly and probably painfully. Noone who has died this way has reported just how painful it was.) Furthermore, cyanide is generally toxic to animal life, so you can’t let it out into the environment.
So, if you have cyanide-containing wastes, it is critical to keep them well-alkalized at all times. Analytical wet-chemistry laboratories, and industries using cyanide, keep such wastes segregated, in order to assure this. Final destruction of cyanide wastes is a somewhat involved process; pH and Oxygen Reducing Potential must both be monitored carefully to avoid producing HCN or using excessive oxidant reagents. The equipment for this is specialized and must be maintained and operated without error.
I said above, “in aqueous medium”, only because if you mixed *dry* sodium cyanide and *dry* citric acid, say, and kept them *dry*, you *probably* wouldn’t produce hydrogen cyanide very rapidly. But I really don’t recommend trying this, especially if you lack enough chemical common sense to ask the question you did.
Assuming you do this in aqueous medium (e.g. in water), you may generate gaseous hydrogen cyanide, which is quite poisonous if inhaled. (It shuts down your body’s ability to respire, and your body starves for energy promptly and probably painfully. Noone who has died this way has reported just how painful it was.) Furthermore, cyanide is generally toxic to animal life, so you can’t let it out into the environment.
So, if you have cyanide-containing wastes, it is critical to keep them well-alkalized at all times. Analytical wet-chemistry laboratories, and industries using cyanide, keep such wastes segregated, in order to assure this. Final destruction of cyanide wastes is a somewhat involved process; pH and Oxygen Reducing Potential must both be monitored carefully to avoid producing HCN or using excessive oxidant reagents. The equipment for this is specialized and must be maintained and operated without error.
I said above, “in aqueous medium”, only because if you mixed *dry* sodium cyanide and *dry* citric acid, say, and kept them *dry*, you *probably* wouldn’t produce hydrogen cyanide very rapidly. But I really don’t recommend trying this, especially if you lack enough chemical common sense to ask the question you did.
Often the whole is greater than the sum of its parts. H2SO4 + HNO3 (mixed acid) is a powerful nitrating agent; HNO3 (aqua regia) dissolves the “Noble metals”,
Often the whole is greater than the sum of its parts. H2SO4 + HNO3 (mixed acid) is a powerful nitrating agent; HNO3 (aqua regia) dissolves the “Noble metals”,
The mixture will produce a lot of chlorine gas. NEVER add an acid or a base to chlorine bleach. It’s extremely dangerous.
The mixture will produce a lot of chlorine gas. NEVER add an acid or a base to chlorine bleach. It’s extremely dangerous.
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In large doses, the body's ability to change cyanide into thiocyanate is overwhelmed. Large doses of cyanide prevent cells from using oxygen and eventually these cells die. The heart, respiratory system, and central nervous system are most susceptible to cyanide poisoning.
In large doses, the body's ability to change cyanide into thiocyanate is overwhelmed. Large doses of cyanide prevent cells from using oxygen and eventually these cells die. The heart, respiratory system, and central nervous system are most susceptible to cyanide poisoning.
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You could add a solution containing either ferrous or ferric ions and produce a [Fe(CN.)6]2+ (or 3+) complex. You’ll get a lovely blue as well…!
You could add a solution containing either ferrous or ferric ions and produce a [Fe(CN.)6]2+ (or 3+) complex. You’ll get a lovely blue as well…!
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I’m not a chemist, but hydrochloric acid, based on the name, has already reacted with chlorine. Id be surprised if anything happened, maybe a slight reaction with impurities in the acid to create more?
I’m not a chemist, but hydrochloric acid, based on the name, has already reacted with chlorine. Id be surprised if anything happened, maybe a slight reaction with impurities in the acid to create more?
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Yes, prussic acid is the acid corresponding to the cyanides. If you add concentrated sulphuric acid to sodium cyanide, you get hydrogen cyanide gas, aka prussic acid.
Yes, prussic acid is the acid corresponding to the cyanides. If you add concentrated sulphuric acid to sodium cyanide, you get hydrogen cyanide gas, aka prussic acid.
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Bile is not a strong acid, it is mildly alkaline. The pH ranges from about 7.50 to 8.05.
Bile is mostly (neutral) cholesteral.
Also, bile salts (salts of bile acids) and other components, such as (but not limited to) bilirubin.
Bilirubin pigments, breakdown products of heme, are likely to lose their orange yellow color or change to a lighter shade when oxidized by bleach..
Bile is not a strong acid, it is mildly alkaline. The pH ranges from about 7.50 to 8.05.
Bile is mostly (neutral) cholesteral.
Also, bile salts (salts of bile acids) and other components, such as (but not limited to) bilirubin.
Bilirubin pigments, breakdown products of heme, are likely to lose their orange yellow color or change to a lighter shade when oxidized by bleach..
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Nothing.
Nitrogen has very strong triple bonds and doesn't react under most conditions.
Nothing.
Nitrogen has very strong triple bonds and doesn't react under most conditions.
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It gets hot and you end up with salt and water. Make sure that it is properly neutralised before you taste it.
It gets hot and you end up with salt and water. Make sure that it is properly neutralised before you taste it.
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Assuming you do this in aqueous medium (e.g. in water), you may generate gaseous hydrogen cyanide, which is quite poisonous if inhaled. (It shuts down your body’s ability to respire, and your body starves for energy promptly and probably painfully. Noone who has died this way has reported just how painful it was.) Furthermore, cyanide is generally toxic to animal life, so you can’t let it out into the environment.
So, if you have cyanide-containing wastes, it is critical to keep them well-alkalized at all times. Analytical wet-chemistry laboratories, and industries using cyanide, keep such wastes segregated, in order to assure this. Final destruction of cyanide wastes is a somewhat involved process; pH and Oxygen Reducing Potential must both be monitored carefully to avoid producing HCN or using excessive oxidant reagents. The equipment for this is specialized and must be maintained and operated without error.
I said above, “in aqueous medium”, only because if you mixed *dry* sodium cyanide and *dry* citric acid, say, and kept them *dry*, you *probably* wouldn’t produce hydrogen cyanide very rapidly. But I really don’t recommend trying this, especially if you lack enough chemical common sense to ask the question you did.
Assuming you do this in aqueous medium (e.g. in water), you may generate gaseous hydrogen cyanide, which is quite poisonous if inhaled. (It shuts down your body’s ability to respire, and your body starves for energy promptly and probably painfully. Noone who has died this way has reported just how painful it was.) Furthermore, cyanide is generally toxic to animal life, so you can’t let it out into the environment.
So, if you have cyanide-containing wastes, it is critical to keep them well-alkalized at all times. Analytical wet-chemistry laboratories, and industries using cyanide, keep such wastes segregated, in order to assure this. Final destruction of cyanide wastes is a somewhat involved process; pH and Oxygen Reducing Potential must both be monitored carefully to avoid producing HCN or using excessive oxidant reagents. The equipment for this is specialized and must be maintained and operated without error.
I said above, “in aqueous medium”, only because if you mixed *dry* sodium cyanide and *dry* citric acid, say, and kept them *dry*, you *probably* wouldn’t produce hydrogen cyanide very rapidly. But I really don’t recommend trying this, especially if you lack enough chemical common sense to ask the question you did.
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Often the whole is greater than the sum of its parts. H2SO4 + HNO3 (mixed acid) is a powerful nitrating agent; HNO3 (aqua regia) dissolves the “Noble metals”,
Often the whole is greater than the sum of its parts. H2SO4 + HNO3 (mixed acid) is a powerful nitrating agent; HNO3 (aqua regia) dissolves the “Noble metals”,
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You make hydrogen cyanide gas which is highly poisonous. Don’t even think about trying this unless you are working in a good fume hood.
You make hydrogen cyanide gas which is highly poisonous. Don’t even think about trying this unless you are working in a good fume hood.
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