Thursday, August 13, 2015

Sodium Cyanide

I was right. This chemical is used in refining Gold and other metals and is illegal to even be in California but might still be allowed in Nevada by gold smelters and refiners. This powder is likely all over the place after the blasts in Tianjin, China. The problem with this is breathing it in a powder form or having it get into the water table because I don't believe there is (Any) safe amount for humans to breathe or to ingest in any way without either getting sick or dying eventually. 

I learned about this while I was a working partner in a mining company in California during the early 1970s.

Sodium cyanide

From Wikipedia, the free encyclopedia
Sodium cyanide
Sodium cyanide bonding
Sodium cyanide space filling
Identifiers
143-33-9 Yes
ChEMBL ChEMBL1644697 
ChemSpider 8587 Yes
EC number 205-599-4
Jmol-3D images Image
PubChem 8929
RTECS number VZ7525000
UN number 1689
Properties
NaCN
Molar mass 49.0072 g/mol
Appearance white solid
Odor faint almond-like
Density 1.5955 g/cm3
Melting point 563.7 °C (1,046.7 °F; 836.9 K)
Boiling point 1,496 °C (2,725 °F; 1,769 K)
48.15 g/100 mL (10 °C)
63.7 g/100 mL (25 °C)
Solubility soluble in ammonia, methanol, ethanol
very slightly soluble in dimethylformamide, SO2
insoluble in dimethylsulphoxide
1.452
Thermochemistry
70.4 J/mol K
115.7 J/mol K
-91 kJ/mol
Hazards
Safety data sheet ICSC 1118
EU classification Very Toxic T+ Dangerous for the Environment (Nature) N Corrosive C [1]
R-phrases R26/27/28, R32, R50/53
S-phrases (S1/2), S7, S28, S29, S45, S60, S61
NFPA 704
Flammability code 0: Will not burn. E.g., water Health code 4: Very short exposure could cause death or major residual injury. E.g., VX gas Reactivity code 0: Normally stable, even under fire exposure conditions, and is not reactive with water. E.g., liquid nitrogen Special hazards (white): no codeNFPA 704 four-colored diamond
0
4
0
Flash point Non-flammable
Lethal dose or concentration (LD, LC):
LD50 (Median dose)
 6.44 mg/kg (oral, rat)
4 mg/kg (sheep, oral)
15 mg/kg (mammal, oral)
8 mg/kg (rat, oral)[3]
US health exposure limits (NIOSH):
TWA 5 mg/m3[2]
C 5 mg/m3 (4.7 ppm) [10-minute][2]
25 mg/m3 (as CN)[2]
Related compounds
Other cations
 Potassium cyanide
Related compounds
 Hydrogen cyanide
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
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Infobox references


Sodium cyanide is an inorganic compound with the formula NaCN. It is a white, water-soluble solid. Cyanide has a high affinity for metals, which leads to the high toxicity of this salt. Its main application, in gold mining, also exploits its high reactivity toward metals. When it is treated with acid, it forms the toxic gas hydrogen cyanide:
NaCN + H2SO4 → HCN + NaHSO4

Contents

Production and chemical properties

Sodium cyanide is produced by treating hydrogen cyanide with sodium hydroxide:[5]
HCN + NaOH → NaCN + H2O
Worldwide production was estimated at 500,000 tons in the year 2006. In former times, it was prepared by the Castner-Kellner process involving the reaction of sodium amide with carbon at elevated temperatures.
NaNH2 + C → NaCN + H2
The structure of solid NaCN is related to that of sodium chloride.[6] The anions and cations are each six-coordinate. Potassium cyanide (KCN) adopts a similar structure. Each Na+ forms pi-bonds to two CN− groups as well as two "bent" Na---CN and two "bent" Na---NC links.[7]
Because the salt is derived from a weak acid, NaCN readily reverts to HCN by hydrolysis: the moist solid emits small amounts of hydrogen cyanide, which smells like bitter almonds (not everyone can smell it—the ability thereof is due to a genetic trait[8]). Sodium cyanide reacts rapidly with strong acids to release hydrogen cyanide. This dangerous process represents a significant risk associated with cyanide salts. It is detoxified most efficiently with hydrogen peroxide (H2O2) to produce sodium cyanate (NaOCN) and water:[5]
NaCN + H2O2 → NaOCN + H2O

Applications

Cyanide mining

See also: cyanide process

Sodium gold cyanide

Sodium cyanide is mainly used to extract gold and other precious metals in mining industry. This application exploits the high affinity of gold(I) for cyanide, which induces gold metal to oxidize and dissolve in the presence of air and water, producing the salt sodium gold cyanide (or gold sodium cyanide) and sodium hydroxide:
4 Au + 8 NaCN + O2 + 2 H2O → 4 Na[Au(CN)2] + 4 NaOH
A similar process uses potassium cyanide (KCN, a close relative of sodium cyanide) to produce potassium gold cyanide (KAu(CN)2).Few other methods exist for this extraction process.

Chemical feedstock

Several commercially significant chemical compounds are derived from cyanide, including cyanuric chloride, cyanogen chloride, and many nitriles. In organic synthesis, cyanide, which is classified as a strong nucleophile, is used to prepare nitriles, which occur widely in many specialty chemicals, including pharmaceuticals.

Niche uses

Being highly toxic, sodium cyanide is used to kill or stun rapidly such as in widely illegal cyanide fishing and in collecting jars used by entomologists.

Toxicity

Main article: Cyanide poisoning
Sodium cyanide, like other soluble cyanide salts, is among the most rapidly acting of all known poisons. NaCN is a potent inhibitor of respiration, acting on mitochondrial cytochrome oxidase and hence blocking electron transport. This results in decreased oxidative metabolism and oxygen utilization. Lactic acidosis then occurs as a consequence of anaerobic metabolism. An oral dosage as small as 200-300 mg can be fatal.

See also

References


  • Oxford MSDS
    1. Online 'Mendelian Inheritance in Man' (OMIM) 304300

    External links

    Authority control

  • "NIOSH Pocket Guide to Chemical Hazards #0562". National Institute for Occupational Safety and Health (NIOSH).

  • "Cyanides (as CN)". Immediately Dangerous to Life and Health. National Institute for Occupational Safety and Health (NIOSH).

  • http://cameochemicals.noaa.gov/chemical/4477

  • Andreas Rubo, Raf Kellens, Jay Reddy, Norbert Steier, Wolfgang Hasenpusch "Alkali Metal Cyanides" in Ullmann's Encyclopedia of Industrial Chemistry 2006 Wiley-VCH, Weinheim, Germany. doi:10.1002/14356007.i01_i01

  • Wells, A.F. (1984) Structural Inorganic Chemistry, Oxford: Clarendon Press. ISBN 0-19-855370-6.

  • H. T. Stokes, D. L. Decker, H. M. Nelson, J. D. Jorgensen (1993). "Structure of potassium cyanide at low temperature and high pressure determined by neutron diffraction". Phys. Rev. B 47 (17): 11082–11092. doi:10.1103/PhysRevB.47.11082.

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