Difference between revisions of "Sodium cyanide"
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| Solubility = 48.15 g/100 ml (10 °C)<br>63.7 g/100 ml (25 °C) | | Solubility = 48.15 g/100 ml (10 °C)<br>63.7 g/100 ml (25 °C) | ||
| SolubleOther = Soluble in [[ammonia]], [[ethanol]], [[methanol]]<br>Slightly soluble in [[dimethylformamide]], liq. [[sulfur dioxide|SO<sub>2</sub>]]<br>Insoluble in [[Dimethyl sulfoxide|DMSO]] | | SolubleOther = Soluble in [[ammonia]], [[ethanol]], [[methanol]]<br>Slightly soluble in [[dimethylformamide]], liq. [[sulfur dioxide|SO<sub>2</sub>]]<br>Insoluble in [[Dimethyl sulfoxide|DMSO]] | ||
| − | | | + | | Solubility1 = 40.3 g/100 g (10 °C)<br>49.4 g/100 g (20 °C)<br>58.5 g/100 g (30 °C)<br>67.6 g/100 g (40 °C)<br>76.7 g/100 g (50 °C) |
| + | | Solvent1 = ammonia | ||
| + | | Solubility2 = 0.97 g/100 g (25 °C) | ||
| + | | Solvent2 = ethanol | ||
| + | | Solubility3 = 1.92 g/100 g (25 °C) | ||
| + | | Solvent3 = ethanol 95% | ||
| + | | Solubility4 = 0.02% (25 °C) | ||
| + | | Solvent4 = furfural | ||
| + | | Solubility5 = 6.44 g/100 ml (15 °C)<br>7.8 g/100 ml (25 °C)<br>4.10 g/100 ml (67.4 °C) | ||
| + | | Solvent5 = methanol | ||
| + | | Solubility6 = 0.018 g/100 ml (0 °C) | ||
| + | | Solvent6 = sulfur dioxide<ref>http://nist.gov/data/PDFfiles/jpcrd643.pdf</ref> | ||
| VaporPressure = | | VaporPressure = | ||
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| − | '''Sodium cyanide''' is an inorganic compound with the formula '''NaCN'''. | + | '''Sodium cyanide''' is an inorganic compound with the formula '''NaCN'''. It is a famous chemical historically used as poison, but it's immensely useful in chemistry. |
==Properties== | ==Properties== | ||
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===Physical=== | ===Physical=== | ||
| − | Sodium cyanide is a white crystalline solid, soluble in water, as well as methanol. | + | Sodium cyanide is a white crystalline solid, soluble in [[water]], aq. alkali as well as [[methanol]]. |
==Availability== | ==Availability== | ||
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==Preparation== | ==Preparation== | ||
| − | Preparation of sodium cyanide is extremely dangerous and an inexperienced chemist may even die if proper safety protocols aren't in place. Do not attempt to synthesize NaCN if you don't know what to do. No seriously, don't | + | Preparation of sodium cyanide is extremely dangerous and an inexperienced chemist may even die if proper safety protocols aren't in place. Do not attempt to synthesize NaCN if you don't know what to do. '''No seriously, don't'''! |
A common route involves the reaction of molten [[sodium hydroxide]] with [[cyanuric acid]]. To do this, in a molten alkali crucible/can add 100 g of sodium hydroxide, 43 g of cyanuric acid and 12 g of [[carbon]], which can be ordinary [[charcoal]], though [[activated carbon]] may work better, due to its high surface area. Using a metal rod, mix the components. Slowly heat the mixture for 1 hour until it melts and raise it to 600 °C. The reaction produces trisodium cyanurate and water, which boils off. Above 550 °C, trisodium cyanurate breaks down to sodium cyanate, which is further reduced by carbon to sodium cyanide. [[Carbon dioxide]] is formed, which boils off, producing lots of bubbles. Lots of [[sodium carbonate]] will be produced, as some of the carbon dioxide does not escape and instead it reacts with the molten sodium hydroxide. When the bubbling stops, turn off the heating and let it cool. Break apart the resulting solid and add [[methanol]] to dissolve sodium cyanide, as sodium carbonate and carbon are insoluble in methanol. After most has dissolved, add 100 g of [[sodium bicarbonate]] to neutralize the leftover sodium hydroxide, since NaOH is soluble in methanol, but sodium carbonate is insoluble. Filter the solution and remove the methanol to get solid sodium cyanide. The final product is impure, but can be further purified via recrystallization.<ref>https://www.youtube.com/watch?v=xz7i11XC9wk</ref> | A common route involves the reaction of molten [[sodium hydroxide]] with [[cyanuric acid]]. To do this, in a molten alkali crucible/can add 100 g of sodium hydroxide, 43 g of cyanuric acid and 12 g of [[carbon]], which can be ordinary [[charcoal]], though [[activated carbon]] may work better, due to its high surface area. Using a metal rod, mix the components. Slowly heat the mixture for 1 hour until it melts and raise it to 600 °C. The reaction produces trisodium cyanurate and water, which boils off. Above 550 °C, trisodium cyanurate breaks down to sodium cyanate, which is further reduced by carbon to sodium cyanide. [[Carbon dioxide]] is formed, which boils off, producing lots of bubbles. Lots of [[sodium carbonate]] will be produced, as some of the carbon dioxide does not escape and instead it reacts with the molten sodium hydroxide. When the bubbling stops, turn off the heating and let it cool. Break apart the resulting solid and add [[methanol]] to dissolve sodium cyanide, as sodium carbonate and carbon are insoluble in methanol. After most has dissolved, add 100 g of [[sodium bicarbonate]] to neutralize the leftover sodium hydroxide, since NaOH is soluble in methanol, but sodium carbonate is insoluble. Filter the solution and remove the methanol to get solid sodium cyanide. The final product is impure, but can be further purified via recrystallization.<ref>https://www.youtube.com/watch?v=xz7i11XC9wk</ref> | ||
| − | Another route involves melting a mixture of [[sodium hydroxide]] with [[urea]]. Sodium cyanate is formed, which is ground, mixed with a reducing agent like [[carbon]], [[magnesium]] and ignited in a thermite-like reaction. This produces sodium cyanide and magnesium/carbon oxide. Dissolve the mixture in water and filter it to get rid of the magnesium oxide/hydroxide. This process gives crude sodium cyanide which needs to be purified. | + | Another route involves melting a mixture of [[sodium hydroxide]] with [[urea]]. Sodium cyanate is formed, which is ground, mixed with a powdered reducing agent like [[carbon]], [[magnesium]], [[aluminium]], [[zinc]] (but NOT iron) and ignited in a thermite-like reaction. This produces sodium cyanide and magnesium/carbon oxide. Dissolve the mixture in water and filter it to get rid of the magnesium oxide/hydroxide. This process gives crude sodium cyanide which needs to be purified. |
| − | The NaCN obtained through these routes is extremely impure, and while can be used for general reactions (like dissolving [[gold]] and making [[Prussian blue]] and other Fe(CN) complexes), it is not pure enough for use in organic reactions. To further purify NaCN, | + | The NaCN obtained through these routes is extremely impure, and while can be used for general reactions (like dissolving [[gold]] and making [[Prussian blue]] and other Fe(CN) complexes), it is not pure enough for use in organic reactions. To further purify NaCN, there are two ways: |
| + | *The safe, slow way: convert the impure NaCN into Prussian blue, filter it from the solution, calcinate the Prussian blue using molten sodium hydroxide to reconvert it back into NaCN, and purify it by recrystallizing it from [[ethanol]] and [[water]]. | ||
| + | *The dangerous, quick way: slowly acidify the impure NaCN with an acid, then gently heat the flask to distill the resulting HCN and bubble it in a cooled alcoholic solution of NaOH (methanol is a good choice). Since this route involves working with gaseous HCN, do not do this unless you have experience and this absolutely must be done outside or under a fumehood. | ||
| + | |||
| + | To accurately determine the amount of cyanide from the resulting mixture, you will have to titrate the cyanide solution using a solution of [[silver nitrate]] and using [[p-Dimethylaminobenzalrhodanine|5-(4-Dimethylaminobenzylidene)rhodanine]] as indicator. | ||
==Projects== | ==Projects== | ||
Revision as of 16:10, 30 October 2017
 Impure sodium cyanide made by NurdRage
| |
| Names | |
|---|---|
| IUPAC name
Sodium cyanide
| |
| Other names
Cyanide of sodium
| |
| 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, ethanol, methanol Slightly soluble in dimethylformamide, liq. SO2 Insoluble in DMSO |
| Solubility in ammonia | 40.3 g/100 g (10 °C) 49.4 g/100 g (20 °C) 58.5 g/100 g (30 °C) 67.6 g/100 g (40 °C) 76.7 g/100 g (50 °C) |
| Solubility in ethanol | 0.97 g/100 g (25 °C) |
| Solubility in ethanol 95% | 1.92 g/100 g (25 °C) |
| Solubility in furfural | 0.02% (25 °C) |
| Solubility in methanol | 6.44 g/100 ml (15 °C) 7.8 g/100 ml (25 °C) 4.10 g/100 ml (67.4 °C) |
| Thermochemistry | |
| Std molar
entropy (S |
115.7 J·mol-1·K-1 |
| Std enthalpy of
formation (ΔfH |
-91 kJ/mol |
| Hazards | |
| Safety data sheet | Sigma-Aldrich |
| Flash point | Non-flammable |
| Lethal dose or concentration (LD, LC): | |
| LD50 (Median dose)
|
6.44 mg/kg (rat, oral) 4 mg/kg (sheep, oral) 15 mg/kg (mammal, oral) 8 mg/kg (rat, oral) |
| Related compounds | |
| Related compounds
|
Potassium cyanide |
| Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa). | |
| Infobox references | |
Sodium cyanide is an inorganic compound with the formula NaCN. It is a famous chemical historically used as poison, but it's immensely useful in chemistry.
Contents
Properties
Chemical
Sodium cyanide reacts with halocarbons to give nitriles. Iodine can be used as catalyst.
Physical
Sodium cyanide is a white crystalline solid, soluble in water, aq. alkali as well as methanol.
Availability
Sodium cyanide is sold by chemical suppliers, but due to it's toxicity, companies won't sell to the amateur chemist.
Preparation
Preparation of sodium cyanide is extremely dangerous and an inexperienced chemist may even die if proper safety protocols aren't in place. Do not attempt to synthesize NaCN if you don't know what to do. No seriously, don't!
A common route involves the reaction of molten sodium hydroxide with cyanuric acid. To do this, in a molten alkali crucible/can add 100 g of sodium hydroxide, 43 g of cyanuric acid and 12 g of carbon, which can be ordinary charcoal, though activated carbon may work better, due to its high surface area. Using a metal rod, mix the components. Slowly heat the mixture for 1 hour until it melts and raise it to 600 °C. The reaction produces trisodium cyanurate and water, which boils off. Above 550 °C, trisodium cyanurate breaks down to sodium cyanate, which is further reduced by carbon to sodium cyanide. Carbon dioxide is formed, which boils off, producing lots of bubbles. Lots of sodium carbonate will be produced, as some of the carbon dioxide does not escape and instead it reacts with the molten sodium hydroxide. When the bubbling stops, turn off the heating and let it cool. Break apart the resulting solid and add methanol to dissolve sodium cyanide, as sodium carbonate and carbon are insoluble in methanol. After most has dissolved, add 100 g of sodium bicarbonate to neutralize the leftover sodium hydroxide, since NaOH is soluble in methanol, but sodium carbonate is insoluble. Filter the solution and remove the methanol to get solid sodium cyanide. The final product is impure, but can be further purified via recrystallization.[2]
Another route involves melting a mixture of sodium hydroxide with urea. Sodium cyanate is formed, which is ground, mixed with a powdered reducing agent like carbon, magnesium, aluminium, zinc (but NOT iron) and ignited in a thermite-like reaction. This produces sodium cyanide and magnesium/carbon oxide. Dissolve the mixture in water and filter it to get rid of the magnesium oxide/hydroxide. This process gives crude sodium cyanide which needs to be purified.
The NaCN obtained through these routes is extremely impure, and while can be used for general reactions (like dissolving gold and making Prussian blue and other Fe(CN) complexes), it is not pure enough for use in organic reactions. To further purify NaCN, there are two ways:
- The safe, slow way: convert the impure NaCN into Prussian blue, filter it from the solution, calcinate the Prussian blue using molten sodium hydroxide to reconvert it back into NaCN, and purify it by recrystallizing it from ethanol and water.
- The dangerous, quick way: slowly acidify the impure NaCN with an acid, then gently heat the flask to distill the resulting HCN and bubble it in a cooled alcoholic solution of NaOH (methanol is a good choice). Since this route involves working with gaseous HCN, do not do this unless you have experience and this absolutely must be done outside or under a fumehood.
To accurately determine the amount of cyanide from the resulting mixture, you will have to titrate the cyanide solution using a solution of silver nitrate and using 5-(4-Dimethylaminobenzylidene)rhodanine as indicator.
Projects
- Dissolve gold
- Make nitriles
- Make cyanogen and cyanuric chloride
Handling
Safety
Sodium cyanide is highly toxic. Doses as small as 200 mg can kill a fully grown man.
Storage
Sodium cyanide should be stored in closed bottles, away from any acids, in a locked cabinet with a clear hazard label on the storage bottle.
Disposal
Sodium cyanide can be destroyed by oxidizing it with excess bleach or hydrogen peroxide to the less harmful sodium cyanate.
