Sodium chloride: Difference between revisions
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==Disposal== | ==Disposal== | ||
==See Also== | ==See Also== | ||
* [ | * [[Salt]] | ||
==References== | ==References== | ||
<references/> | <references/> | ||
Revision as of 12:04, 25 June 2019
| Chemical formula | NaCl |
|---|---|
| OTP appearance | white crystals |
| Molar Mass(g/mol) | 58.44 |
| Density(g/cc) | 2.16 |
| Melting Point(°C) | 801 |
| Boiling Point(°C) | 1413 |
| Solubility in water(g/L) | 359 |
| Solubility in ethanol(g/L) | 0.65 |
| NFPA 704 |  0
0
0
|
Uses
Primary
- WHO LEM
- Necessary for human diet
- Essential feedstock for hydrochloric acid
- Primary source of sodium and chlorine for chemistry
Natural occurrence
- Sodium chloride occurrs naturally in salt
Hazards
Production
Extraction
from salt
removing magnesium, iron, sulfate, phosphate, carbonate
By adding an excess of calcium hydroxide, magnesium and iron anions precipitate as Mg(OH)2,Fe(OH)2,Fe(OH)3 and the cations SO4,PO4,CO3 precipitate as their calcium salts. See also Lime softening.
- Produce a warm saturated solution of salt in distilled water
- Produce a warm saturated solution of calcium hydroxide in distilled water
- Combine the solutions
- Cool
- Bubble carbon dioxide through solution, if necessary
- Filter
- Discard residue
- Evaporate filtrate, containing purer salt
removing bromine and iodine
- See the production of bromine and iodine from salt water using chlorine gas.
removing potassium
- Produce a hot saturated solution of salt
- Cool until ppt forms.
- Filter
- The residue contains all the potassium chloride along with some sodium chloride. Recycle.
- Evaporate the filtrate
- The residue is purer salt
Synthesis
- Combine 23g of sodium metal with 35g of chlorine gas in a closed but not sealed container, and ignite. This is a very exothermic reaction.
- 2 Na + Cl2 → 2 NaCl
- Combine 36.46g of hydrochloric acid with 40g of sodium hydroxide. This is a very exothermic reaction.
- NaOH + HCl → NaCl + H2O
Testing
Purification
Remove sodium iodide
- Wash with propanone. NaI is soluble in acetone, salt is not.
removing magnesium, iron, sulfate, phosphate, carbonate
By adding an excess of calcium hydroxide, magnesium and iron anions precipitate as Mg(OH)2,Fe(OH)2,Fe(OH)3 and the cations SO4,PO4,CO3 precipitate as their calcium salts. See also Lime softening.
- Produce a warm saturated solution of salt in distilled water
- Produce a warm saturated solution of calcium hydroxide in distilled water
- Combine the solutions
- Cool
- Bubble carbon dioxide through solution, if necessary
- Filter
- Discard residue
- Evaporate filtrate, containing purer salt