pure sodium
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anyone has any idea as to how to extract/obtain pure sodium from salt?
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dissolve it in coke and heat it strongly for 24hrs...
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Here is a brief summary of the isolation of sodium.
Sodium would not normally be made in the laboratory as it is so readily available commercially. All syntheses require an electrolytic step as it is so difficult to add an electron to the poorly electronegative sodium ion Na+.
Sodium is present as salt (sodium chloride, NaCl) in huge quantities in underground deposits (salt mines) and seawater and other natural waters. It is easily recovered as a solid by drying.
Sodium chloride has a high melting point (> 800°C) meaning that it sould be expensive to melt it in order to carry out the electrolysis. However a mixture of NaCl (40%) and calcium chloride, CaCl2 (60%) melts at about 580°C and so much less energy and so expense is required for the electrolysis.
cathode: Na+(l) + e- Na (l)
anode: Cl-(l) 1/2Cl2 (g) + e-
The electrolysis is carried out as a melt in a "Downs cell". In practice, the electrolysis process produces calcium metal as well but this is solidified in a collection pipe and returned back to the melt. -
(English, soda; Medieval Latin, sodanum, headache remedy) Long recognized in compounds, sodium was first isolated by Davy in 1807 by electrolysis of caustic soda. Sodium is present in fair abundance in the sun and stars. The D lines of sodium are among the most prominent in the solar spectrum. Sodium is the fourth most abundant element on earth, comprising about 2.6% of the earth's crust; it is the most abundant of the alkali group of metals of which it is a member. The most common compound is sodium chloride, but it occurs in many other minerals, such as soda niter, cryolite, amphibole, zeolite, etc. It is a very reactive element and is never found free in nature. It is now obtained commercially by the electrolysis of absolutely dry fused sodium chloride. This method is much cheaper than that of electrolyzing sodium hydroxide, as was used several years ago. Sodium is a soft, bright, silvery metal which floats on water, decomposing it with the evolution of hydrogen and the formation of the hydroxide. It may or may not ignite spontaneously on water, depending on the amount of oxide and metal exposed to the water. It normally does not ignite in air at temperatures below 115C. Sodium should be handled with respect, as it can be dangerous when improperly handled. Metallic sodium is vital in the manufacture of esters and in the preparation of organic compounds. The metal may be used to improve the structure of certain alloys, to descale metal, to purify molten metals, and as a heat transfer agent. An alloy of sodium with potassium, NaK, is also an important heat transfer agent. Sodium compounds are important to the paper, glass, soap, textile, petroleum, chemical, and metal industries. Soap is generally a sodium salt of certain fatty acids. The importance of common salt to animal nutrition has been recognized since prehistoric times. Among the many compounds that are of the greatest industrial importance are common salt (NaCl), soda ash (Na2CO3), baking soda (NaHCO3), caustic soda (NaOH), Chile saltpeter (NaNO3), di- and tri-sodium phosphates, sodium thiosulfate (hypo, Na2S2O3) . 5H2O), and borax (Na2B4O7 . 10H2O). Thirteen isotopes of sodium are recognized. Metallic sodium is priced at about 15 to 20 cents/lb in quantity. Reagent grade (ACS) sodium in January 1990 cost about $35/lb. On a volume basis, it is the cheapest of all metals. Sodium metal should be handled with great care. It cannot be maintained in an inert atmosphere and contact with water and other substances with which sodium reacts should be avoided.
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something u shldnt be handling in the high humidity of sg
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Ask your chemistry teacher?
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put in water will burn or explode 1 right?
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yupOriginally posted by digicharat:put in water will burn or explode 1 right?
last time chem teacher showed us a video...put in water, the explosion even cause the beaker to break -
depend on amount. if a bit it will "sizzle" on the surfaceOriginally posted by digicharat:put in water will burn or explode 1 right?
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then i think this joker trying to make bomb or do something illegal with it.....
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I dun think you can get the pure form in your home
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Originally posted by deathscythe99:I dun think you can get the pure form in your home
nope.... it'll combust if left in air also... -
Na will combine with H2O.
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singapore air got a lot of water.Originally posted by SBS1908B:Na will combine with H2O. -
normally stored in oilOriginally posted by starblue: nope.... it'll combust if left in air also... -
U mean...humid...Originally posted by starblue:singapore air got a lot of water.
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Seawater...?Originally posted by starblue:singapore air got a lot of water.
+1...
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It's called react, not combineOriginally posted by SBS1908B:Na will combine with H2O. -
alamak la you, that one is caesium la, never pay attentionOriginally posted by monkeybusiness:yup
last time chem teacher showed us a video...put in water, the explosion even cause the beaker to break -
combust? turn into sodium oxide ah?Originally posted by starblue: nope.... it'll combust if left in air also...