ලෙඩ් නයිට්ට්‍රේට්

ලෙඩ්(II) නයිට්‍රේට් යනු රසායනික සූත්‍රය Pb(NO3)₂ වූ අකාබනික සංයෝගයකි. එය සාමාන්‍යයෙන් වර්ණයක් රහිත ස්පටිකයක් හෝ සුදු පැහැ කුඩක් ලෙස පවතින අතර අනෙක් බොහෝ ලෙඩ්(II) ලවණ මෙන් නොව, ජලයේ හොඳින් දිය වේ.

ලෙඩ් නයිට්ට්‍රේට්

Names
Lead(II) nitrate
වෙනත් නාම Lead nitrate Plumbous nitrate Lead dinitrate Plumb dulcis
Identifiers
	{{{value}}}
3D model ()	Interactive image
	CHEBI:{{{value}}}
	100.030.210
	{{{value}}}
	{{{value}}}
	{{{value}}}
	1469
(EPA)	DTXSID2035069
Properties
Molecular formula	Pb(NO3)2
	331.2 g/mol
Appearance	White colourless crystals
	4.53 g/cm^3 (20 °C)
	270 °C, decomp.
in water	52 g/100 mL (20 °C) 127 g/100 mL (100 °C)
in nitric acid in in	insoluble 0.04 g/100 mL 1.3 g/100 mL
, Ksp	1.782
Structure
	cuboctahedral
Hazards
	{{{value}}}
Related compounds
Other anions
Other cations	Tin(II) nitrate
Related compounds	Bismuth(III) nitrate
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).  Y   (verify)

මධ්‍යම යුගයේ සිට plumb dulcis ලෙස හඳුන්වන මෙය ලෝහක ලෙඩ්(II) හෝ නයිට්‍රික් ඇසිඩ් තුළ ලෙඩ් ඔක්සයිඩ් මඟින් ලෙඩ්(II) නයිට්‍රේට් උත්පාදනය කුඩා ප්‍රමාණ වලින් සිදු වන අතර වෙනත් ලෙඩ් සංයෝග සඳහා කෙලින් ම යොදා ගැනේ. 19 වන සියවසේ දී එක්සත් ජනපදයේ සහ යුරෝපයේ ලෙඩ්(II) නයිට්‍රේට් වාණිජ වශයෙන් නිෂ්පාදනය ඇරඹුණි. ඓතිහාසික වශයෙන් වර්ණක නිෂ්පාදනයේ දී තීන්ත සඳහා අමු ද්‍රව්‍ය ලෙස යොදා ගැනීම ප්‍රධාන භාවිතය වූ නමුත් ටයිටේනියම් ඩයොක්සයිඩ් වලින් සාදන විෂ අඩු තීන්ත නිසා අභාවයට පැමිණෙමින් තිබේ. අනෙකුත් කාර්මික භාවිත වනුයේ නයිලෝන් සහ පොලියෙස්ටර වල තාප ස්ථායිකරණය සහ ඡායා තාප ලේඛ කඩදාසි වල ආලේපන යි. වසර 2000 පමණ සිට ලෙඩ්(II) නයිට්‍රේට් රත්රන් සයනයිඩ සඳහා යොදා ගැණින.

ලෙඩ්(II) නයිට්‍රේට් විෂ සහිත ඔක්සිකාරකයක් වන අතර බොහෝ විට මනුෂ්‍ය ශරීරයට පිළිකා කාරකයක් ලෙස පිළිකා පර්යේෂණ සඳහා වූ අන්තර්ජාතික ඒජන්සිය(International Agency for Research on Cancer) විසින් වර්ගීකරණය කොට ඇත. එම නිසා එය ආශ්වාසයෙන්, අධිග්‍රහණයෙන් සහ ස්පර්ශයෙන් වැළකෙන පරිදි සුදුසු ආරක්ෂිත ස්ථාන වල හැසිරවීම සහ ගබඩා කිරීම කළ යුතු වේ. ලෙඩ්(II) නයිට්‍රේට් වල උපද්‍රව සහිත ස්වාභාවය නිසා එහි සීමාසහිත භාවිත නිරන්තර සමීක්ෂණ යටතේ පවතී.

ඉතිහාසය

මධ්‍යම යුගයේ සිට ක්‍රෝමියම් කහ(lead(II) chromate), ක්‍රෝමියම් තැඹිලි(lead(II) hydroxide chromate), සහ සමාන ලෙඩ් සංයෝග වැනි ලෙඩ් සායම් වල දී වර්ණක සඳහා අමුද්‍රව්‍යයක් ලෙස ලෙඩ්(II) නයිට්‍රේට් නිෂ්පාදනය කරනු ලැබීය. මෙම වර්ණක, සායම් පෙවීම සහ කපු රෙදි වල මුද්‍රණය කිරීම සහ අනෙකුත් රෙදිපිළි සඳහා යොදා ගන්නා ලදී.

1597 දී ජර්මානු විද්‍යාඥ Andreas Libavius විසින් පළමුවෙන් ම නිෂ්පාදිත plumb dulcis සහ calx plumb dulcis සංයෝග වල මධ්‍යකාලීන නම් වල තේරුම එහි රසය නිසා "sweet lead" යැයි නම් කළේය. මතු සියවස් තුළ දී නිසියාකාර අවබෝධයක් නැති නමුත් ලෙඩ්(II) නයිට්‍රේට් හි පිපිරීමේ ගුණය lead azide වැනි විශේෂ ස්පෝටක සඳහා භාවිතා විය.

නිෂ්පාදන ක්‍රියාවලිය සරල රසායනික වන අතර ජලීය නයිට්‍රික් ඇසිඩ් තුළ ලෙඩ් ඵලදායී ලෙස දිය වන අතර පසුව ප්‍රතිඵල ලෙස අවක්ෂේප ඇති කරයි. කෙසේ නමුත් නිෂ්පාදිතයෙන් කුඩා ප්‍රමාණයක් සියවස් ගණනාවක් ඉතිරි වූ අතර ලෙඩ් සංයෝග සෑදීමේ අමු ද්‍රව්‍යක් ලෙස ලෙඩ්(II) නයිට්‍රේට් හි ව්‍යාපාරික නිෂ්පාදනය 1835 තෙක් වාර්තා නොවීය. 1974 දී වර්ණක සහ ගැසලීන් වැනි සංකලන ද්‍රව්‍ය හැර එක්සත් ජනපදයේ ලෙඩ් සංයෝග වල පරිභෝජනය ටොන් 642ක් විය.

ව්‍යුහය

Crystal structure [111] plane

The of solid lead(II) nitrate has been determined by . The compound in the cubic system with the lead atoms in a system. Its is Pa3_Z=4 ( notation), with each side of the cube with length 784 .

The black dots represent the lead atoms, the white dots the nitrate groups 27 picometres above the plane of the lead atoms, and the blue dots the nitrate groups the same distance below this plane. In this configuration, every lead atom is bonded to twelve oxygen atoms (: 281 pm). All N–O bond lengths are identical, at 127 picometres.

Research interest in the crystal structure of lead(II) nitrate was partly based on the possibility of free internal rotation of the nitrate groups within the crystal lattice at elevated temperatures, but this did not materialise.

සම්මිශ්‍රණය සහ උත්පාදනය

ලෙඩ්(II) නයිට්‍රේට් ස්වභාවිකව නොපවතියි. ජලීය නයිට්‍රික් අම්ලයෙහි දියකිරීමෙන් සංයෝගය සාදා ගත හැක:

3 Pb (s) + 8 H⁺ (aq) + 2 NO^-3 (aq) → 3 Pb²⁺ (aq) + 2 NO (g) + 4 H₂O (l)

More commonly, lead(II) nitrate is obtained by dissolving , which is readily available as an intermediate in the processing of , in aqueous nitric acid:

PbO (s) + 2 H⁺ (aq) → Pb²⁺ (aq) + H₂O (l)

In either case, since the is concentrated nitric acid (in which lead(II) nitrate has very low solubility) and the resulting solution contains ions, anhydrous crystals of lead(II) nitrate spontaneously form as a result of the :

Pb²⁺ (aq) + 2 NO^-3 (aq) → Pb(NO₃)₂ (s)

Most commercially available lead(II) nitrate, as well as -scale material, is produced accordingly. Supply is in 25 kilogram bags up to 1000 kilogram , and in laboratory containers, both by general producers of laboratory chemicals and by producers of lead and . No large-scale production has been reported.

In nitric acid treatment of lead-containing wastes, e.g., in the processing of lead– wastes from lead refineries, impure solutions of lead(II) nitrate are formed as . These solutions are reported to be used in the process.

ප්‍රතික්‍රියා

Apart from , lead(II) nitrate is the only common soluble lead compound. Lead(II) nitrate readily in water to give a clear, colourless solution. As an , the dissolution of lead(II) nitrate involves into its constituent ions.

Pb(NO₃)₂ (s) → Pb²⁺ (aq) + 2 NO^-3 (aq)

Lead(II) nitrate forms a slightly acidic solution, with a pH of 3.0 to 4.0 for a 20% aqueous solution.

When concentrated solution is added to lead(II) nitrate solution, are formed, even well past the . Up through the half equivalence point, Pb(NO₃)₂·Pb(OH)₂ predominates, then after this point Pb(NO₃)₂·5Pb(OH)₂ is formed. No simple Pb(OH)₂ is formed up to at least 12.

සංකීර්ණ බව

Lead(II) nitrate is associated with interesting because of its to nitrogen and oxygen electron-donating compounds. The interest is largely academic, but with several potential applications. For example, combining lead nitrate and (EO₅) in a solution of and followed by slow produces a new crystalline material [Pb(NO₃)₂(EO₅)]. In the crystal structure for this compound, the EO₅ chain is wrapped around the lead ion in an similar to that of a . The two bidentate nitrate are in . The total is 10, with the lead ion in a bicapped .

The complex formed by lead(II) nitrate, and a bidentate N-donor ligand is binuclear, with a nitrate group bridging the lead atoms with coordination number of 5 and 6. One interesting aspect of this type of complexes is the presence of a physical gap in the ; i.e., the ligands are not placed symmetrically around the metal ion. This is potentially due to a lead of electrons, also found in lead complexes with an ligand.

This type of chemistry is not unique to the nitrate salt; other lead(II) compounds such as also form complexes, but the nitrate is frequently used because of its solubility properties and its bidentate nature.

ඔක්සිකරණය සහ පිපිරීම

Lead(II) nitrate is an . Depending on the reaction, this may be due to the Pb²⁺(aq) ion, which has a standard (E⁰) of −0.125 V, or the nitrate ion, which under acidic conditions has an E⁰ of +0.956 V. The nitrate would function at high temperatures or in an acidic condition, while the lead(II) works best in a neutral aqueous solution.

When heated, lead(II) nitrate crystals decompose to , (dioxygen) and , accompanied by a crackling noise. This effect is referred to as .

2 Pb(NO₃)₂ (s) → 2 PbO (s) + 4 NO₂ (g) + O₂ (g)

Because of this property, lead nitrate is sometimes used in such as fireworks.

භාවිත

Due to the hazardous nature of lead(II) nitrate, there is a preference for using alternatives in industrial applications. In the formerly major application of , it has largely been replaced by . Other historical applications of lead(II) nitrate, such as in matches and fireworks, have declined or ceased as well. Current applications of lead(II) nitrate include use as a heat stabiliser in nylon and polyesters, as a coating for paper, and in .

On a laboratory scale, lead(II) nitrate provides one of two convenient and reliable sources of . By carefully drying lead(II) nitrate and then heating it in a steel vessel, is produced along with (dioxygen) following the decripitation equation shown above. Alternatively, nitrogen dioxide is formed when concentrated nitric acid is added to copper turnings; in this case, substantial can also be produced. In either case, the resulting nitrogen dioxide exists in equilibrium with its dimer, :

2 NO₂⇌ N₂O₄

In order to remove either impurity, the gas mixture is condensed and fractionally distilled to give a mixture of NO₂ and N₂O₄. As the dimerisation is exothermic, low temperatures favour N₂O₄ as the dominant form.

To improve the process in the , lead(II) nitrate solution is added. Although a bulk process, only limited amounts (10 to 100 milligrams lead(II) nitrate per kilogram gold) are required. Both the cyanidation itself, as well as the use of lead compounds in the process, are deemed controversial due to the compounds' toxic nature.

In organic chemistry, lead(II) nitrate has been used as an oxidant, for example as an alternative to the for oxidation of halides to aldehydes. It has also found use in the preparation of from . Because of its toxicity it has largely fallen out of favour, but it still finds occasional use, for example as a bromide scavenger during .

සුරක්ෂිතභාවය

ප්‍රධාන ලිපිය:

Lead(II) nitrate is toxic, and ingestion may lead to acute lead poisoning, as is applicable for all soluble lead compounds. All are classified by the (IARC) as (Category 2A). They have been linked to and in experimental animals and to renal cancer, and lung cancer in humans, although studies of workers exposed to lead are often complicated by concurrent exposure to . Lead is known to substitute for in a number of enzymes, including (porphobilinogen synthase) in the biosynthetic pathway and , important for the correct metabolism of DNA and can therefore cause fetal damage.

මේවාත් බලන්න

• Pigments containing lead, such as , , and
• Historical compounds, such as , , , and

යොමුව

1. Patnaik, Pradyot (2003). Handbook of Inorganic Chemical Compounds. McGraw-Hill. p. 475. ISBN . සම්ප්‍රවේශය 2009-06-06.
2. Partington, James Riddick (1950). A Text-book of Inorganic Chemistry. MacMillan. p.  838.
3. (1595). Alchemia Andreæ Libavii. Francofurti: Iohannes Saurius.
4. Barkley, J.B. (October 1978). "Lead nitrate as an oxidizer in blackpowder". Pyrotechnica. IV. : Pyrotechnica Publications: 16–18.
5. "Lead". Encyclopædia Britannica Eleventh Edition. සම්ප්‍රවේශය 2006-10-11.
6. Macgregor, John (1847). Progress of America to year 1846. London: Whittaker & Co. ISBN .
7. Greenwood, Norman N. (1997). Chemistry of the Elements (2nd ed.). Oxford: Butterworth-Heinemann. pp. 388, 456. ISBN . {{}}: Unknown parameter |coauthors= ignored (|author= suggested) ()
8. Hamilton, W.C. (1957). "A neutron crystallographic study of lead nitrate". 10 (2): 103–107. doi:10.1107/S0365110X57000304.
9. Nowotny, H. (1986). "Structure refinement of lead nitrate". C42 (2): 133–35. doi:10.1107/S0108270186097032. {{}}: Unknown parameter |coauthors= ignored (|author= suggested) ()
10. (1967). Kirk-Othmer Encyclopedia of Chemical Technology. Vol. 12 (Iron to Manganese) (second completely revised ed.). New York: & Sons. p.  272. ISBN .
11. Adlam, George Henry Joseph (1938). A Inorganic Chemistry. London: John Murray. {{}}: Unknown parameter |coauthors= ignored (|author= suggested) ()
12. "Product catalog; other products". Tilly, Belgium: Sidech. සම්ප්‍රවේශය 2008-01-05.
13. Ferris, L.M. (1959). "Lead nitrate—Nitric acid—Water system". Journal of Chemicals and Engineering Date. 5 (3): 242–242. doi:10.1021/je60007a002.
14. http://www.mallbaker.com/americas/msds/english/L3130_msds_us_Default.pdf^[]
15. Pauley, J. L. (1954). "Basic Salts of Lead Nitrate Formed in Aqueous Media". . 76 (16): 4220–4222. doi:10.1021/ja01645a062. {{}}: Unknown parameter |coauthors= ignored (|author= suggested) ()
16. Rogers, Robin D. (1996). "Structural Chemistry of Poly (ethylene glycol). Complexes of Lead(II) Nitrate and Lead(II) Bromide". 35 (24): 6964–6973. doi:10.1021/ic960587b. PMID 11666874. {{}}: Unknown parameter |coauthors= ignored (|author= suggested) (); Unknown parameter |vol= ignored (|volume= suggested) ()
17. Mahjoub, Ali Reza (2001). "A Dimeric Mixed-Anions Lead(II) Complex: Synthesis and Structural Characterization of [Pb₂(BTZ)₄(NO₃)(H₂O)](ClO₄)₃ {BTZ = 4,4'-Bithiazole}". . 30 (12): 1234. doi:10.1246/cl.2001.1234. {{}}: Unknown parameter |coauthors= ignored (|author= suggested) ()
18. Wan, Shuang-Yi (2002). "2D 4.8² Network with threefold parallel interpenetration from nanometre-sized tripodal ligand and lead(II) nitrate". (21): 2520–2521. doi:10.1039/b207568g. {{}}: Unknown parameter |coauthors= ignored (|author= suggested) ()
19. Hill, John W. (1999). General Chemistry (2nd ed.). Upper Saddle River, New Jersey: Prentice Hall. p.  781. ISBN . {{}}: Unknown parameter |coauthors= ignored (|author= suggested) ()
20. "Historical development of titanium dioxide". Millennium Inorganic Chemicals. October 21, 2007 දින මුල් පිටපත වෙතින් සංරක්ෂණය කරන ලදී. සම්ප්‍රවේශය 2008-01-04.
21. Habashi, Fathi (1998 (est)). . Quebec City, Canada: Laval University. 2008-03-30 දින මුල් පිටපත වෙතින් සංරක්ෂණය කරන ලදී. සම්ප්‍රවේශය 2008-01-05. {{}}: Check date values in: |year= (); Unknown parameter |deadurl= ignored (|url-status= suggested) ()
22. "Auxiliary agents in gold cyanidation". Gold Prospecting and Gold Mining. සම්ප්‍රවේශය 2008-01-05.
23. Schulze, K. E. (1884). "Über α- und β-Methylnaphtalin". . 17: 1530. doi:10.1002/cber.188401701384.
26. "Lead nitrate, Chemical Safety Card 1000". , International Occupational Safety and Health Information Centre. 1999. සම්ප්‍රවේශය 2008-01-19. {{}}: Unknown parameter |month= ignored ()
27. "Inorganic and Organic Lead Compounds" (PDF). IARC Monographs on the Evaluation of Carcinogenic Risks to Humans. Suppl. 7. : 239. 1987. සම්ප්‍රවේශය 2008-01-19.
28. World Health Organization, International Agency for Research on Cancer. (2006). "Inorganic and Organic Lead Compounds" (PDF). IARC Monographs on the Evaluation of Carcinogenic Risks to Humans. 87. . ISBN . සම්ප්‍රවේශය 2008-01-01.
29. Mohammed-Brahim, B. (1985). "Erythrocyte pyrimidine 5'-nucleotidase activity in workers exposed to lead, mercury or cadmium". Int Arch Occup Environ Health. 55 (3): 247–52. doi:10.1007/BF00383757. PMID 2987134. {{}}: Unknown parameter |coauthors= ignored (|author= suggested) ()

බාහිර ඇමුණුම්

ලෙඩ් නයිට්ට්‍රේට් හා සබැඳි මාධ්‍ය විකිමාධ්‍ය කොමන්ස් හි ඇත.

• Woodbury, William D. (1982). "Lead". Mineral yearbook metals and minerals. : 515–42. සම්ප්‍රවේශය 2008-01-18.
• "Lead". NIOSH Pocket Guide to Chemical Hazards. National Institute for Occupational Safety and Health. 2005. NIOSH 2005-149. සම්ප්‍රවේශය 2008-01-19. {{}}: Unknown parameter |month= ignored ()
• "Lead and Lead Compounds Fact Sheet". National Pollutant Inventory. Australian Government, Department of the Environment and Water Resources. 2007. January 11, 2008 දින මුල් පිටපත වෙතින් සංරක්ෂණය කරන ලදී. සම්ප්‍රවේශය 2008-01-19. {{}}: Unknown parameter |month= ignored ()
• "Lead". A Healthy home environment, Health hazards. US Alliance for healthy homes. සම්ප්‍රවේශය 2008-01-19.
• "Demonstration movie: Bright Orange Yellow How can you get it". සම්ප්‍රවේශය 2008-01-19.

Material Safety Data Sheets

• MSDS for lead nitrate, PTCL, Oxford University 2007-09-16 at the Wayback Machine
• MSDS for lead nitrate, ProSciTechPDF (126 )
• MSDS for lead nitrate, Science Stuff Inc 2006-03-28 at the Wayback Machine
• MSDS for lead nitrate, Iowa State University 2006-05-04 at the Wayback Machine
• MSDS for lead nitrate, NIST