Molar Mass Of Silver Nitrate
 Structural formula | |
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 Crystal structure | |
| Names | |
|---|---|
| IUPAC name Silver nitrate | |
| Systematic IUPAC name Silver(I) nitrate | |
| Other names Nitric acrid silvery(1+) salt | |
| Identifiers | |
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| ECHA InfoCard | 100.028.958 |
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| United nations number | 1493 |
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| Properties | |
| Chemical formula | Ag North O 3 |
| Molar mass | 169.872 g·mol−1 |
| Appearance | colorless solid |
| Aroma | Odorless |
| Density | four.35 k/cm3 (24 °C) 3.97 1000/cmiii (210 °C)[1] |
| Melting point | 209.vii °C (409.five °F; 482.viii G)[one] [iii] |
| Humid point | 440 °C (824 °F; 713 K) decomposes[1] |
| Solubility in h2o | 122 one thousand/100 mL (0 °C) 170 g/100 mL (10 °C) 256 g/100 mL (25 °C) 373 yard/100 mL (40 °C) 912 grand/100 mL (100 °C)[ii] |
| Solubility | Soluble in acetone,[ane] ammonia, ether, glycerol |
| Solubility in acetic acid | 0.776 k/kg (30 °C) 1.244 thou/kg (forty °C) v.503 g/kg (93 °C)[3] |
| Solubility in acetone | 0.35 g/100 g (14 °C) 0.44 g/100 grand (eighteen °C)[two] |
| Solubility in benzene | 0.22 1000/kg (35 °C) 0.44 grand/kg (40.5 °C)[2] |
| Solubility in ethanol | 3.1 g/100 g (19 °C)[two] |
| Solubility in ethyl acetate | ii.7 chiliad/100 g (twenty °C)[3] |
| log P | 0.19 |
| Magnetic susceptibility (χ) | −45.7·x−half-dozen cm3/mol |
| Refractive alphabetize (due north D) | 1.744 |
| Viscosity | 3.77 cP (244 °C) iii.04 cP (275 °C)[3] |
| Structure | |
| Crystal structure | Orthorhombic, oP56[4] |
| Space grouping | P2ane212one, No. 19[iv] |
| Point group | 222[4] |
| Lattice abiding | a = six.992(2) Å, b = 7.335(2) Å, c = 10.125(2) Å[4] α = xc°, β = 90°, γ = 90° |
| Thermochemistry | |
| Heat capacity (C) | 93.i J/mol·K[1] |
| Std molar | 140.ix J/mol·K[i] |
| Std enthalpy of | −124.iv kJ/mol[1] |
| Gibbs costless free energy (Δf G ⦵) | −33.iv kJ/mol[i] |
| Pharmacology | |
| ATC code | D08AL01 (WHO) |
| Hazards | |
| Occupational safety and health (OHS/OSH): | |
| Master hazards | Reacts explosively with ethanol. Toxic. Corrosive. |
| GHS labelling: | |
| Pictograms |     [5] |
| Signal discussion | Danger |
| Hazard statements | H272, H314, H410 [5] |
| Precautionary statements | P220, P273, P280, P305+P351+P338, P310, P501 [five] |
| NFPA 704 (burn down diamond) | 3 0 two OX |
| Lethal dose or concentration (LD, LC): | |
| LDLo (lowest published) | 800 mg/kg (rabbit, oral) 20 mg/kg (canis familiaris, oral)[6] |
| Except where otherwise noted, data are given for materials in their standard land (at 25 °C [77 °F], 100 kPa). Infobox references | |
Crystals of silver nitrate under a microscope.
Silver nitrate is an inorganic compound with chemical formula AgNO
3 . It is a versatile precursor to many other silverish compounds, such as those used in photography. It is far less sensitive to low-cal than the halides. It was once called lunar caustic because silver was called luna past ancient alchemists who associated argent with the moon.[7] In solid silver nitrate, the silver ions are three-coordinated in a trigonal planar organisation.[4]
Synthesis and structure [edit]
Albertus Magnus, in the 13th century, documented the ability of nitric acid to separate gold and silver past dissolving the silverish.[viii] Indeed silver nitrate can be prepared by dissolving argent in nitric acid followed past evaporation of the solution. The stoichiometry of the reaction depends upon the concentration of nitric acid used.
- 3 Ag + 4 HNO3 (cold and diluted) → 3 AgNO3 + 2 H2O + NO
- Ag + two HNOiii (hot and concentrated) → AgNO3 + H2O + NO2
The construction of silver nitrate has been examined by X-ray crystallography several times. In the common orthorhombic class stable at ordinary temperature and force per unit area, the silver atoms grade pairs with Ag---Ag contacts of 3.227 Å. Each Ag+ heart is bonded to vi oxygen centers of both uni- and bidentate nitrate ligands. The Ag-O distances range from 2.384 to 2.702 Å.[4]
Reactions [edit]
A typical reaction with silver nitrate is to suspend a rod of copper in a solution of silvery nitrate and get out information technology for a few hours. The argent nitrate reacts with copper to form hairlike crystals of argent metallic and a blue solution of copper nitrate:
- 2 AgNO3 + Cu → Cu(NOthree)two + ii Ag
Silver nitrate decomposes when heated:
- 2 AgNO3(l) → 2 Ag(south) + O2(m) + 2 NOii(m)
Qualitatively, decomposition is negligible below the melting point, but becomes appreciable around 250 °C and fully decomposes at 440 °C.[nine]
Most metal nitrates thermally decompose to the corresponding oxides, simply silver oxide decomposes at a lower temperature than silver nitrate, so the decomposition of silverish nitrate yields elemental silver instead.
Uses [edit]
Precursor to other silver compounds [edit]
Silver nitrate is the least expensive common salt of silver; it offers several other advantages every bit well. It is non-hygroscopic, in contrast to silver fluoroborate and silver perchlorate. It is relatively stable to calorie-free. Finally, it dissolves in numerous solvents, including water. The nitrate can exist easily replaced by other ligands, rendering AgNOthree versatile. Handling with solutions of halide ions gives a precipitate of AgX (Ten = Cl, Br, I). When making photographic film, silverish nitrate is treated with halide salts of sodium or potassium to form insoluble silver halide in situ in photographic gelatin, which is then applied to strips of tri-acetate or polyester. Similarly, silver nitrate is used to prepare some silverish-based explosives, such as the fulminate, azide, or acetylide, through a precipitation reaction.
Treatment of silvery nitrate with base gives dark grey silver oxide:[10]
- 2 AgNO3 + 2 NaOH → Ag2O + 2 NaNOthree + HtwoO
Halide abstraction [edit]
The silver cation, Ag +
, reacts rapidly with halide sources to produce the insoluble silver halide, which is a cream precipitate if Br −
is used, a white precipitate if Cl −
is used and a yellow precipitate if I −
is used. This reaction is commonly used in inorganic chemistry to abstract halides:
- Ag +
(aq) + X −
(aq) → AgX(south)
where X −
= Cl −
, Br −
, or I −
.
Other silver salts with not-coordinating anions, namely silver tetrafluoroborate and silverish hexafluorophosphate are used for more enervating applications.
Similarly, this reaction is used in analytical chemistry to confirm the presence of chloride, bromide, or iodide ions. Samples are typically acidified with dilute nitric acid to remove interfering ions, due east.g. carbonate ions and sulfide ions. This step avoids confusion of argent sulfide or silverish carbonate precipitates with that of silvery halides. The color of precipitate varies with the halide: white (silvery chloride), pale yellow/cream (argent bromide), xanthous (silver iodide). AgBr and especially AgI photo-decompose to the metal, as testify by a grayish color on exposed samples.
The aforementioned reaction was used on steamships in order to make up one's mind whether or not boiler feedwater had been contaminated with seawater. It is still used to make up one's mind if moisture on formerly dry cargo is a consequence of condensation from boiling air, or from seawater leaking through the hull.[11]
Organic synthesis [edit]
Silver nitrate is used in many ways in organic synthesis, e.g. for deprotection and oxidations. Ag +
binds alkenes reversibly, and silvery nitrate has been used to split up mixtures of alkenes by selective absorption. The resulting adduct can be decomposed with ammonia to release the gratis alkene.[12] Silver nitrate is highly soluble in water but is poorly soluble in nigh organic solvents, except acetonitrile (111.8 m/100 thou, 25 °C).[13]
Biology [edit]
In histology, silver nitrate is used for silver staining, for demonstrating reticular fibers, proteins and nucleic acids. For this reason it is also used to demonstrate proteins in Page gels. Information technology can exist used as a stain in scanning electron microscopy.[14]
Enduring ink [edit]
Argent nitrate produces long-lasting stain when practical to skin. An electoral stain makes utilize of this to mark a finger of people who take voted in an election, assuasive easy identification to prevent double-voting.
Medicine [edit]
Silverish salts accept clarified properties. In 1881 Credé introduced the use of dilute solutions of AgNO3 in newborn babies' eyes at nativity to prevent wrinkle of gonorrhea from the mother, which could crusade blindness. (Mod antibiotics are at present used instead).[fifteen] [16] [17]
Fused silver nitrate, shaped into sticks, was traditionally called "lunar caustic". It is used as a cauterizing agent, for example to remove granulation tissue around a stoma. General Sir James Abbott noted in his journals that in India in 1827 it was infused by a British surgeon into wounds in his arm resulting from the seize with teeth of a mad dog to cauterize the wounds and prevent the onset of rabies.[18]
Silver nitrate is used to cauterize superficial claret vessels in the nose to help foreclose nose bleeds.
Dentists sometimes utilize silver nitrate-infused swabs to heal oral ulcers. Silverish nitrate is used by some podiatrists to impale cells located in the nail bed.
The Canadian medico C. A. Douglas Ringrose researched the employ of silverish nitrate for sterilization procedures, believing that silvery nitrate could exist used to block and corrode the fallopian tubes.[19] The technique was ineffective.[20]
Disinfection [edit]
Much research has been done in evaluating the ability of the silvery ion at inactivating Escherichia coli, a microorganism commonly used as an indicator for fecal contamination and equally a surrogate for pathogens in drinking water treatment. Concentrations of silver nitrate evaluated in inactivation experiments range from 10–200 micrograms per liter as Ag+. Silvery'due south antimicrobial activity saw many applications prior to the discovery of mod antibiotics, when it cruel into near disuse. Its association with argyria fabricated consumers wary and led them to turn away from it when given an alternative.
Against warts [edit]
Peel stained by silver nitrate
Repeated daily awarding of silver nitrate can induce adequate destruction of cutaneous warts, but occasionally pigmented scars may develop. In a placebo-controlled study of 70 patients, silver nitrate given over nine days resulted in clearance of all warts in 43% and improvement in warts in 26% one calendar month later treatment compared to 11% and 14%, respectively, in the placebo group.[21]
Prophylactic [edit]
Equally an oxidant, silvery nitrate should be properly stored away from organic compounds. Despite its common usage in extremely depression concentrations to forestall gonorrhea and command olfactory organ bleeds, silvery nitrate is still very toxic and corrosive.[22] Brief exposure will not produce any firsthand side effects other than the majestic, chocolate-brown or black stains on the peel, but upon constant exposure to high concentrations, side effects will exist noticeable, which include burns. Long-term exposure may crusade center impairment. Silver nitrate is known to be a peel and eye irritant. Silver nitrate has not been thoroughly investigated for potential carcinogenic consequence.[23]
Silverish nitrate is currently unregulated in h2o sources past the United States Environmental Protection Agency. Nonetheless, if more than 1 gram of silver is accumulated in the body, a condition called argyria may develop. Argyria is a permanent corrective condition in which the pare and internal organs plough a bluish-gray colour. The United states of america Ecology Protection Agency used to have a maximum contaminant limit for silvery in water until 1990, when it was determined that argyria did not impact the office of any affected organs despite the discolouration.[24] Argyria is more oft associated with the consumption of colloidal silver solutions rather than with silver nitrate, since information technology is only used at extremely low concentrations to disinfect the water. However, it is nevertheless of import to be wary before ingesting any sort of silver-ion solution.
References [edit]
- ^ a b c d e f g h Lide, David R., ed. (2009). CRC Handbook of Chemistry and Physics (90th ed.). Boca Raton, Florida: CRC Press. ISBN978-1-4200-9084-0.
- ^ a b c d Seidell, Atherton; Linke, William F. (1919). Solubilities of Inorganic and Organic Compounds (2nd ed.). New York City: D. Van Nostrand Company. pp. 617–619.
- ^ a b c d Kiper, Ruslan Anatolievich. "silver nitrate". Chemister.ru . Retrieved 2014-07-xx .
- ^ a b c d e f Meyer, P.; Rimsky, A.; Chevalier, R. (1978). "Construction du nitrate d'argent à pression et température ordinaires. Exemple de cristal parfait". Acta Crystallogr. B. 34 (v): 1457–1462. doi:10.1107/S0567740878005907.
- ^ a b c Sigma-Aldrich Co., Silver nitrate. Retrieved on 2014-07-20.
- ^ "Silver (metallic dust and soluble compounds, as Ag)". Immediately Dangerous to Life or Health Concentrations (IDLH). National Found for Occupational Safety and Health (NIOSH).
- ^ "Definition of Lunar Caustic". lexicon.die.net. Archived from the original on 2012-01-31.
- ^ Szabadváry, Ferenc (1992). History of analytical chemistry. Taylor & Francis. p. 17. ISBN978-2-88124-569-v.
- ^ Stern, One thousand. H. (1972). "High Temperature Properties and Decomposition of Inorganic Salts Part 3, Nitrates and Nitrites". Journal of Physical and Chemic Reference Information. 1 (3): 747–772. Bibcode:1972JPCRD...1..747S. doi:10.1063/i.3253104. S2CID 95532988.
- ^ Campaigne, East.; LeSuer, West. M. (1963). "3-Thiophenecarboxylic (Thenoic) Acid". Organic Syntheses.
{{cite journal}}: CS1 maint: multiple names: authors list (link); Commonage Volume, vol. 4, p. 919 (preparation of AgiiO, used in oxidation of an aldehyde) - ^ "Silvery nitrate method". Transport Data Service. Gesamtverband der Deutschen Versicherungswirtschaf. Retrieved 22 June 2015.
- ^ Cope, A. C.; Bach, R. D. (1973). "trans-Cyclooctene". Organic Syntheses.
{{cite periodical}}: CS1 maint: multiple names: authors list (link); Collective Book, vol. 5, p. 315 - ^ "silver nitrate". chemister.ru . Retrieved 2019-04-04 .
- ^ Geissinger HD (2011). "The use of argent nitrate as a stain for scanning electron microscopy of arterial intima and paraffin sections of kidney". Journal of Microscopy. 95 (3): 471–481. doi:x.1111/j.1365-2818.1972.tb01051.ten. PMID 4114959. S2CID 38335416.
- ^ Peter.H (2000). "Dr Carl Credé (1819–1892) and the prevention of ophthalmia neonatorum". Arch Dis Child Fetal Neonatal Ed. 83 (ii): F158–F159. doi:x.1136/fn.83.2.F158. PMC1721147. PMID 10952715.
- ^ Credé C. Southward. E. (1881). "Die Verhürtung der Augenentzündung der Neugeborenen". Archiv für Gynäkologie. 17 (one): 50–53. doi:10.1007/BF01977793. S2CID 10053605.
- ^ Schaller, Ulrich C. & Klauss, Volker (2001). "Is Credés prophylaxis for ophthalmia neonatorum still valid?". Message of the Globe Health Organization. 79 (3): 262–266. PMC2566367. PMID 11285676.
- ^ British Library, India Office Records, European Manuscripts, MSS EUR F171/33/iii, page 109.
- ^ Ringrose CA. (1973). "Office tubal sterilization". Obstetrics and Gynecology. 42 (1): 151–five. PMID 4720201.
- ^ Cryderman five. Ringrose (1978), 89 D.L.R. (3d) 32 (Alta S.C.) and Zimmer et al. five. Ringrose (1981) four Due west.Westward.R. 75 (Alta C.A.).
- ^ Sterling, J. C.; Handfield-Jones, Due south.; Hudson, P. M.; British Association of Dermatologists (2001). "Guidelines for the direction of cutaneous warts" (PDF). British Journal of Dermatology. 144 (1): 4–11. doi:10.1046/j.1365-2133.2001.04066.x. PMID 11167676. S2CID 20179474. Archived from the original (PDF) on 2012-03-03.
- ^ "Safety data for silver nitrate (MSDS)". Oxford University Chemistry department.
- ^ "New Jersey Correct-To-Know-Deed Hazardous Substance Fact Canvas - Silver Nitrate" (PDF).
- ^ "Silver Compounds." Encyclopedia of Chemical Technology. Vol. 22. Quaternary Ed. Excec. Ed. Jaqueline I. Kroschwitz. New York: John Wiley and Sons, 1997.
External links [edit]
- International Chemic Safety Card 1116
- NIOSH Pocket Guide to Chemical Hazards
- History of Kodak: About Film and Imaging
Molar Mass Of Silver Nitrate,
Source: https://en.wikipedia.org/wiki/Silver_nitrate
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