Silver nitrate

Last updated
Silver nitrate
Silver-nitrate-2D.svg
Silver nitrate crystals.jpg
Silver-nitrate-xtal-2x2x2-c-3D-bs-17.png
Names
IUPAC name
Silver nitrate
Systematic IUPAC name
Silver(I) nitrate
Other names
Nitric acid silver(1+) salt
Lapis infernalis
Argentous nitrate
Identifiers
3D model (JSmol)
ChEBI
ChEMBL
ChemSpider
ECHA InfoCard 100.028.958 OOjs UI icon edit-ltr-progressive.svg
EC Number
  • 231-853-9
PubChem CID
RTECS number
  • VW4725000
UNII
UN number 1493
  • InChI=1S/Ag.NO3/c;2-1(3)4/q+1;-1 Yes check.svgY
    Key: SQGYOTSLMSWVJD-UHFFFAOYSA-N Yes check.svgY
  • InChI=1/Ag.NO3/c;2-1(3)4/q+1;-1
    Key: SQGYOTSLMSWVJD-UHFFFAOYAW
  • [N+](=O)([O-])[O-].[Ag+]
Properties
AgNO3
Molar mass 169.872 g·mol−1
Appearancecolorless solid
Odor Odorless
Density 4.35 g/cm3 (24 °C)
3.97 g/cm3 (210 °C) [1]
Melting point 209.7 °C (409.5 °F; 482.8 K) [1] [2]
Boiling point 440 °C (824 °F; 713 K)
decomposes [1]
122 g/100 mL (0 °C)
170 g/100 mL (10 °C)
256 g/100 mL (25 °C)
373 g/100 mL (40 °C)
912 g/100 mL (100 °C) [3]
Solubility Soluble in acetone, [1] ammonia, ether, glycerol
Solubility in acetic acid 0.776 g/kg (30 °C)
1.244 g/kg (40 °C)
5.503 g/kg (93 °C) [2]
Solubility in acetone 0.35 g/100 g (14 °C)
0.44 g/100 g (18 °C) [3]
Solubility in benzene 0.22 g/kg (35 °C)
0.44 g/kg (40.5 °C) [3]
Solubility in ethanol 3.1 g/100 g (19 °C) [3]
Solubility in ethyl acetate 2.7 g/100 g (20 °C) [2]
log P 0.19
−45.7·10−6 cm3/mol
1.744
Viscosity 3.77 cP (244 °C)
3.04 cP (275 °C) [2]
Structure
Orthorhombic, oP56 [4]
P212121, No. 19 [4]
222 [4]
a = 6.992(2) Å, b = 7.335(2) Å, c = 10.125(2) Å [4]
α = 90°, β = 90°, γ = 90°
Thermochemistry
93.1 J/mol·K [1]
Std molar
entropy (S⦵298)
140.9 J/mol·K [1]
−124.4 kJ/mol [1]
−33.4 kJ/mol [1]
Pharmacology
D08AL01 ( WHO )
Hazards
Occupational safety and health (OHS/OSH):
Main hazards
Reacts explosively with ethanol. Toxic. Corrosive.
GHS labelling:
GHS-pictogram-rondflam.svg GHS-pictogram-acid.svg GHS-pictogram-skull.svg GHS-pictogram-pollu.svg [5]
Danger
H272, H314, H410 [5]
P220, P273, P280, P305+P351+P338, P310, P501 [5]
NFPA 704 (fire diamond)
NFPA 704.svgHealth 3: Short exposure could cause serious temporary or residual injury. E.g. chlorine gasFlammability 0: Will not burn. E.g. waterInstability 2: Undergoes violent chemical change at elevated temperatures and pressures, reacts violently with water, or may form explosive mixtures with water. E.g. white phosphorusSpecial hazard OX: Oxidizer. E.g. potassium perchlorate
3
0
2
OX
Lethal dose or concentration (LD, LC):
800 mg/kg (rabbit, oral)
20 mg/kg (dog, oral) [6]
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
Yes check.svgY  verify  (what is  Yes check.svgYX mark.svgN ?)
Crystals of silver nitrate under a microscope. AgNO3 microscope 2.JPG
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 silver compounds, such as those used in photography. It is far less sensitive to light than the halides. It was once called lunar caustic because silver was called luna by ancient alchemists who associated silver with the moon. [7] In solid silver nitrate, the silver ions are three-coordinated in a trigonal planar arrangement. [4]

Contents

Synthesis and structure

Albertus Magnus, in the 13th century, documented the ability of nitric acid to separate gold and silver by dissolving the silver. [8] Indeed silver nitrate can be prepared by dissolving silver in nitric acid followed by 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 + 2 HNO3 (hot and concentrated) → AgNO3 + H2O + NO2

The structure of silver nitrate has been examined by X-ray crystallography several times. In the common orthorhombic form stable at ordinary temperature and pressure, the silver atoms form pairs with Ag---Ag contacts of 3.227 Å. Each Ag+ center is bonded to six oxygen centers of both uni- and bidentate nitrate ligands. The Ag-O distances range from 2.384 to 2.702 Å. [4]

Silver-nitrate-xtal-Ag-coordination-3D-bs-17.png

Reactions

A typical reaction with silver nitrate is to suspend a rod of copper in a solution of silver nitrate and leave it for a few hours. The silver nitrate reacts with copper to form hairlike crystals of silver metal and a blue solution of copper nitrate:

2 AgNO3 + Cu → Cu(NO3)2 + 2 Ag

Silver nitrate decomposes when heated:

2 AgNO3(l) → 2 Ag(s) + O2(g) + 2 NO2(g)

Qualitatively, decomposition is negligible below the melting point, but becomes appreciable around 250 °C and fully decomposes at 440 °C. [9]

Most metal nitrates thermally decompose to the respective oxides, but silver oxide decomposes at a lower temperature than silver nitrate, so the decomposition of silver nitrate yields elemental silver instead.

Uses

Precursor to other silver compounds

Silver nitrate is the least expensive salt of silver; it offers several other advantages as well. It is non-hygroscopic, in contrast to silver fluoroborate and silver perchlorate. In addition, it is relatively stable to light, and it dissolves in numerous solvents, including water. The nitrate can be easily replaced by other ligands, rendering AgNO3 versatile. Treatment with solutions of halide ions gives a precipitate of AgX (X = Cl, Br, I). When making photographic film, silver 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 silver-based explosives, such as the fulminate, azide, or acetylide, through a precipitation reaction.

Treatment of silver nitrate with base gives dark grey silver oxide: [10]

2 AgNO3 + 2 NaOH → Ag2O + 2 NaNO3 + H2O

Halide abstraction

The silver cation, Ag+
, reacts quickly 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(s)

where X−
 = Cl−
, Br−
, or I−
.

Other silver salts with non-coordinating anions, namely silver tetrafluoroborate and silver hexafluorophosphate are used for more demanding 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, e.g. carbonate ions and sulfide ions. This step avoids confusion of silver sulfide or silver carbonate precipitates with that of silver halides. The color of precipitate varies with the halide: white (silver chloride), pale yellow/cream (silver bromide), yellow (silver iodide). AgBr and especially AgI photo-decompose to the metal, as evidenced by a grayish color on exposed samples.

The same reaction was used on steamships in order to determine whether or not boiler feedwater had been contaminated with seawater. It is still used to determine if moisture on formerly dry cargo is a result of condensation from humid air, or from seawater leaking through the hull. [11]

Organic synthesis

Silver nitrate is used in many ways in organic synthesis, e.g. for deprotection and oxidations. Ag+
 binds alkenes reversibly, and silver nitrate has been used to separate mixtures of alkenes by selective absorption. The resulting adduct can be decomposed with ammonia to release the free alkene. [12] Silver nitrate is highly soluble in water but is poorly soluble in most organic solvents, except acetonitrile (111.8 g/100 g, 25 °C). [13]

Biology

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. It can be used as a stain in scanning electron microscopy. [14]

Indelible ink

Silver nitrate produces long-lasting stain when applied to skin and is one of the ink’s ingredients. An electoral stain makes use of this to mark a finger of people who have voted in an election, allowing easy identification to prevent double-voting. [15] [16]

Medicine

Micrograph showing a silver nitrate (brown) marked surgical margin. Atypical leiomyoma intermed mag.jpg
Micrograph showing a silver nitrate (brown) marked surgical margin.

Silver salts have antiseptic properties. In 1881 Credé introduced the use of dilute solutions of AgNO3 in newborn babies' eyes at birth to prevent contraction of gonorrhea from the mother, which could cause blindness. (Modern antibiotics are now used instead). [17] [18] [19]

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 bite of a mad dog to cauterize the wounds and prevent the onset of rabies. [20]

Silver nitrate is used to cauterize superficial blood vessels in the nose to help prevent nosebleeds.

Dentists sometimes use silver nitrate-infused swabs to heal oral ulcers. Silver nitrate is used by some podiatrists to kill cells located in the nail bed.

The Canadian physician C. A. Douglas Ringrose researched the use of silver nitrate for sterilization procedures, believing that silver nitrate could be used to block and corrode the fallopian tubes. [21] The technique was ineffective. [22]

Disinfection

Much research has been done in evaluating the ability of the silver ion at inactivating Escherichia coli , a microorganism commonly used as an indicator for fecal contamination and as 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+. Silver's antimicrobial activity saw many applications prior to the discovery of modern antibiotics, when it fell into near disuse. Its association with argyria made consumers wary and led them to turn away from it when given an alternative.[ citation needed ]

Against warts

Skin stained by silver nitrate Silver nitrate stains.jpg
Skin stained by silver nitrate

Repeated daily application 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 month after treatment compared to 11% and 14%, respectively, in the placebo group. [23]

Safety

As an oxidant, silver nitrate should be properly stored away from organic compounds. Despite its common usage in extremely low concentrations to prevent gonorrhea and control nosebleeds, silver nitrate is still very toxic and corrosive. [24] Brief exposure will not produce any immediate side effects other than the purple, brown or black stains on the skin, but upon constant exposure to high concentrations, side effects will be noticeable, which include burns. Long-term exposure may cause eye damage. Silver nitrate is known to be a skin and eye irritant. Silver nitrate has not been thoroughly investigated for potential carcinogenic effect. [25]

Silver nitrate is currently unregulated in water sources by the United States Environmental Protection Agency. However, if more than 1 gram of silver is accumulated in the body, a condition called argyria may develop. Argyria is a permanent cosmetic condition in which the skin and internal organs turn a blue-gray color. The United States Environmental Protection Agency used to have a maximum contaminant limit for silver in water until 1990, when it was determined that argyria did not impact the function of any affected organs despite the discolouration. [26] Argyria is more often associated with the consumption of colloidal silver solutions rather than with silver nitrate, since it is only used at extremely low concentrations to disinfect the water. However, it is still important to be wary before ingesting any sort of silver-ion solution.

Related Research Articles

<span class="mw-page-title-main">Nitric acid</span> Highly corrosive mineral acid

Nitric acid is the inorganic compound with the formula HNO3. It is a highly corrosive mineral acid. The compound is colorless, but samples tend to acquire a yellow cast over time due to decomposition into oxides of nitrogen. Most commercially available nitric acid has a concentration of 68% in water. When the solution contains more than 86% HNO3, it is referred to as fuming nitric acid. Depending on the amount of nitrogen dioxide present, fuming nitric acid is further characterized as red fuming nitric acid at concentrations above 86%, or white fuming nitric acid at concentrations above 95%.

<span class="mw-page-title-main">Silver</span> Chemical element, symbol Ag and atomic number 47

Silver is a chemical element; it has symbol Ag ) and atomic number 47. A soft, white, lustrous transition metal, it exhibits the highest electrical conductivity, thermal conductivity, and reflectivity of any metal. The metal is found in the Earth's crust in the pure, free elemental form, as an alloy with gold and other metals, and in minerals such as argentite and chlorargyrite. Most silver is produced as a byproduct of copper, gold, lead, and zinc refining.

The term chloride refers to a compound or molecule that contains either a chlorine ion, which is a negatively charged chlorine atom, or a non-charged chlorine atom covalently bonded to the rest of the molecule by a single bond. Many inorganic chlorides are salts. Many organic compounds are chlorides. The pronunciation of the word "chloride" is.

In chemistry, a halide is a binary chemical compound, of which one part is a halogen atom and the other part is an element or radical that is less electronegative than the halogen, to make a fluoride, chloride, bromide, iodide, astatide, or theoretically tennesside compound. The alkali metals combine directly with halogens under appropriate conditions forming halides of the general formula, MX. Many salts are halides; the hal- syllable in halide and halite reflects this correlation. All Group 1 metals form halides that are white solids at room temperature.

<span class="mw-page-title-main">Dinitrogen pentoxide</span> Chemical compound

Dinitrogen pentoxide is the chemical compound with the formula N2O5. It is one of the binary nitrogen oxides, a family of compounds that only contain nitrogen and oxygen. It exists as colourless crystals that sublime slightly above room temperature, yielding a colorless gas.

<span class="mw-page-title-main">Silver chloride</span> Chemical compound with the formula AgCl

Silver chloride is an inorganic chemical compound with the chemical formula AgCl. This white crystalline solid is well known for its low solubility in water and its sensitivity to light. Upon illumination or heating, silver chloride converts to silver, which is signaled by grey to black or purplish coloration in some samples. AgCl occurs naturally as the mineral chlorargyrite.

<span class="mw-page-title-main">Tollens' reagent</span> Chemical reagent used to distinguish between aldehydes and ketones

Tollens' reagent is a chemical reagent used to distinguish between aldehydes and ketones along with some alpha-hydroxy ketones which can tautomerize into aldehydes. The reagent consists of a solution of silver nitrate, ammonium hydroxide and some sodium hydroxide. It was named after its discoverer, the German chemist Bernhard Tollens. A positive test with Tollens' reagent is indicated by the precipitation of elemental silver, often producing a characteristic "silver mirror" on the inner surface of the reaction vessel.

<span class="mw-page-title-main">Uranyl nitrate</span> Chemical compound

Uranyl nitrate is a water-soluble yellow uranium salt with the formula UO2(NO3)2 · n H2O. The hexa-, tri-, and dihydrates are known. The compound is mainly of interest because it is an intermediate in the preparation of nuclear fuels. In the nuclear industry, it is commonly referred to as yellow salt.

A salt metathesis reaction is a chemical process involving the exchange of bonds between two reacting chemical species which results in the creation of products with similar or identical bonding affiliations. This reaction is represented by the general scheme:

<span class="mw-page-title-main">Silver chromate</span> Chemical compound

Silver chromate is an inorganic compound with formula Ag2CrO4 which appears as distinctively coloured brown-red crystals. The compound is insoluble and its precipitation is indicative of the reaction between soluble chromate and silver precursor salts (commonly potassium/sodium chromate with silver nitrate). This reaction is important for two uses in the laboratory: in analytical chemistry it constitutes the basis for the Mohr method of argentometry, whereas in neuroscience it is used in the Golgi method of staining neurons for microscopy.

A nitrate test is a chemical test used to determine the presence of nitrate ion in solution. Testing for the presence of nitrate via wet chemistry is generally difficult compared with testing for other anions, as almost all nitrates are soluble in water. In contrast, many common ions give insoluble salts, e.g. halides precipitate with silver, and sulfate precipitate with barium.

<span class="mw-page-title-main">Iron(III) nitrate</span> Chemical compound

Iron(III) nitrate, or ferric nitrate, is the name used for a series of inorganic compounds with the formula Fe(NO3)3.(H2O)n. Most common is the nonahydrate Fe(NO3)3.(H2O)9. The hydrates are all pale colored, water-soluble paramagnetic salts.

The chemical element nitrogen is one of the most abundant elements in the universe and can form many compounds. It can take several oxidation states; but the most common oxidation states are -3 and +3. Nitrogen can form nitride and nitrate ions. It also forms a part of nitric acid and nitrate salts. Nitrogen compounds also have an important role in organic chemistry, as nitrogen is part of proteins, amino acids and adenosine triphosphate.

<span class="mw-page-title-main">Silver compounds</span> Chemical compounds containing silver

Silver is a relatively unreactive metal, although it can form several compounds. The common oxidation states of silver are (in order of commonness): +1 (the most stable state; for example, silver nitrate, AgNO3); +2 (highly oxidising; for example, silver(II) fluoride, AgF2); and even very rarely +3 (extreme oxidising; for example, potassium tetrafluoroargentate(III), KAgF4). The +3 state requires very strong oxidising agents to attain, such as fluorine or peroxodisulfate, and some silver(III) compounds react with atmospheric moisture and attack glass. Indeed, silver(III) fluoride is usually obtained by reacting silver or silver monofluoride with the strongest known oxidizing agent, krypton difluoride.

<span class="mw-page-title-main">Bromous acid</span> Chemical compound

Bromous acid is the inorganic compound with the formula of HBrO2. It is an unstable compound, although salts of its conjugate base – bromites – have been isolated. In acidic solution, bromites decompose to bromine.

<span class="mw-page-title-main">Lead compounds</span> Type of compound

Compounds of lead exist with lead in two main oxidation states: +2 and +4. The former is more common. Inorganic lead(IV) compounds are typically strong oxidants or exist only in highly acidic solutions.

<span class="mw-page-title-main">Thorium(IV) nitrate</span> Chemical compound

Thorium(IV) nitrate is a chemical compound, a salt of thorium and nitric acid with the formula Th(NO3)4. A white solid in its anhydrous form, it can form tetra- and pentahydrates. As a salt of thorium it is weakly radioactive.

Silver hyponitrite is an ionic compound with formula Ag2N2O2 or (Ag+
)2[ON=NO]2−, containing monovalent silver cations and hyponitrite anions. It is a bright yellow solid practically insoluble in water and most organic solvents, including DMF and DMSO.

<span class="mw-page-title-main">Iron(II) nitrate</span> Chemical compound

Iron(II) nitrate is the nitrate salt of iron(II). It is commonly encountered as the green hexahydrate, Fe(NO3)2·6H2O, which is a metal aquo complex, however it is not commercially available unlike iron(III) nitrate due to its instability to air. The salt is soluble in water serves as a ready source of ferrous ions.

<span class="mw-page-title-main">Bismuthyl (ion)</span> Chemical compound

Bismuthyl — inorganic oxygen-containing singly charged ion with the chemical formula BiO+, is an oxycation of bismuth in the +3 oxidation state. Most often it is formed during the hydrolysis of trivalent bismuth salts, primarily nitrate, chloride and other halides. In chemical compounds, bismuthyl plays the role of a monovalent cation.

References

  1. 1 2 3 4 5 6 7 8 Lide, David R., ed. (2009). CRC Handbook of Chemistry and Physics (90th ed.). Boca Raton, Florida: CRC Press. ISBN   978-1-4200-9084-0.
  2. 1 2 3 4 Kiper, Ruslan Anatolievich. "silver nitrate". Chemister.ru. Retrieved 2014-07-20.
  3. 1 2 3 4 Seidell, Atherton; Linke, William F. (1919). Solubilities of Inorganic and Organic Compounds (2nd ed.). New York City: D. Van Nostrand Company. pp.  617–619.
  4. 1 2 3 4 5 6 Meyer, P.; Rimsky, A.; Chevalier, R. (1978). "Structure du nitrate d'argent à pression et température ordinaires. Exemple de cristal parfait". Acta Crystallogr. B . 34 (5): 1457–1462. Bibcode:1978AcCrB..34.1457M. doi:10.1107/S0567740878005907.
  5. 1 2 3 Sigma-Aldrich Co., Silver nitrate. Retrieved on 2014-07-20.
  6. ↑ "Silver (metal dust and soluble compounds, as Ag)". Immediately Dangerous to Life or Health Concentrations (IDLH). National Institute for Occupational Safety and Health (NIOSH).
  7. ↑ "Definition of Lunar Caustic". dictionary.die.net. Archived from the original on 2012-01-31.
  8. ↑ Szabadváry, Ferenc (1992). History of analytical chemistry. Taylor & Francis. p. 17. ISBN   978-2-88124-569-5.
  9. ↑ Stern, K. H. (1972). "High Temperature Properties and Decomposition of Inorganic Salts Part 3, Nitrates and Nitrites". Journal of Physical and Chemical Reference Data. 1 (3): 747–772. Bibcode:1972JPCRD...1..747S. doi:10.1063/1.3253104. S2CID   95532988.
  10. ↑ Campaigne, E.; LeSuer, W. M. (1963). "3-Thiophenecarboxylic (Thenoic) Acid". Organic Syntheses {{cite journal}}: CS1 maint: multiple names: authors list (link); Collected Volumes, vol. 4, p. 919. (preparation of Ag2O, used in oxidation of an aldehyde)
  11. ↑ "Silver nitrate method". Transport Information Service. Gesamtverband der Deutschen Versicherungswirtschaf. Retrieved 22 June 2015.
  12. ↑ Cope, A. C.; Bach, R. D. (1973). "trans-Cyclooctene". Organic Syntheses {{cite journal}}: CS1 maint: multiple names: authors list (link); Collected Volumes, vol. 5, p. 315.
  13. ↑ "silver nitrate". chemister.ru. Retrieved 2019-04-04.
  14. ↑ Geissinger HD (2011). "The use of silver nitrate as a stain for scanning electron microscopy of arterial intima and paraffin sections of kidney". Journal of Microscopy. 95 (3): 471–481. doi:10.1111/j.1365-2818.1972.tb01051.x. PMID   4114959. S2CID   38335416.
  15. ↑ "The ink with a 'secret formula' that powers the world's biggest democratic exercise | India | The Guardian". web.archive.org. 2023-06-17. Retrieved 2024-04-17.
  16. ↑ Dhillon, Amrit (2019-03-28). "The ink with a 'secret formula' that powers the world's biggest democratic exercise". The Guardian. ISSN   0261-3077 . Retrieved 2024-04-17.
  17. ↑ Peter.H (2000). "Dr Carl Credé (1819–1892) and the prevention of ophthalmia neonatorum". Arch Dis Child Fetal Neonatal Ed. 83 (2): F158–F159. doi:10.1136/fn.83.2.F158. PMC   1721147 . PMID   10952715.
  18. ↑ Credé C. S. E. (1881). "Die Verhürtung der Augenentzündung der Neugeborenen". Archiv für Gynäkologie. 17 (1): 50–53. doi:10.1007/BF01977793. S2CID   10053605.
  19. ↑ Schaller, Ulrich C. & Klauss, Volker (2001). "Is Credés prophylaxis for ophthalmia neonatorum still valid?". Bulletin of the World Health Organization. 79 (3): 262–266. PMC   2566367 . PMID   11285676.
  20. ↑ British Library, India Office Records, European Manuscripts, MSS EUR F171/33/3, page 109.
  21. ↑ Ringrose CA. (1973). "Office tubal sterilization". Obstetrics and Gynecology. 42 (1): 151–5. PMID   4720201.
  22. ↑ Cryderman v. Ringrose (1978), 89 D.L.R. (3d) 32 (Alta S.C.) and Zimmer et al. v. Ringrose (1981) 4 W.W.R. 75 (Alta C.A.).
  23. ↑ Sterling, J. C.; Handfield-Jones, S.; Hudson, P. M.; British Association of Dermatologists (2001). "Guidelines for the management 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.
  24. ↑ "Safety data for silver nitrate (MSDS)". Oxford University Chemistry department. Archived from the original on 2011-12-02. Retrieved 2008-03-25.
  25. ↑ "New Jersey Right-To-Know-Act Hazardous Substance Fact Sheet - Silver Nitrate" (PDF).
  26. ↑ "Silver Compounds." Encyclopedia of Chemical Technology. Vol. 22. Fourth Ed. Excec. Ed. Jaqueline I. Kroschwitz. New York: John Wiley and Sons, 1997.
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