Indium(III) sulfate

Last updated
Indium(III) sulfate
Names
Other names
Indium sulfate
Identifiers
3D model (JSmol)
ChemSpider
ECHA InfoCard 100.033.340 OOjs UI icon edit-ltr-progressive.svg
EC Number
  • 236-689-1
PubChem CID
RTECS number
  • NL1925000
UNII
  • InChI=1S/2In.3H2O4S/c;;3*1-5(2,3)4/h;;3*(H2,1,2,3,4)/q2*+3;;;/p-6 Yes check.svgY
    Key: XGCKLPDYTQRDTR-UHFFFAOYSA-H Yes check.svgY
  • InChI=1/2In.3H2O4S/c;;3*1-5(2,3)4/h;;3*(H2,1,2,3,4)/q2*+3;;;/p-6
    Key: XGCKLPDYTQRDTR-CYFPFDDLAA
  • [In+3].[In+3].[O-]S(=O)(=O)[O-].[O-]S([O-])(=O)=O.[O-]S([O-])(=O)=O
Properties
In2(SO4)3
Molar mass 517.81 g/mol
Appearancewhite-gray odorless powder, hygroscopic, monoclinic crystals
Density 3.44 g/cm3, solid
Melting point decomposes at 600 °C [1]
soluble, (539.2 g/L at 20 °C) [2]
Structure
monoclinic (room temperature)
P121
a = 8.57 Å [3] , b = 8.908 Å, c = 14.66 Å
α = 90°, β = 124.72°, γ = 90°
Structure
rhombohedral
R-3
a = 8.44 Å [3] [4] , b = 8.44 Å, c = 23.093 Å
α = 90°, β = 90°, γ = 120°
6 formula per cell
Thermochemistry
0.129 [5]
Hazards
GHS labelling:
GHS-pictogram-exclam.svg
Warning
H315, H319, H335
P261, P264, P271, P280, P302+P352, P304+P340, P305+P351+P338, P312, P321, P332+P313, P337+P313, P362, P403+P233, P405, P501
NFPA 704 (fire diamond)
[6]
2
0
0
0.1 [7] (TWA), 0.3 [7] (STEL)
NIOSH (US health exposure limits):
PEL (Permissible)
0.1 [7]
Safety data sheet (SDS) tttmetalpowder
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 ?)

Indium(III) sulfate (In2(SO4)3) is a sulfate salt of the metal indium. It is a sesquisulfate, meaning that the sulfate group occurs 11/2 times as much as the metal. It may be formed by the reaction of indium, its oxide, or its carbonate with sulfuric acid. An excess of strong acid is required, otherwise insoluble basic salts are formed. [8] As a solid indium sulfate can be anhydrous, or take the form of a pentahydrate with five water molecules [9] or a nonahydrate with nine molecules of water. Indium sulfate is used in the production of indium or indium containing substances. Indium sulfate also can be found in basic salts, acidic salts or double salts including indium alum.

Contents

Properties

In water solution, the indium ion forms a complex with water and sulfate, examples being In(H2O)5(SO4)+ and In(H2O)4(SO4)2−. [10] [11] Indium is unusual in forming a sulfate complex. The effect on the sulfate ion is revealed in the Raman spectrum. [8] The proportion of sulfate complex increases with temperature showing the reaction that forms it is endothermic. The proportion also increases with concentration of the solution and can be over a half. [12] The sulfate complex rapidly exchanges with water at a rate of over 10,000,000 per second, so that NMR cannot detect the difference that results from a complexed and noncomplexed indium ion. [12] An indium sulfate water solution is quite acidic with a 0.14 mol/liter solution having a pH of 1.85. If the pH rises above 3.4 then a precipitate will form. [13]

The Raman spectrum of the solution shows lines at 650, 1000 and 1125 cm−1 due to a sulfur–oxygen bonds in sulfate bound to indium. A line at 255 cm−1 is due to the indium-oxygen bond to the sulfate. The water attached to the indium atom causes a band at about 400 cm−1. [8]

Solid anhydrous indium sulfate has two crystalline forms. When formed by chlorine gas chemical transport at 848 K, it has a monoclinic form with unit cell dimensions a = 8.570 Å, b = 8.908 Å and c = 12.0521 Å, β = 91.05°, and four formulae per cell. A high temperature form deposited at 973K has a hexagonal (or rhombohedral) form with cell dimensions of a = 8.440 Å, c = 23.093 Å and six formulae per cell. [14]

During extraction of indium, a sulfate solution of mixed metals, including indium sulfate, has trivalent metals partitioned into a kerosene solution of di-2-ethylhexyl hydrogen phosphate. Isododecylphosphetanic and diisooctylphosphinic acids can also be used for this function. The kerosene mixture is then backwashed with an acid to recover the metals in a water solution and regenerate the extracting fluid. [15]

Production

Indium metal reacts with cold concentrated sulfuric acid to produce Indium sulfate and hydrogen gas. If hot concentrated sulfuric acid is used indium will reduce the sulfuric acid to sulfur dioxide. [16]

Indium sulfate can also be produced from a reaction of sulfuric acid on indium oxide, indium carbonate, or indium hydroxide.

Reactions

When heated to 710 K (437 °C) or above, indium sulfate decomposes by giving off sulfur trioxide vapour, yielding indium oxide. [17]

Alkalis added to indium sulfate solutions precipitate basic salts. For example, potassium hydroxide produces either a basic sulfate, 2In2O3.SO3·nH2O, or KIn3(OH)6(SO4)2 depending on pH. [18] Sodium pyrophosphate causes a slimy precipitate of indium pyrophosphate, In4(P2O7)3·3H2O. Potassium periodate causes a precipitate of a basic indium periodate, 2InO5·In(OH)3·6H2O . [19] Oxalic acid causes a precipitate of indium oxalate, In2(C2O4)3·10H2O. Alkali oxalates cause a precipitate of the alkali dioxalatoindate to form MIn(C2O4)2·3H2O, where M = Na, K or NH4. [20]

Hydrogen sulfates

An acid sulfate, indium hydrogensulfate tetrahydrate with the formula HIn(SO4)2·4H2O crystallises in the orthorhombic system with unit cell dimensions a = 9.997 Å, b = 5.477 Å, c = 18.44 Å, with four of the formula per cell. The density is 2.50 cm−3. In the acid sulfate, two water molecules are linked to the indium atom and a hydronium ion H5O2 takes care of the proton. This is part of an acid sulfate family that includes Al, Ga, In, Tl(III), Fe(III) and Ti(III). HIn(SO4)2 is made by evaporating an indium sulfate in 40% sulfuric acid solution [21] or cooling indium sulfate in a 60% sulfuric acid solution. [22] As the acid tetrahydrate is heated it gives off water yielding a trihydrate, monohydrate, and an anhydrous form at 370, 385 and 482K. Above 505K it gives out more water and sulfur dioxide yielding the neutral indium sulfate. [22] Indium hydrogensulfate is a proton conductor with conductivity 0.0002Ω−1cm−1. [22]

Basic sulfates

A basic indium sulfate is made by adding ethanol to a water solution of indium sulfate. Crystals can be formed by using a 0.05 molar solution with twice the volume of ethanol, and waiting for several weeks for crystals to form. [23] InOHSO4·(H2O)2 has monoclinic crystals with a=6.06 Å b=7.89 Å c=12.66 Å and β=107.5°. Cell volume is 577.6 Å3. [23] Another basic indium sulfate InOHSO4 with rhombohedral crystals is made by heating an indium sulfate solution at 160 °C or over for about a week in a sealed tube. [24] This insoluble basic salt also forms if indium sulfate solution is diluted below 0.005 molar. So a precipitate forms from diluted solutions as well as from heated solutions. [12]

Anhydrous double sulfates

Two different types of anhydrous double indium sulfates have been made. One is from the family MI
3MIII(XO4)3, with MI being a large singly positive ion such as K, Rb, Cs, Tl or NH3; MIII is triply charged and can be Al, Ga, In, Tl, V, Cr, Fe, Sc and other rare earths; and X is S or Se. [25] Most of these have a rhombohedral crystal structure. However, triammonium indium trisulfate, (NH4)3In(SO4)3 converts from rhombohedral to monoclinic as the temperature drops below 80 °C, and converts back into a rhombohedral form with space group R3c as the temperature rises above 110 °C. [25] The low temperature monoclinic form has space group P21/c, a=8.96, b=15.64 c=9.13 β=108.28° Z=4 [25] The high temperature form is termed "β-". An explanation for this transition is that ammonium (and also thallium) is a non-spherical ion and thus has lower symmetry. However, when it is heated enough, dynamical disorder causing random orientations makes the ions on average spherically symmetric. Alkali metal ions are spherical in shape at all temperatures and form rhombohedral structures. [25] Double sulfates of this form exist of indium with the alkali metals sodium, potassium, rubidium, and cesium. These can be formed by heating a solid mixture of the individual sulfates to 350 °C. [9]

nameformulamolecular weighta Åc Åαvolume Å3density
trisodium indium trisulfate471.9713.9708.771109°00′4943.172
tripotassium indium trisulfate520.3014.8628.960109°45′5713.026
trirubidium indium trisulfate659.4115.4139.136110°03′6263.498
tricesium indium trisulfate801.7216.0689.211110°36′6873.876
triammonium indium trisulfate361.0615.5319.163120°1914.11.88
ammonium indium disulfate324.984.9028.70373.643171.273.15
rubidium indium disulfate392.414.9088.786273.781173.503.75
cesium indium disulfate439.854.9569.256774.473187.263.90
thallium indium disulfate511.334.9198.788273.748174.274.87

Another series of anhydrous rhombohedral double salts in the same series of TlFe(SO4)2 exists. These can be made by heating a mixture of anhydrous sulfates at 350 °C, or by dehydrating hydrous double alum type salts at 300 °C. The substances in this series are RbIn(SO4)2, CsIn(SO4)2, TlIn(SO4)2 and NH4In(SO4)2. Although KIn(SO4)2 exists it has a different crystalline form. [26]

Hydrated double sulfates

Hydrated double salts of indium in an alum structure exist with formula MIIn(SO4)2·12H2O. All alums have a cubic crystal structure with space group Pa3. [27] The indium cesium alum CsIn(SO4)2•12H2O [12] has formula weight 656.0, unit cell width 12.54 Å, cell volume 1972 Å3 and density 2.20 g/cm3. [27] It has the β alum structure. [28] The cesium alum can be used in the analysis of indium. It precipitates when cesium nitrate is added to indium sulfate solution with extra sulfuric acid added. [29]

Indium ammonium alum NH4In(SO4)2·12H2O [30] is fairly unstable at room temperature and must be crystallised below 5 °C. [31] It decomposes at 36 °C to a tetrahydrate. [32] It changes to a ferroelectric phase below 127K. [33] The alum methyl ammonium indium sulfate dodecahydrate CH3NH3In(SO4)2·12H2O becomes ferroelectric below 164K. [34] Potassium indium alum has not been crystallised. [35] Rubidum indium alum is highly efflorescent very easily losing its water. [36]

Another series of monoclinic hydrated double salts have four water molecules MIn(SO4)2·4H2O, with five formulae per unit cell, where M is NH4, K or Rb and the point group is P21/c. The prototype substance for the series is (NH4)Sm(SO4)2(H2O)4.

formulaweighta Åb Åc Åβvolume Å3densityref
NH4In(SO4)2•4H2O397.0410.65110.7459.279102.67°1036.083.182 [37]
KIn(SO4)2•4H2O418.1010.58110.6419.224101.93°1016.13.416 [38]
RbIn(SO4)2•4H2O464.4710.65110.7459.279102.67°1036.13.722 [39]

Cadmium can also form a double sulfate, Cd3In2(SO4)6·26H2O. [40]

Crystals with less water also exist like KIn(SO4)2·H2O. [41]

Organic double sulfates

Organic base double sulfates of indium include the guanidinium salt [C(NH2)3][In(H2O)2(SO4)2], which crystallises in a monoclinic system with space group P21/c a = 4.769 Å, b = 20.416 Å, c = 10.445 Å, β = 93.39°, cell volume 1015.3 Å3, 4 formulas per cell and density 2.637. [H2(4,4'-bi-py)][In2(H2O)6(SO4)4]·2H2O crystallises in the triclinic system with a = 7.143 Å, b = 7.798 Å, c = 12.580 Å, α = 107.61°, β = 98.79°, γ = 93.89°, cell volume 655.2 Å3, one formula per cell and density 2.322. [42] [H(2,2'-bipy)][In(H2O)(SO4)2]·2H2O, the hexamethylenediamine salt [H3N(CH2)6NH3][In(H2O)2(SO4)2]2·2H2O and [H2(Py(CH2)3Py)][In(H2O)2(SO4)2]2·2H2O also exist. [42] Yet other organic derivatives include those of triethylenetetramine, [43] and amylammonium. [30] Tri-μ-sulfato-κ6O:O'-bis[aqua(1,10-phenanthroline-κ2N,N')indium(III)] dihydrate, [In2(SO4)3(C12H8N2)2(H2O)2]·2H2O, has a 1,10-phenanthroline molecule linked to each indium ion. Two indium ions are linked via three sulfate groups. It forms triclinic crystals with two formulas per unit cell. The density is 2.097 g/cm3. [44]

Dimethylindium sulfate [(CH3)2In]2SO4 can be made by reacting trimethylindium with dry sulfuric acid. [45]

Mixed

A double indium sulfate chloride salt has formula In2(SO4)3·InCl3·(17±1)H2O. [46]

Monovalent

Indium(I) sulfate, In2SO4 can be made in a solid state by heating indium metal with indium(III) sulfate, [47] but when dissolving in water or sulfuric acid, In+ reacts to produce hydrogen gas. [48] The mixed valence salt InIInIII(SO4)2 is also made by heating indium metal with indium(III) sulfate. [49]

Use

Philco surface-barrier transistor developed and produced in 1953 Philco Surface Barrier transistor=1953.jpg
Philco surface-barrier transistor developed and produced in 1953

Indium sulfate is a commercially available chemical. It can be used to electroplate indium metal, [50] as a hardening agent in gold electroplating [51] or to prepare other indium containing substances such as copper indium selenide. It has been sold as a health supplement, even though there is no evidence of benefit to humans, and it is toxic. [52]

The first high-frequency transistor was the surface-barrier germanium transistor developed by Philco in 1953, capable of operating up to 60 MHz. [53] These were made by etching depressions into an N-type germanium base from both sides with jets of indium sulfate until it was a few ten-thousandths of an inch thick. Indium electroplated into the depressions formed the collector and emitter. [54] [55]

Related Research Articles

In chemistry, a salt is a chemical compound consisting of an ionic assembly of positively charged cations and negatively charged anions, which results in a compound with no net electric charge. A common example is table salt, with positively charged sodium ions and negatively charged chloride ions.

<span class="mw-page-title-main">Alum</span> Family of double sulfate salts of aluminium

An alum is a type of chemical compound, usually a hydrated double sulfate salt of aluminium with the general formula XAl(SO
4)
2·12 H
2O, where X is a monovalent cation such as potassium or ammonium. By itself, "alum" often refers to potassium alum, with the formula KAl(SO
4)
2·12 H
2O. Other alums are named after the monovalent ion, such as sodium alum and ammonium alum.

<span class="mw-page-title-main">Sulfate</span> Oxyanion with a central atom of sulfur surrounded by 4 oxygen atoms

The sulfate or sulphate ion is a polyatomic anion with the empirical formula SO2−4. Salts, acid derivatives, and peroxides of sulfate are widely used in industry. Sulfates occur widely in everyday life. Sulfates are salts of sulfuric acid and many are prepared from that acid.

<span class="mw-page-title-main">Zinc sulfate</span> Chemical compound

Zinc sulfate describes a family of inorganic compounds with the formula ZnSO4(H2O)x. All are colorless solids. The most common form includes water of crystallization as the heptahydrate, with the formula ZnSO4·7H2O. It was historically known as "white vitriol". Zinc sulfate and its hydrates are colourless solids.

<span class="mw-page-title-main">Sodium sulfate</span> Chemical compound with formula Na2SO4

Sodium sulfate (also known as sodium sulphate or sulfate of soda) is the inorganic compound with formula Na2SO4 as well as several related hydrates. All forms are white solids that are highly soluble in water. With an annual production of 6 million tonnes, the decahydrate is a major commodity chemical product. It is mainly used as a filler in the manufacture of powdered home laundry detergents and in the Kraft process of paper pulping for making highly alkaline sulfides.

<span class="mw-page-title-main">Hypochlorite</span> Ion

In chemistry, hypochlorite is an anion with the chemical formula ClO−. It combines with a number of cations to form hypochlorite salts. Common examples include sodium hypochlorite and calcium hypochlorite. The Cl-O distance in ClO− is 1.69 Å.

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

Cerium(IV) sulfate, also called ceric sulfate, is an inorganic compound. It exists as the anhydrous salt Ce(SO4)2 as well as a few hydrated forms: Ce(SO4)2(H2O)x, with x equal to 4, 8, or 12. These salts are yellow to yellow/orange solids that are moderately soluble in water and dilute acids. Its neutral solutions slowly decompose, depositing the light yellow oxide CeO2. Solutions of ceric sulfate have a strong yellow color. The tetrahydrate loses water when heated to 180-200 °C.

<span class="mw-page-title-main">Ammonium sulfate</span> Chemical compound

Ammonium sulfate (American English and international scientific usage; ammonium sulphate in British English); (NH4)2SO4, is an inorganic salt with a number of commercial uses. The most common use is as a soil fertilizer. It contains 21% nitrogen and 24% sulfur.

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

Sulfamic acid, also known as amidosulfonic acid, amidosulfuric acid, aminosulfonic acid, sulphamic acid and sulfamidic acid, is a molecular compound with the formula H3NSO3. This colourless, water-soluble compound finds many applications. Sulfamic acid melts at 205 °C before decomposing at higher temperatures to water, sulfur trioxide, sulfur dioxide and nitrogen.

<span class="mw-page-title-main">Aluminium sulfate</span> Chemical compound

Aluminium sulfate is a salt with the formula Al2(SO4)3. It is soluble in water and is mainly used as a coagulating agent (promoting particle collision by neutralizing charge) in the purification of drinking water and wastewater treatment plants, and also in paper manufacturing.

Selenic acid is the inorganic compound with the formula H2SeO4. It is an oxoacid of selenium, and its structure is more accurately described as O2Se(OH)2. It is a colorless compound. Although it has few uses, its derivative sodium selenate is used in the production of glass and animal feeds.

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In chemistry, hexol is a cation with formula {[Co(NH3)4(OH)2]3Co}6+ — a coordination complex consisting of four cobalt cations in oxidation state +3, twelve ammonia molecules NH
3, and six hydroxy anions HO−
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<span class="mw-page-title-main">Indium(III) oxide</span> Chemical compound

Indium(III) oxide (In2O3) is a chemical compound, an amphoteric oxide of indium.

<span class="mw-page-title-main">Ammonium iron(II) sulfate</span> Chemical compound

Ammonium iron(II) sulfate, or Mohr's salt, is the inorganic compound with the formula (NH4)2Fe(SO4)2(H2O)6. Containing two different cations, Fe2+ and NH4+, it is classified as a double salt of ferrous sulfate and ammonium sulfate. It is a common laboratory reagent because it is readily crystallized, and crystals resist oxidation by air. Like the other ferrous sulfate salts, ferrous ammonium sulfate dissolves in water to give the aquo complex [Fe(H2O)6]2+, which has octahedral molecular geometry. Its mineral form is mohrite.

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

Chromium(III) sulfate usually refers to the inorganic compounds with the formula Cr2(SO4)3.x(H2O), where x can range from 0 to 18. Additionally, ill-defined but commercially important "basic chromium sulfates" are known. These salts are usually either violet or green solids that are soluble in water. It is commonly used in tanning leather.

<span class="mw-page-title-main">Cobalt(II) sulfate</span> Inorganic compound

Cobalt(II) sulfate is any of the inorganic compounds with the formula CoSO4(H2O)x. Usually cobalt sulfate refers to the hexa- or heptahydrates CoSO4.6H2O or CoSO4.7H2O, respectively. The heptahydrate is a red solid that is soluble in water and methanol. Since cobalt(II) has an odd number of electrons, its salts are paramagnetic.

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

Chromium(II) sulfate refers to inorganic compounds with the chemical formula CrSO4·n H2O. Several closely related hydrated salts are known. The pentahydrate is a blue solid that dissolves readily in water. Solutions of chromium(II) are easily oxidized by air to Cr(III) species. Solutions of Cr(II) are used as specialized reducing agents of value in organic synthesis.

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

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Gallium(III) sulfate refers to the chemical compound, a salt, with the formula Ga2(SO4)3, or its hydrates Ga2(SO4)3·xH2O. Gallium metal dissolves in sulfuric acid to form solutions containing [Ga(OH2)6]3+ and SO42− ions. The octadecahydrate Ga2(SO4)3·18H2O crystallises from these solutions at room temperature. This hydrate loses water in stages when heated, forming the anhydrate Ga2(SO4)3 above 150 °C and completely above 310 °C. Anhydrous Ga2(SO4)3 is isostructural with iron(III) sulfate, crystallizing in the rhombohedral space group R3.

References

  1. ↑ Perry D, Phillips S (1995) Handbook of Inorganic Compounds: Version 2.0, An Electronic Database, CRC Press ISBN   0-8493-8671-3
  2. ↑ Indium Sulfate. Product Data Sheet Archived 10 February 2012 at the Wayback Machine Indium Cooperation
  3. 1 2 Villars, Pierre; Cenzual, Karin; Gladyshevskii, Roman (2015). Handbook of Inorganic Substances 2015. Walter de Gruyter. p. 654. ISBN   9783110311747.
  4. ↑ Pallister, Peter J.; Moudrakovski, Igor L.; Enright, Gary D.; Ripmeester, John A. (2013). "Structural assessment of anhydrous sulfates with high field 33S solid state NMR and first principles calculations". CrystEngComm. 15 (43): 8808. doi:10.1039/C3CE41233D.
  5. ↑ Nilson, L. F.; Pettersson, Otto (1 January 1880). "On the Molecular Heat and Volume of the Rare Earths and Their Sulphates". Proceedings of the Royal Society of London. 31 (206–211): 46–51. Bibcode:1880RSPS...31...46N. doi: 10.1098/rspl.1880.0005 .
  6. ↑ "Sfety Data Sheet Indium sulfate anhydrous 99.99%". Pfaltz & Bauer, Inc.
  7. 1 2 3 Tritrust Industrial C. Ltd. "MSDS OF Indium Sulfate" (PDF). Archived from the original (PDF) on 4 March 2016. Retrieved 31 May 2015.
  8. 1 2 3 Hester, Ronald E.; Plane, Robert A.; Walrafen, George E. (1963). "Raman Spectra of Aqueous Solutions of Indium Sulfate, Nitrate, and Perchlorate". The Journal of Chemical Physics. 38 (1): 249. Bibcode:1963JChPh..38..249H. doi:10.1063/1.1733470.
  9. 1 2 Perret, R; Tudo, J; Jolibois, B; Couchot, P (July 1974). "Préparation et caractérisation cristallographique de quelques sulfates doubles d'indium(III) et de thallium(III), MI3MIII (SO4)3 (MI = Na, K, Rb et Cs)". Journal of the Less Common Metals (in French). 37 (1): 9–12. doi:10.1016/0022-5088(74)90003-4.
  10. ↑ Caminiti, R.; Paschina, G. (September 1981). "An X-ray diffraction study of the structure of the aqua indium(III) ion in indium sulphate solution". Chemical Physics Letters. 82 (3): 487–491. Bibcode:1981CPL....82..487C. doi:10.1016/0009-2614(81)85425-5.
  11. ↑ Cotton, F. Albert; Wilkinson, Geoffrey (1966). Advanced Inorganic Chemistry. John Wiley & Sons. p. 438.
  12. 1 2 3 4 Rudolph, Wolfram W.; Fischer, Dieter; Tomney, Madelaine R.; Pye, Cory C. (2004). "Indium(iii) hydration in aqueous solutions of perchlorate, nitrate and sulfate. Raman and infrared spectroscopic studies and ab-initio molecular orbital calculations of indium(iii)-water clusters". Physical Chemistry Chemical Physics. 6 (22): 5145. Bibcode:2004PCCP....6.5145R. doi:10.1039/b407419j . Retrieved 31 May 2015.
  13. ↑ Busev, A.I. (22 October 2013). The Analytical Chemistry of Indium. Elsevier. p. 30. ISBN   9781483149554.
  14. ↑ Krause, M.; Gruehn, R. (January 1995). "Contributions on the thermal behaviour of sulphates XVII. Single crystal structure refinements of In2(SO4)3 and Ga2(SO4)3". Zeitschrift für Kristallographie. 210 (6): 427–431. Bibcode:1995ZK....210..427K. doi:10.1524/zkri.1995.210.6.427.
  15. ↑ Travkin, V. F.; Kubasov, V. L.; Glubokov, Yu. M.; Busygina, N. S.; Kazanbaev, L. A.; Kozlov, P. A. (October 2004). "Extraction of indium(III) from sulfate solutions with organophosphorus acids". Russian Journal of Applied Chemistry. 77 (10): 1613–1617. doi:10.1007/s11167-005-0082-9. S2CID   94902567.
  16. ↑ Geckler, Robert P.; Marchi, Louis E. (August 1944). "Indium". Journal of Chemical Education. 21 (8): 407. Bibcode:1944JChEd..21..407G. doi:10.1021/ed021p407.
  17. ↑ Zhou, Huijuan; Cai, Weiping; Zhang, Lide (April 1999). "Synthesis and structure of indium oxide nanoparticles dispersed within pores of mesoporous silica". Materials Research Bulletin. 34 (6): 845–849. doi:10.1016/S0025-5408(99)00080-X.
  18. ↑ Grimes, S. M. (1984). "Chapter 4. Al, Ga, In, Tl". Annual Reports on the Progress of Chemistry, Section A. 81: 90. doi:10.1039/IC9848100075.
  19. ↑ Busev, A.I. (22 October 2013). The Analytical Chemistry of Indium. Elsevier. pp. 67–68. ISBN   9781483149554.
  20. ↑ Busev, A.I. (22 October 2013). The Analytical Chemistry of Indium. Elsevier. pp. 111–112. ISBN   9781483149554.
  21. ↑ Tudo, J.; Jolibois, B.; Laplace, G.; Nowogrocki, G.; Abraham, F. (15 July 1979). "Structure cristalline du sulfate acide d'indium(III) hydraté". Acta Crystallographica Section B (in French). 35 (7): 1580–1583. doi:10.1107/s0567740879007172.
  22. 1 2 3 Voropaeva, E. Yu.; Stenina, I. A.; Yaroslavtsev, A. B. (January 2007). "Proton conduction in indium hydrogensulfate and hydrous zirconia composites". Russian Journal of Inorganic Chemistry. 52 (1): 1–6. doi:10.1134/S0036023607010019. S2CID   96716246.
  23. 1 2 Johansson, Georg (1961). "The Crystal Structure of " (PDF). Acta Chemica Scandinavica. 15 (7): 1437–1453. doi: 10.3891/acta.chem.scand.15-1437 . Retrieved 31 May 2015.
  24. ↑ Johansson, Georg (1962). "The Crystal Structure of FeOHSO4 and InOHSO4" (PDF). Acta Chemica Scandinavica. 16 (5): 1234–1244. doi: 10.3891/acta.chem.scand.16-1234 . Retrieved 31 May 2015.
  25. 1 2 3 4 Jolibois, B.; Laplace, G.; Abraham, F.; Nowogrocki, G. (15 November 1980). "The low-temperature forms of some M1/3MIII(XO4)3 compounds: structure of triammonium indium(III) trisulfate". Acta Crystallographica Section B. 36 (11): 2517–2519. doi:10.1107/S0567740880009338.
  26. ↑ Perret, R.; Couchot, P. (June 1972). "Preparation et caracterisation cristallographique des sulfates et seleniates doubles anhydres d'indium M1In(XO4)2". Journal of the Less Common Metals (in French). 27 (3): 333–338. doi:10.1016/0022-5088(72)90065-3.
  27. 1 2 Beattie, James K.; Best, Stephen P.; Skelton, Brian W.; White, Allan H. (1981). "Structural studies on the caesium alums, CsM III [SO4]2•12H2O". Journal of the Chemical Society, Dalton Transactions (10): 2105–2111. doi:10.1039/DT9810002105.
  28. ↑ Armstrong, Robert S.; Berry, Andrew J.; Cole, Bradley D.; Nugent, Kerry W. (1997). "Chromium luminescence as a probe of site effects in the alum lattice". Journal of the Chemical Society, Dalton Transactions (3): 363–366. doi:10.1039/A605705E.
  29. ↑ Busev, A.I. (22 October 2013). The Analytical Chemistry of Indium. Elsevier. p. 5. ISBN   9781483149554.
  30. 1 2 Ekeley, John B.; Potratz, Herbert A. (June 1936). "Some Double Salts of Indium and Organic Bases". Journal of the American Chemical Society. 58 (6): 907–909. doi:10.1021/ja01297a016.
  31. ↑ Fimland, B. O.; Svare, I (1 September 1987). "NMR and dielectric studies of NH4+ motion in some ammonium alums". Physica Scripta. 36 (3): 559–562. Bibcode:1987PhyS...36..559F. doi:10.1088/0031-8949/36/3/031. S2CID   250876849.
  32. ↑ The Encyclopædia Britannica: A Dictionary of Arts, Sciences, and General Literature. Vol. 5. 1888. p. 533. Retrieved 3 June 2015.
  33. ↑ Bailey, W. C.; Story, H. S. (1973). "Nuclear quadrupole coupling of 115In in NH4In(SO4)2•12H2O". The Journal of Chemical Physics. 58 (3): 1255–1256. Bibcode:1973JChPh..58.1255B. doi:10.1063/1.1679317.
  34. ↑ Navalgund, R. R.; Gupta, L. C. (1 September 1975). "EPR of Cr3+ in Methyl Ammonium Indium Sulfate Dodecahydrate". Physica Status Solidi B. 71 (1): K87–K90. Bibcode:1975PSSBR..71...87N. doi:10.1002/pssb.2220710161.
  35. ↑ Purkayastha, B.C.; Das, H.B. (1 February 1963). "A STUDY ON THE PROBABLE EXISTENCE OF POTASSIUM INDIUM ALUM WITH RADIOACTIVE NUCLEI. PART I". Journal of the Indian Chemical Society. 40.
  36. ↑ Ivanovski, Vladimir; Petruševski, Vladimir M.; Šoptrajanov, Bojan (April 1999). "Vibrational spectra of hexaaqua complexes". Vibrational Spectroscopy. 19 (2): 425–429. doi:10.1016/S0924-2031(98)00068-X.
  37. ↑ "inorganic Materials Database". Atom Work. Retrieved 31 May 2015.
  38. ↑ "Inorganic Materials Database". AtomWork. Retrieved 31 May 2015.
  39. ↑ "Inorganic Materials Database". AtomWork. Retrieved 31 May 2015.
  40. ↑ Fedorov, P.I.; Lovetskaya, G.A.; Starikova, Z.A.; Vlaskin, O.I. (November 1983). "[Study of zinc- and cadmium sulfates interaction with indium sulfate in aqueous solution at 25 deg C]". Zhurnal Neorganicheskoj Khimii. 28 (11): 2962–2965.
  41. ↑ Mukhatarova, N. N.; Rastsvetaeva, R. K.; Ilyukhin, V. V.; Belov, N. V. (March 1979). "Crystal structure of KIn(SO4)2·H2O". Soviet Physics Doklady. 24: 140. Bibcode:1979SPhD...24..140M.
  42. 1 2 Petrosyants, S. P.; Ilyukhin, A. B.; Ketsko, V. A. (November 2006). "Supramolecular compounds of indium sulfates with nitrogen-containing cations". Russian Journal of Coordination Chemistry. 32 (11): 777–783. doi:10.1134/s1070328406110029. S2CID   95016069.
  43. ↑ Tian, Zhen-Fen (March 2009). "Solvothermal Synthesis and Characterization of One-dimensional Chained Indium-Sulfate". Chemical Journal of Chinese Universities.
  44. ↑ Shen, Fwu Ming; Lush, Shie Fu (15 September 2010). "Tri-µ-sulfato-κ6O:O'-bis[aqua(1,10-phenanthroline- κ2N,N')indium(III)] dihydrate". Acta Crystallographica Section E. 66 (10): m1260–m1261. doi:10.1107/S1600536810036330. PMC   2983182 . PMID   21587408 . Retrieved 3 June 2015.
  45. ↑ Olapinski, H.; Weidlein, J. (June 1973). "Bis(dialkylmetall)sulfate der elemente gallium, indium und thallium". Journal of Organometallic Chemistry. 54: 87–93. doi:10.1016/s0022-328x(00)84995-5.
  46. ↑ Kartzmark, Elinor M. (August 1977). "Double salts of indium trichloride with the alkali chlorides, with ammonium chloride, and with indium sulfate". Canadian Journal of Chemistry. 55 (15): 2792–2798. doi: 10.1139/v77-388 .
  47. ↑ Dmitriev, V.S.; Malinov, S.A.; Dubovitskaya, L.G.; Smirnov, V.A. (September 1986). "Vzaimodejstvie metallicheskogo indiya s sul'fatom indiya(3)" [Metallic indium interaction with indium(3) sulfate]. Zhurnal Neorganicheskoj Khimii (in Russian). 31 (9): 2372–2377. ISSN   0044-457X.
  48. ↑ Kozin, L.F.; Egorova, A.G. (May 1982). "Sul'fat odnovalentnogo indiya, ego sintez i svojstva" [Monovalent indium sulfate, its synthesis and properties]. Zhurnal Obshchej Khimii (in Russian). 52 (5): 1020–1024. ISSN   0044-460X.
  49. ↑ Downs, A. J. (31 May 1993). Chemistry of Aluminium, Gallium, Indium, and Thallium. Springer. p. 211. ISBN   9780751401035.
  50. ↑ Schwarz-Schampera, Ulrich; Herzig, Peter M. (14 March 2013). Indium: Geology, Mineralogy, and Economics. Springer Science & Business Media. p. 171. ISBN   9783662050767.
  51. ↑ "Indium Corp. In2(SO4)3 Indium Sulfate Anhydrous" . Retrieved 2 June 2015.
  52. ↑ Bradley, David (2 July 2008). "Health Benefits of Indium". Archived from the original on 16 March 2006. Retrieved 2 June 2015.
  53. ↑ Bradley, W.E. (December 1953). "The Surface-Barrier Transistor: Part I-Principles of the Surface-Barrier Transistor". Proceedings of the IRE. 41 (12): 1702–1706. doi:10.1109/JRPROC.1953.274351. S2CID   51652314.
  54. ↑ "Philco Claims Its Transistor Outperforms Others Now In Use". Wall Street Journal. 4 December 1953. p. 4.
  55. ↑ "Electroplated Transistors Announced". Electronics Magazine. January 1954.

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