Difference between revisions of "Potassium hexachlorostannate"
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| − | Potassium hexachlorostannate (IV) | + | {{Stub}} |
| + | {{Chembox | ||
| + | | Name = Potassium hexachlorostannate | ||
| + | | Reference = | ||
| + | | IUPACName = Potassium hexachlorostannate(IV) | ||
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| + | <!-- Sections --> | ||
| + | | Section1 = {{Chembox Identifiers | ||
| + | | 3DMet = | ||
| + | | Abbreviations = | ||
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| + | }} | ||
| + | | Section2 = {{Chembox Properties | ||
| + | | AtmosphericOHRateConstant = | ||
| + | | Appearance = White solid | ||
| + | | BoilingPt = | ||
| + | | BoilingPtC = 520 | ||
| + | | BoilingPt_ref = | ||
| + | | BoilingPt_notes = Decomposes | ||
| + | | Density = 2.719 g/cm<sup>3</sup><ref>Vogt, K.; Reichardt, W.; Prandl, W.; Haussuehl, S.; Physica Status Solidi A: Applied Research; vol. 57; (1980); p. K145 - K148</ref> | ||
| + | | Formula = K<sub>2</sub>SnCl<sub>6</sub> | ||
| + | | HenryConstant = | ||
| + | | LogP = | ||
| + | | MolarMass = 409.605 g/mol | ||
| + | | MeltingPt = | ||
| + | | MeltingPtC = 300 | ||
| + | | MeltingPt_ref = | ||
| + | | MeltingPt_notes = (decomposes) | ||
| + | | pKa = | ||
| + | | pKb = | ||
| + | | Solubility = Soluble | ||
| + | | SolubleOther = Soluble in liq. [[ammonia|NH<sub>3</sub>]]<br>Insoluble in [[acetonitrile]], conc. [[hydrochloric acid|HCl]], [[Tin(IV) chloride|SnCl<sub>4</sub>]] | ||
| + | | Solvent = | ||
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| + | | Section3 = {{Chembox Structure | ||
| + | | Coordination = | ||
| + | | CrystalStruct = Cubic | ||
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| + | | Section4 = {{Chembox Thermochemistry | ||
| + | | DeltaGf = | ||
| + | | DeltaHc = | ||
| + | | DeltaHf = -1,483.8 kJ/kmol | ||
| + | | Entropy = | ||
| + | | HeatCapacity = 221.2 J·mol<sup>-1</sup>·K<sup>-1</sup> | ||
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| + | | Section5 = {{Chembox Explosive | ||
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| + | | REFactor = | ||
| + | }} | ||
| + | | Section6 = {{Chembox Hazards | ||
| + | | AutoignitionPt = Non-flammable | ||
| + | | ExploLimits = Non-explosive | ||
| + | | ExternalMSDS = None | ||
| + | | FlashPt = Non-flammable | ||
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| + | | MainHazards = Harmful | ||
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| + | | OtherAnions = | ||
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| + | | OtherFunction = | ||
| + | | OtherFunction_label = | ||
| + | | OtherCompounds = [[Ammonium hexachlorostannate]] | ||
| + | }} | ||
| + | }} | ||
| + | '''Potassium hexachlorostannate''' is an inorganic chemical compound with the chemical formula '''K<sub>2</sub>SnCl<sub>6</sub>''', used mainly for obtaining [[tin(IV) chloride]]. | ||
| − | + | ==Properties== | |
| + | ===Chemical=== | ||
| + | Potassium hexachlorostannate is the salt of a strong acid and its solutions react neutral in water. Addition of alkali or ammonia solution precipitates Sn(OH)<sub>4</sub>·nH<sub>2</sub>O. Further addition of strong alkali causes soluble stannate (K<sub>2</sub>Sn(OH)<sub>6</sub>) to form. | ||
| − | 3 Sn<sup>4+</sup>(aq) + 18 HCl(aq) | + | On strong heating (> 300 °C, est.) it releases SnCl<sub>4</sub> (b.p. 114.15 °C), so it affords a chlorine-free route to this useful chemical. The ammonium salt sublimes completely. |
| + | |||
| + | ===Physical=== | ||
| + | Potassium hexachlorostannate is a colorless crystalline solid. | ||
| + | |||
| + | It is insoluble in 37 w% HCl which offers an easy method of purifying the salt. | ||
| + | |||
| + | In literature, there are multiple values given for the melting and decomposition point of this compound: 409 °C<ref>Yu, Jiang-Tsu; Wu, Ching-Jiun; Lou, Ssu-Hao; Tsai, Mei-Na; Journal of Solid State Chemistry; vol. 98; (1992); p. 159 - 173</ref>, 470 °C<ref>Janiak; Nikel; Blazejowski; Journal of thermal analysis; vol. 36; nb. 6; (1990); p. 2205 - 2210</ref>, 520 °C<ref>Volkov, V. V.; Myakishev, K. G.; Solomatina, L. Ya.; Russian Journal of Inorganic Chemistry (Translation of Zhurnal Neorganicheskoi Khimii); vol. 40; (1995); p. 1559 - 1562;</ref>, 760 °C<ref>Zalewicz, Malgorzata; Thermochimica Acta; vol. 116; (1987); p. 217 - 224</ref> | ||
| + | |||
| + | ==Availability== | ||
| + | It is not sold by most chemical entities and has to be prepared. | ||
| + | |||
| + | ==Preparation== | ||
| + | Potassium hexachlorostannate (IV) is prepared by dissolving [[tin]] metal (or pewter) in a mixture of [[nitric acid]] and [[hydrochloric acid]] ([[aqua regia]]). More or less stoichiometric amounts of the acids can be used in accordance with: | ||
| + | |||
| + | :3 Sn(s) + 4 NO<sub>3</sub><sup>-</sup>(aq) + 16 H<sup>+</sup>(aq) → 3 Sn<sup>4+</sup>(aq) + 4 NO(g) + 8 H<sub>2</sub>O(l) | ||
| + | |||
| + | :3 Sn<sup>4+</sup>(aq) + 18 HCl(aq) → 3 SnCl<sub>6</sub><sup>2-</sup>(aq) + 18 H<sup>+</sup>(aq) | ||
Dissolution is very swift and does not usually require heating. | Dissolution is very swift and does not usually require heating. | ||
| − | Once complete the solution is brought to a gentle simmer and solid KCl is added, 2 mol per mol of tin. The mixture is then simmered and stirred until all the KCl is dissolved, then allowed to cool naturally, then further chilled on ice bath, e.g. overnight. | + | Once complete the solution is brought to a gentle simmer and solid [[Potassium chloride|KCl]] is added, 2 mol per mol of tin. The mixture is then simmered and stirred until all the KCl is dissolved, then allowed to cool naturally, then further chilled on ice bath, e.g. overnight. |
Well-formed crystals of K<sub>2</sub>SnCl<sub>6</sub> are obtained. | Well-formed crystals of K<sub>2</sub>SnCl<sub>6</sub> are obtained. | ||
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The salts can also be obtained by oxidation of an SnCl<sub>2</sub> solution in HCl, with hydrogen peroxide or nitric acid as oxidiser. Add KCl (or NH<sub>4</sub>Cl) as per above. | The salts can also be obtained by oxidation of an SnCl<sub>2</sub> solution in HCl, with hydrogen peroxide or nitric acid as oxidiser. Add KCl (or NH<sub>4</sub>Cl) as per above. | ||
| − | + | ==Projects== | |
| + | *Make tin(IV) chloride | ||
| − | + | ==Handling== | |
| + | ===Safety=== | ||
| + | Potassium hexachlorostannate may be corrosive and should be handled with proper protection | ||
| + | |||
| + | ===Storage=== | ||
| + | In closed containers. | ||
| + | |||
| + | ===Disposal=== | ||
| + | Should be disposed like any other tin compound. | ||
| − | + | ==References== | |
| + | <references/> | ||
| + | ===Relevant Sciencemadness threads=== | ||
[[Category:Chemical compounds]] | [[Category:Chemical compounds]] | ||
Latest revision as of 18:27, 13 November 2018
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|
| Names | |
|---|---|
| IUPAC name
Potassium hexachlorostannate(IV)
| |
| Properties | |
| K2SnCl6 | |
| Molar mass | 409.605 g/mol |
| Appearance | White solid |
| Density | 2.719 g/cm3[1] |
| Melting point | 300 °C (572 °F; 573 K) (decomposes) |
| Boiling point | 520 °C (968 °F; 793 K) Decomposes |
| Soluble | |
| Solubility | Soluble in liq. NH3 Insoluble in acetonitrile, conc. HCl, SnCl4 |
| Thermochemistry | |
| Std enthalpy of
formation (ΔfH |
-1,483.8 kJ/kmol |
| Hazards | |
| Safety data sheet | None |
| Flash point | Non-flammable |
| Related compounds | |
| Related compounds
|
Ammonium hexachlorostannate |
| Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa). | |
| Infobox references | |
Potassium hexachlorostannate is an inorganic chemical compound with the chemical formula K2SnCl6, used mainly for obtaining tin(IV) chloride.
Contents
Properties
Chemical
Potassium hexachlorostannate is the salt of a strong acid and its solutions react neutral in water. Addition of alkali or ammonia solution precipitates Sn(OH)4·nH2O. Further addition of strong alkali causes soluble stannate (K2Sn(OH)6) to form.
On strong heating (> 300 °C, est.) it releases SnCl4 (b.p. 114.15 °C), so it affords a chlorine-free route to this useful chemical. The ammonium salt sublimes completely.
Physical
Potassium hexachlorostannate is a colorless crystalline solid.
It is insoluble in 37 w% HCl which offers an easy method of purifying the salt.
In literature, there are multiple values given for the melting and decomposition point of this compound: 409 °C[2], 470 °C[3], 520 °C[4], 760 °C[5]
Availability
It is not sold by most chemical entities and has to be prepared.
Preparation
Potassium hexachlorostannate (IV) is prepared by dissolving tin metal (or pewter) in a mixture of nitric acid and hydrochloric acid (aqua regia). More or less stoichiometric amounts of the acids can be used in accordance with:
- 3 Sn(s) + 4 NO3-(aq) + 16 H+(aq) → 3 Sn4+(aq) + 4 NO(g) + 8 H2O(l)
- 3 Sn4+(aq) + 18 HCl(aq) → 3 SnCl62-(aq) + 18 H+(aq)
Dissolution is very swift and does not usually require heating.
Once complete the solution is brought to a gentle simmer and solid KCl is added, 2 mol per mol of tin. The mixture is then simmered and stirred until all the KCl is dissolved, then allowed to cool naturally, then further chilled on ice bath, e.g. overnight.
Well-formed crystals of K2SnCl6 are obtained.
Ammonium hexachlorostannate is obtained in identical conditions but by replacing KCl with NH4Cl.
Instead of pure tin, pewter (Sn/Sb alloy) can also be used because the corresponding Sb salt, KSbCl6 is very soluble even at low temperature and simply stays in solution.
The salts can also be obtained by oxidation of an SnCl2 solution in HCl, with hydrogen peroxide or nitric acid as oxidiser. Add KCl (or NH4Cl) as per above.
Projects
- Make tin(IV) chloride
Handling
Safety
Potassium hexachlorostannate may be corrosive and should be handled with proper protection
Storage
In closed containers.
Disposal
Should be disposed like any other tin compound.
References
- ↑ Vogt, K.; Reichardt, W.; Prandl, W.; Haussuehl, S.; Physica Status Solidi A: Applied Research; vol. 57; (1980); p. K145 - K148
- ↑ Yu, Jiang-Tsu; Wu, Ching-Jiun; Lou, Ssu-Hao; Tsai, Mei-Na; Journal of Solid State Chemistry; vol. 98; (1992); p. 159 - 173
- ↑ Janiak; Nikel; Blazejowski; Journal of thermal analysis; vol. 36; nb. 6; (1990); p. 2205 - 2210
- ↑ Volkov, V. V.; Myakishev, K. G.; Solomatina, L. Ya.; Russian Journal of Inorganic Chemistry (Translation of Zhurnal Neorganicheskoi Khimii); vol. 40; (1995); p. 1559 - 1562;
- ↑ Zalewicz, Malgorzata; Thermochimica Acta; vol. 116; (1987); p. 217 - 224
