出典(authority):フリー百科事典『ウィキペディア(Wikipedia)』「2015/04/25 23:25:58」(JST)
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Names | |||
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Other names
Potassium chlorate(VII); Perchloric acid, potassium salt; peroidin
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Identifiers | |||
CAS Registry Number
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7778-74-7 Y | ||
ChEMBL | ChEMBL1200696 N | ||
ChemSpider | 22913 Y | ||
EC number | 231-912-9 | ||
InChI
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Jmol-3D images | Image | ||
PubChem | 516900 | ||
RTECS number | SC9700000 | ||
SMILES
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UNII | 42255P5X4D Y | ||
UN number | 1489 | ||
Properties | |||
Molecular formula
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ClKO4 | ||
Molar mass | 138.55 g·mol−1 | ||
Appearance | colourless/ white crystalline powder | ||
Density | 2.5239 g/cm3 | ||
Melting point | 610 °C (1,130 °F; 883 K) decomposes from 400 °C[4][5] |
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Solubility in water
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0.76 g/100 mL (0 °C) 1.5 g/100 mL (25 °C)[1] |
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Solubility product (Ksp)
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1.05·10−2[3] | ||
Solubility | negligible in alcohol insoluble in ether |
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Solubility in ethanol | 47 mg/kg (0 °C) 120 mg/kg (25 °C)[2] |
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Solubility in acetone | 1.6 g/kg[2] | ||
Solubility in ethyl acetate | 15 mg/kg[2] | ||
Refractive index (nD)
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1.4724 | ||
Structure | |||
Crystal structure | Rhombohedral | ||
Thermochemistry | |||
Specific
heat capacity (C) |
111.35 J/mol·K[6] | ||
Std molar
entropy (S |
150.86 J/mol·K[6] | ||
Std enthalpy of
formation (ΔfH |
-433 kJ/mol[7] | ||
Gibbs free energy (ΔfG˚)
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-300.4 kJ/mol[2] | ||
Hazards | |||
MSDS | MSDS | ||
GHS pictograms | [5] | ||
GHS signal word | Danger | ||
GHS hazard statements
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H271, H302[5] | ||
GHS precautionary statements
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P220[5] | ||
EU Index | 017-008-00-5 | ||
EU classification | O Xn | ||
R-phrases | R9, R22 | ||
S-phrases | (S2), S13, S22, S27 | ||
NFPA 704 |
0
1
1
OX
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Related compounds | |||
Other anions
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Potassium chloride Potassium chlorate |
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Other cations
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Ammonium perchlorate Sodium perchlorate |
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Except where noted otherwise, data is given for materials in their standard state (at 25 °C (77 °F), 100 kPa)
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N verify (what is: Y/N?) | |||
Infobox references | |||
Potassium perchlorate is the inorganic salt with the chemical formula KClO4. Like other perchlorates, this salt is a strong oxidizer although it usually reacts very slowly with organic substances. This usually obtained as a colorless, crystalline solid is a common oxidizer used in fireworks, ammunition percussion caps, explosive primers, and is used variously in propellants, flash compositions, stars, and sparklers. It has been used as a solid rocket propellant, although in that application it has mostly been replaced by the higher performance ammonium perchlorate. KClO4 has the lowest solubility of the alkali metal perchlorates (1.5 g in 100 mL of water at 25 °C).[1]
KClO4 is prepared industrially by treating an aqueous solution of sodium perchlorate with KCl. This single precipitation reaction exploits the low solubility of KClO4, which is about 100 times less than the solubility of NaClO4 (209.6 g/100 mL at 25 °C).[8] It can also be produced by the reaction of perchloric acid with potassium hydroxide, however this is not used widely, due to the dangers of perchloric acid.
KClO4 is an oxidizer in the sense that it exothermically transfers oxygen to combustible materials, greatly increasing their rate of combustion relative to that in air. Thus, with glucose it gives carbon dioxide:
The conversion of solid glucose into hot gaseous CO2 is the basis of the explosive force of this and other such mixtures. Even with cane sugar, KClO4 yields a low explosive, provided the necessary confinement. Otherwise such mixtures simply deflagrate with an intense purple flame characteristic of potassium. Flash compositions used in firecrackers usually consist of fine aluminium powder mixed with potassium perchlorate.
As an oxidizer, potassium perchlorate can be used safely in the presence of sulfur, whereas potassium chlorate cannot. The greater reactivity of chlorate is typical – perchlorates are kinetically poorer oxidants. Chlorate produces chloric acid, which is highly unstable and can lead to premature ignition of the composition. Correspondingly, perchloric acid is quite stable.[9]
Potassium perchlorate can be used as an antithyroid agent used to treat hyperthyroidism, usually in combination with one other medication. This application exploits the similar ionic radii and hydrophilicity of perchlorate and iodide.
Since 2005, a cartridge with potassium perchlorate mixed with anthracene and sulfur is used for generating the black smoke signalling the failure of reaching a two-thirds majority needed for the election of new pope by a papal conclave.
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(help)Wikimedia Commons has media related to Potassium perchlorate. |
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HClO4 | He | ||||||||||||||||||
LiClO4 | Be(ClO4)2 | B(ClO4)4− | ROClO3 | N(ClO4)3 NH4ClO4 |
O | FClO4 | Ne | ||||||||||||
NaClO4 | Mg(ClO4)2 | Al(ClO4)3 | Si | P | S | ClO4− ClOClO3 |
Ar | ||||||||||||
KClO4 | Ca(ClO4)2 | Sc(ClO4)3 | Ti(ClO4)4 | VO(ClO4)3 | Cr(ClO4)3 | Mn(ClO4)2 | Fe(ClO4)3 | Co(ClO4)2, Co(ClO4)3 |
Ni(ClO4)2 | Cu(ClO4)2 | Zn(ClO4)2 | Ga(ClO4)3 | Ge | As | Se | Br | Kr | ||
RbClO4 | Sr(ClO4)2 | Y | Zr | Nb | Mo | Tc | Ru | Rh | Pd(ClO4)2 | AgClO4 | Cd(ClO4)2 | In | Sn | Sb | Te | I | Xe | ||
CsClO4 | Ba(ClO4)2 | Hf | Ta | W | Re | Os | Ir | Pt | Au | Hg2(ClO4)2, Hg(ClO4)2 |
Tl(ClO4)3 | Pb(ClO4)2 | Bi(ClO4)3 | Po | At | Rn | |||
Fr | Ra | Rf | Db | Sg | Bh | Hs | Mt | Ds | Rg | Cn | Uut | Fl | Uup | Lv | Uus | Uuo | |||
↓ | |||||||||||||||||||
La | Ce(ClO4)x | Pr | Nd | Pm | Sm | Eu | Gd | Tb | Dy | Ho | Er | Tm | Yb | Lu | |||||
Ac | Th | Pa | UO2(ClO4)2 | Np | Pu | Am | Cm | Bk | Cf | Es | Fm | Md | No | Lr |
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関連記事 | 「perchlorate」 |
過塩素酸、(化合物)過塩素酸塩
.