16871-90-2 Usage
References
[1] W. John Williams, Handbook of Anion Determination, 1979
[2] Ruth Winter, A Consumer's Dictionary of Cosmetic Ingredients, 7th Edition, 2009
[3] B. A. Richardson, Wood Preservation, 2nd Edition, 1993
[4] Werner Vogel, Glass Chemistry, 2nd Edition, 1994
Chemical Properties
White, odorless, crystalline powder. D
3.0. Slightly soluble in water; soluble in hydrochlo-
ric acid.
Uses
Different sources of media describe the Uses of 16871-90-2 differently. You can refer to the following data:
1. In the manufacture of opalescent glass, in porcelain enamels, in insecticides. Also used in aluminum metallurgy.
2. Potassium hexafluorosilicate is used in the production of porceleins. It is also used for the preservation of timber. It is involved in the manufacturing of ceramics, aluminum and magnesium smelting. In addition, it is used as an intermediate in the manufacturing of optical glass.
General Description
A white, odorless crystalline powder. Denser than water. Contact may cause irritation to skin, eyes, and mucous membranes. May be toxic by ingestion. Used to make other chemicals.
Air & Water Reactions
Slightly soluble in water.
Reactivity Profile
Potassium fluorosilicate has weak oxidizing or reducing powers. Redox reactions can however still occur. The majority of compounds in this class are slightly soluble or insoluble in water. If soluble in water, then the solutions are usually neither strongly acidic nor strongly basic. These compounds are not water-reactive.
Hazard
Toxic by ingestion and inhalation, strong
irritant to tissue.
Health Hazard
Highly toxic, may be fatal if inhaled, swallowed or absorbed through skin. Avoid any skin contact. Effects of contact or inhalation may be delayed. Fire may produce irritating, corrosive and/or toxic gases. Runoff from fire control or dilution water may be corrosive and/or toxic and cause pollution.
Fire Hazard
Non-combustible, substance itself does not burn but may decompose upon heating to produce corrosive and/or toxic fumes. Containers may explode when heated. Runoff may pollute waterways.
Industrial uses
Potassium fluorosilicate is a white to yellowish powder, poorly soluble in water (0.68%
at 20 °C). Because of its poor solubility, it is not commonly used as a modifying reagent.
Safety Profile
A poison by ingestion
and subcutaneous routes. Ingestion can
cause vomiting and dtarrhea. A strong
irritant. Incompatible with hydrofluoric acid.
When heated to decomposition it emits
toxic fumes of SiF4, K3SiF7, and KF.
Purification Methods
Crystallise it several times from conductivity water (100mL/g) between 100o and 0o.
Check Digit Verification of cas no
The CAS Registry Mumber 16871-90-2 includes 8 digits separated into 3 groups by hyphens. The first part of the number,starting from the left, has 5 digits, 1,6,8,7 and 1 respectively; the second part has 2 digits, 9 and 0 respectively.
Calculate Digit Verification of CAS Registry Number 16871-90:
(7*1)+(6*6)+(5*8)+(4*7)+(3*1)+(2*9)+(1*0)=132
132 % 10 = 2
So 16871-90-2 is a valid CAS Registry Number.
InChI:InChI=1/FO2Si.K/c1-4(2)3;/q-1;+1
16871-90-2Relevant articles and documents
Generation of Nitrosyl Salts in Dry Organic Media
Weiss, Robert,Wagner, Klaus-Georg
, p. 1973 - 1976 (2007/10/02)
Trimethylsilyl halides (CH3)3SiX (2a - c, X = Cl, Br, I) are sufficiently electrophilic to cleave, in an equilibrium reaction, alkyl nitrites O=NOR (1a, b, R = i-C5H11, C2H5) with formation of O=NX (3a - c) and (CH3)3SiOR (4a, b).This reaction serves as a convenient in-situ-method to generate nitrosyl compounds NOX in chlorinated hydrocarbons as inert organic media.
Synthesis and properties of NF4+ClO4- and NF4+HF2-·nHF and some reaction chemistry of NF4+ salts
Christe, Karl O.,Wilson, William W.,Wilson, Richard D.
, p. 1494 - 1498 (2008/10/08)
The possibility of synthesizing NF4+XO4- (X = Cl, Br, I) salts by metathesis between NF4SbF6 and CsXO4 in anhydrous HF solution at -78°C was studied. Of these NF4XO4 salts, NF4ClO4 was isolated and characterized by vibrational and 19F NMR spectroscopy. It is an unstable white solid decomposing at 25°C to give NF3 and FOClO3 in high yield. The NF4BrO4 salt is of marginal stability in HF solution and decomposes to NF3, O2, and FBrO2. Attempts to isolate NF4BrO4 as a solid resulted in explosions. The NF4IO4 salt could not be prepared due to the facile fluorination of IO4- to IF4O2- by either HF or BrF5. Attempts to prepare NF4+XF4O- (X = Cl, Br) salts by metathesis between NF4SbF6 and CsXF4O in BrF5 solution at 25°C were unsuccessful; with BrF4O-, fluoride abstraction occurred, resulting in the formation of NF3, F2, and BrF3O, whereas CsClF4O underwent a displacement reaction with BrF5 to give CsBrF6 and ClF3O. The metathetical synthesis of NF4NO3 could not be studied in HF due to the reaction of NO3- with HF to give NO2+, H2O, and HF2-. The metathesis between NF4SbF6 and CsF in HF at -78°C did not produce NF4+F- but produced an unstable white solid of the composition NF4+HF2-·nHF. The composition, thermal stability, spectroscopic properties, and decomposition products of this solid were studied. The NF4+HF2- salt is stable in HF solution at 25°C, and the synthetic usefulness of these solutions for the synthesis of other NF4+ salts is briefly discussed. Attempts to prepare NCl4+ and NCl2O+ salts by F-Cl exchange between BCl3 and NF4+ and NF2O+ were unsuccessful.
