Silver chloride fluoride

Bideauxite Lead silver chloride fluoride hydroxide Pb2AgCl3(F,OH)2... 

Silver bromide Silver chloride Silver perchlorate Silver cyanide Silver fluoride Silver iodide Silver permar>gate Silver nitrate Silver carbonate Silver oxide Silver sulphate Silver sulphide Silver phosphate... 

Fluoro-l-(4-methoxyphenyl)-3-(phenylselanyl)propane is obtained in 53 % yield in a one-pot synthesis by reaction of 3-(4-methoxyphenyl)prop-l-ene with benzeneselenenic chloride and silver(I) fluoride in acetonitrile at room temperature for 18 hours.37... 

Phenylmercury(II) fluoride was first claimed to have been isolated as a white powder (which decomposed at 170°C) in the reaction of phenylmercury(II) chloride with silver(I) fluoride.60 Later it was found that this material was a hydrogen fluoride adduct of phenylmercury(II) fluoride,61 obtained also by the more convenient reaction of excess 48% hydrogen fluoride with an ethanol slurry of phenylmercury(II) hydroxide.61 The hydrogen fluoride contained in this product appears to be only loosely bound since prolonged storage at room temperature gives phenylmercury(II) fluoride with mp 300 C. Uncomplexed phenylmercury(II) fluoride can also be obtained from the adduct with hydrogen fluoride by treatment with base.61... 

Disulfides, RSSR, and methylsulfanyl chloride are converted29 into the sulfur(IV) and sulfur(VI) compounds RSF3 (56-61 % with R = Ph) and RSF5 by treatment with silver(II) fluoride in the liquid phase. RSeF3 compounds are prepared similarly.119... 

A second area in which polarization effects show up is the solubility of salts in polar solvents such as water. For example, consider the silver halides, in which we have a polarizing cation and increasingly polarizable anions. Silver fluoride, which is quite ionic, is soluble in water, but the less ionic silver chloride is soluble only with the inducement ofcomplexing ammonia. Silver bromide is only slightly soluble and silver iodide is insoluble even with the addition of ammonia. Increasing covalency from fluoride to iodide is expected and decreased solubility in water is observed. 

The concentration of Cl- ions can be measured gravimetrically by precipitating silver chloride, with silver nitrate as the precipitating reagent in the presence of dilute nitric acid. The white precipitate is filtered off and its mass is determined, (a) Calculate the Cl ion concentration in 25.00 mL of a solution that gave a silver chloride precipitate of mass 3.050 g. (b) Why is the method inappropriate for measuring the concentration of fluoride ions ... 

Carbonyl fluoride can be prepared by any of several methods, including the conversion of carbonyl chloride to the fluoride by such reagents as hydrogen fluoride1 and antimony (III) fluoride.2 The direct combination of carbon monoxide and fluorine is another route to this fluoride, but carbon tetrafluoride is a by-product of the reaction.8 A particularly suitable laboratory preparation of carbonyl fluoride is the fluorination of carbon monoxide by silver (II) fluoride.4 This method, described below, gives directly carbonyl fluoride of rather high purity without recourse to a low-temperature distillation. 

AgCl Silver chloride, 1 3 AgClOs Silver chlorate, 2 4 AgF Silver(I) fluoride, 4 136 AgF2 Silver (II) fluoride, 3 176 Agl Silver iodide, 2 6 AgO Silver (II) oxide, 4 12 Ag2CN2 Silver cyanamide, 1 98 Ag2P03F Silver monofluorophos-phate, 3 109... 

Methoxyphenyl Tellurium Trilluoride1 A 100 ml two-necked flask fitted with a magnetic stirrer and a reflux condenser is charged with 1.3 g (6 mmol) of silver fluoride and 30 ml of dry toluene. The stirred suspension is heated to reflux, 0.68 g (2 mmol) of 4-methoxyphenyl tellurium trichloride are added in small portions, and refluxing is continued for 3 h. The mixture is allowed to cool to 20°, silver chloride is filtered off, and fight petroleum is added to the filtrate. The precipitated product is collected and dried m.p. 176 178 . 4-Ethoxy phenyl tellurium trifluoride (m.p. 204°) was similarly prepared. 

Electrode System Use a fluoride-specific, ion-indicating electrode and a silver-silver chloride reference electrode connected to a pH meter capable of measuring potentials with a minimum reproducibility of 0.2 mV. 

Imidodisulfuryl fluoride is a colorless liquid, b.p. 170°, m.p. 17°. It behaves as a weak acid in water, in w-hich it is stable, and undergoes slow hydrolysis in alkaline solution. The infrared spectrum of imidodisulfuryl fluoride obtained using silver chloride plates (it reacts with sodium chloride) contains bands at 3311(m), 1471(vs), 1337(w), 1248(w), 1217(vs), 923(s), 893(m), and 832(s) cm. . The n.m.r. spectrum of imidodisulfuryl fluoride consists of a single band at —58.5 p.p.m. (from CC1 F), and the proton spectrum consists of a single band at —8.60 p.p.m. (from TMS). 

Preparation of Copper(II) Fluoride (256). 2. Preparation of Copper(II) Nitride (256). 3. Preparation of Copper(II) Bromide (257). 4. Preparation of Copper(II) Acetylide (257). 5. Preparation of Silver from Silver Chloride (257). 

Nielsen compared the induction periods observed by various investigators for several precipitates. He reported the induction period for silver chloride to be inversely proportional to the fifth power of the initial concentration after mixing. Similarly, induction periods for silver chromate, calcium fluoride, calcium oxalate, and potassium perchlorate are inversely proportional to the 4.7,9,3.3, and 2.6 powers of the initial concentrations. For barium sulfate, on the other hand, a variety of discordant values has been observed. La Mer summarized the data of two groups of observers, covering a range of concentrations (Figure 8-1). 

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