Silver sulfate

Silver sulfate, Ag2S04—A713 (saturated solution) stir mechanically 10 g of the salt in a liter of water for 3 hours decant and use the clear liquid. 

Acetylene can be deterrnined volumetricaHy by absorption in Aiming sulfuric acid (or more conveniently in sulfuric acid activated with silver sulfate) or by reaction with silver nitrate in solution and titration of the nitric acid formed ... 

A quinoline—bromine adduct in hot carbon tetrachloride containing pyridine gives a 90% yield of 3-bromoquinoline (21) 3-chloroquinoline [612-59-9] is prepared by an analogous route, but in poorer yield. A quinoline—aluminum chloride complex heated with bromine gives a 78% yield of 5-bromoquinoline [165-18-3] (22). Equal quantities of 5- and 8-bromoquinoline [16567-18-3] are formed when quinoline is treated with one equivalent of bromine in concentrated sulfuric acid containing silver sulfate (23). 

Silver Chloride. Silver chloride, AgCl, is a white precipitate that forms when chloride ion is added to a silver nitrate solution. The order of solubility of the three silver halides is Cl" > Br" > I. Because of the formation of complexes, silver chloride is soluble in solutions containing excess chloride and in solutions of cyanide, thiosulfate, and ammonia. Silver chloride is insoluble in nitric and dilute sulfuric acid. Treatment with concentrated sulfuric acid gives silver sulfate. 

Silver Nitrite. Silver nitrite, AgN02, is prepared from silver nitrate and a soluble nitrite, or silver sulfate and barium nitrite. 

Perhalates. Whereas silver perchlorate [7783-93-9] AgClO, and silver periodate [15606-77-6] AglO, are well known, silver perbromate [54494-97-2] AgBrO, has more recendy been described (18). Silver perchlorate is prepared from silver oxide and perchloric acid, or by treating silver sulfate with barium perchlorate. Silver perchlorate is one of the few silver salts that is appreciably soluble in organic solvents such as glycerol, toluene, and chlorobenzene. 

Silver Sulfate. Silver sulfate, AggSe204, is prepared by treating metallic silver with hot sulfuric acid. Alternatively, a solution of silver nitrate is acidified with sulfuric acid and the nitric acid is evaporated, leaving a solution of silver sulfate. Silver sulfate is more soluble in sulfuric acid than in water because of the formation of silver hydrogen sulfate [19287-89-9], AgHSO. ... 

Silver sulfate decomposes above 1085°C into silver, sulfur dioxide, and oxygen. This property is utilized ia the separation of silver from sulfide ores by direct oxidation. Silver sulfate is reduced to silver metal by hydrogen, carbon, carbon monoxide, zinc, and copper. 

Combination silver—silver salt electrodes have been used in electrochemistry. The potential of the common Ag/AgCl (saturated)—KCl (saturated) reference electrode is +0.199 V. Silver phosphate is suitable for the preparation of a reference electrode for the measurement of aqueous phosphate solutions (54). The silver—silver sulfate—sodium sulfate reference electrode has also been described (55). 

Silver sulfate has been described as a catalyst for the reduction of aromatic hydrocarbons to cyclohexane derivatives (69). It is also a catalyst for oxidation reactions, and as such has long been recommended for the oxidation of organic materials during the deterrnination of the COD of wastewater samples (70,71) (see WASTES, INDUSTRIAL WATER, INDUSTRIAL WATERTTEATI NT). 

Other Uses. Photochromic glass contains silver chloride (80) and silver molybdate [13765-74-7] (81) (see Chromogenic materials). An apparatus coated with silver nitrate has been described for the detection of rain or snow (82). Treatment with silver-thiosulfate complex has been reported as dramatically increasing the post-harvest life of cut carnations (83). Silver sulfate has been used in the electrolytic coloring of aluminum (84). Silver sulfate also imparts a yellowish red color to glass bulbs (85). 

Purification actually starts with the precipitation of the hydrous oxides of iron, alumina, siUca, and tin which carry along arsenic, antimony, and, to some extent, germanium. Lead and silver sulfates coprecipitate but lead is reintroduced into the electrolyte by anode corrosion, as is aluminum from the cathodes and copper by bus-bar corrosion. 

Hydrolysis of Ethyl Esters. The hydrolysis of esters (other than ethyl sulfates) is not a commercial route for producing ethanol. An indirect hydration of ethylene actually takes place during the proposed (153) hydrolysis of ethyl sulfite cataly2ed by silver sulfate. 

Silver sulfate [10294-26-5] M 311.8, m 652°, b 1085°(dec), d 5.45. Crystd form hot cone H2SO4 contg a trace of HNO3, cooled and diluted with H2O. The ppte was filtd off, washed and dried at 120°. 

Carboplatin (96) is significantly less toxic in the clinic than cisplatin. Most particularly, it is much less nephrotoxic. Use of a bidentate ligand also ensures formation of a ds complex. Its synthesis begins with cis-diammine platinum diiodide (94) which is reacted with silver sulfate to give cis-diaquodiam mine platinum sulfate (95). This is reacted with the barium salt of 1,1-cyclo-butanedicarboxylic acid to yield carboplatin [23],... 

The saturated solution of silver sulfate in water at 25°C has a molality equal to 0.02689, and the activity coefficient y of tho solute in this saturated solution is 0.533. 

Taking the values for the Ag+ ion and the SOi ion from Table 45, find the value of the partial molal entropy of silver sulfate in an aqueous solution at 25° having a molality equal to 10 see the discussion of (179). 

A saturated solution of silver sulfate at 25°C can be prepared by dissolving 1.2gof silver(I) sulfate in water to make 250.0 mL of solution. What is f p for silver(I) sulfate ... 

In Experiment 7, would the ratio between moles of copper atoms used and moles of silver atoms formed change if silver sulfate, Ag2S04, had been used rather than silver nitrate, AgN03 Explain. 

The nature of the brominating medium has an influence on reaction products. Although there is no need for strongly acidic reagents, a buffer is frequently added to adsorb HBr [81H(15)1285]. When 2,3-dibromobenzo[f>]thiophene was brominated in sulfuric acid with silver sulfate present, a small amount of the 4-bromo (but none of the expected 5-bromo) derivative was observed [70JCS(C)1949]. 

Activating groups at the 5-position led to high yields when bromination took place in chloroform or acetic acid. Products obtained were the 4-bromo derivatives of 5-amino- (90%), 5-hydroxy- (95%), and 5-methoxy-benzisothiazole (40%). Use of the bromine-sulfuric acid-silver sulfate system raised the yield of the last-named product to 87% [80JCR(S)197], 7-Amino-4-chloro-l,2-benzisothiazole was brominated in the 6-position [71JCS(C)3994],... 

Reactions in acetic anhydride with metal acetates present probably occur by 1,4-addition of bromonium acetate (85CHE458). When NBS in sulfuric acid at 20°C was used, the product ratio resembled that observed with bromine-sulfuric acid-silver sulfate. At 60°C the ratio changed to 2 1.2 1 as a consequence of more extensive dibromination (88CHE892) (Scheme 33). As might have been deduced, 2-(2 -thienyl)quinoline was brominated only in the thiophene ring (82CHE28). 

Phenanthridine (74) was converted by NBS into the 2-bromo derivative (40%) (55JA6379), but the bromine-sulfuric acid-silver sulfate reagent gave low yields of 1-, 4-, and 10-bromophenanthridines in the ratio (1 6.4 9.5), a reactivity order which contrasts with that found in nitration (1 > 10 > 4 > 2) (69AJC1105). Phosphoryl chloride converted phenanthridine 5-oxide into the 6-chloro derivative, but when that position was blocked by a phenyl substituent, the reductive chlorination process gave a 2-chloro compound (84MI2). 

Sei.f-Tfst 11.11A The solubility product of silver sulfate, Ag2S04, is 1.4 X 10 Estimate the molar solubility of the salt. 

Ag2 SO4 The polyatomic sulfate ion indicates that this is an ionic compound. Silver is always +1, so no Roman numeral is needed silver sulfate. 

Arrhenius devised demonstrations to support his ideas. The diagrams illustrate two of these. Layers of acetic acid solution and pure water, separated by a thin layer of concentrated sugar solution, show low conductivity. When the layers are mixed, the conductivity increases. To Arrhenius, this demonstrated that diluting acetic acid leads to more dissociation into ions. Layers of solutions of silver sulfate and barium... 

C18-0108. When silver sulfate dissolves in water at 25 °C, the equilibrium concentration of Ag is 3.0x10 mol / L. Use this information to calculate for Ag2 SO4. ... 

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