Silver hypophosphite

Silver nitrate Mercury (II) chloride Hypophosphites, H2P02 White precipitate of silver hypophosphite White precipitate of calomel in cold solution, which darkens upon... 

Silver nitrate solution white precipitate of silver hypophosphite, AgH2P02, which is slowly reduced to silver at the ordinary temperature, but more rapidly on warming, hydrogen being simultaneously evolved. 

Solutions of phosphites and hypophosphites with silver nitrate give initially white precipitates of silver phosphite and silver hypophosphite, respectively. Both these precipitates decompose to give metallic silver on warming (14.7) and (14.8). This test will distinguish them from hypophosphates or fully oxidised phosphates whose silver salts are relatively stable when precipitated. 

Water Treatment of sample with NaOH and hypophosphite passage through silver filter (free cyanide) treatment in photo cell prior to filter for total cyanide and selective oxidation for cyanides not amenable to chlorination (CNATC) Flame AAS or graphite furnace AAS 2 ng/mL (flame AAS) 0.06 ng/mL (graphite furnace AAS 107 (free cyanide), 90.4 (CNATC), 98.1 (total cyanide) Rosentreter and Skogerboe 1992... 

As a last example on the fabrication of silver clusters, it is worth mentioning that they can also be prepared in microemulsions, where the small droplets of water act as nanoreactors. The surfactant used was AOT and the reducing agent was a very mild one, i.e. sodium hypophosphite. In this manner, fluorescent silver clusters with less than ten atoms are formed and showed planar shape when deposited onto gold substrates, as determined by scanning tunneling microscopy [67, 68]. 

Salts of the noble metals are reduced by hypophosphorous acid or hypophosphites, and in many cases phosphorous acid can be isolated among the products. The reduction of silver nitrate was noticed by the early workers.7 Phosphoric acid was formed with or without the evolution of hydrogen, thus —... 

Detection and Estimation of Phosphites and Hypophosphites. —Solutions of hypophosphorous and phosphorous acids, as well as their salts, when evaporated to dryness and heated, give spontaneously inflammable phosphine and a residue of phosphoric acid or phosphate respectively. The reduction of salts of copper and silver, and of mercuric chloride, by these acids may also be used as tests. When the alkali salts are boiled -with concentrated alkali hydrogen is evolved and a phosphate is found in solution, thus... 

Hypophosphites are all soluble in water and therefore the solutions give no precipitates with the ions of the alkaline earths, silver, etc. Silver salts, however, are rapidly reduced to metallic silver, and phosphoric acid is found in the solution —... 

Phosphites may be distinguished from hypophosphites by several tests. The ions of barium and lead give white precipitates with solutions of phosphites. Silver nitrate gives a white precipitate in the cold, from which black metallic silver is quickly deposited on warming —... 

Hypophosphite. (i) Silver nitrate solution test (IV.31, 1), copper sulphate solution test (IV.31, 4), and ammonium molybdate test (IV.31, 9). 

Mn(II) can be oxidized quantitatively to permanganate in perchloric acid by the use of silver ion as a catalyst. In the presence of phosphate, Ce(III) is oxidized to Ce(lV) phosphate, which precipitates from a solution containing sulfuric and phosphoric acids. The precipitate can be dissolved in sulfuric acid. Other oxidations that can be performed quantitatively are V(IV) to V(V) in acid solution, hypophosphite and phosphite to phosphate, selenite to selenate, tellurite to tellurate, nitrite to nitrate, and in alkaline solution, iodide to periodate. 

Fig. 3. Polarization curves for anodic oxidation of hypophosphite on different metals (bath composition 0.2 mol dm NaH2P02, 0.2 mol dm sodium citrate, 0.5 mol dm H3BO3, pH 9, 70°C). Dashed lines current density attributed to anodic dissolution of silver or copper (I. Ohno et al., 1985 [5]).

Aldehydes N,N -Carbonylimidazole. Ethoxymethyleneaniline. Ethyleneimine. For-maldoxime. Imidazole. N-Methyl-N-phenylcarbamyl chloride. p-Nitro-N.N-dimethylaniline. Phosgene. Silver tosylate. Sodium ethoxide. Sodium hypophosphite. Sodium 2-nitropro-panenitronate. Trimethylamine oxide. 

NITRIC ACID, SILVER(I) SALT (7761-88-8) A powerful oxidizer. Forms friction- and shock-sensitive compounds with many materials, including acetylene, anhydrous ammonia (produces compounds that are explosive when dry), 1,3-butadiyne, buten-3-yne, calcium carbide, dicopper acetylide. Contact with hydrogen peroxide causes violent decomposition to oxygen gas. Violent reaction with chlorine trifluoride, metal powders, nitrous acid, phospho-nium iodide, red or yellow phosphorus, sulfur. Incompatible with acetylides, acrylonitrile, alcohols, alkalis, ammonium hydroxide, arsenic, arsenites, bromides, carbonates, carbon materials, chlorides, chlorosulfonic acid, cocaine chloride, hypophosphites, iodides, iodoform, magnesium, methyl acetylene, phosphates, phosphine, salts of antimony or iron, sodium salicylate, tannic acid, tartrates, thiocyanates. Attacks chemically active metals and some plastics, rubber, and coatings. 

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