Alloys lead-antimony-cadmium

In some regions, a widely used lead alloy is lead antimony cadmium. Antimony and cadmium will react to form an intermetallic compound SbCd. During charge, the positive grid undergoes corrosion and produces antimony in the corrosion layer. 

Solders are alloys that have melting temperatures below 300°C, formed from elements such as tin, lead, antimony, bismuth, and cadmium. Tin—lead solders are commonly used for electronic appHcations, showing traces of other elements that can tailor the solder properties for specific appHcations. 

Pure or alloyed lead may be employed as anode in sulfuric acid addition of 1% silver, 0.3% tin, and a little cobalt raises its resistance toward corrosion. Other metals may improve the yield of a given electrode process. Thus, addition of antimony and cadmium to a lead anode [152] is advantageous in the oxidation of o-toluenesulfonamide to o-benzoylsulfonimide (saccharin). The same effect may be obtained, however, by using an uncoated, unalloyed lead anode if Sb203 is added to the anolyte [153]. It seems possible that the dissolution of some antimony from the alloyed lead anode takes place and produces the same effect as the Sb203 in the anolyte. 

In the analysis of high purity metals, trace elements were pre-concentrated by partial dissolution of the matrix. The remaining small part of the matrix retains all trace elements that are electrochemically less noble than the matrix [79,80]. In this way the trace elements were pre-concentrated from silver-, cadmium-, gallium-, indium-, zinc-, lead-, manganese-, aluminium-, and lead-antimony alloys. 

The first attempts (5) to reduce metal salts with sodium at low temperatures were made by researchers working with solutions of sodium in liquid ammonia. In 1925 Kraus and Kurtz (7) showed that liquid ammonia solutions of sodium could be used to reduce halides of metals that form alloys with sodium. Operating at temperatures below the boiling point of the ammonia solutions they succeeded in reducing the halides of mercury, cadmium, zinc, tin, lead, antimony, bismuth, and thallium, and, by using an excess of sodium, concomitantly produced sodium alloys of these metals. Kraus and Kurtz postulated mechanisms for the reactions and showed that many of the alloys formed were unstable in liquid ammonia— i.e., they disproportionated into free sodium and lower sodium alloys. 

Smelter revenues are also boosted by an ability to recover and sell by-products such as sulfuric acid and copper, as weU as some minor elements such as antimony in the form of antimonial lead alloys, mercury and cadmium. In some instances zinc can be recovered from smelter slags by fuming. 

Rubidium metal alloys with the other alkaU metals, the alkaline-earth metals, antimony, bismuth, gold, and mercury. Rubidium forms double haUde salts with antimony, bismuth, cadmium, cobalt, copper, iron, lead, manganese, mercury, nickel, thorium, and 2iac. These complexes are generally water iasoluble and not hygroscopic. The soluble mbidium compounds are acetate, bromide, carbonate, chloride, chromate, fluoride, formate, hydroxide, iodide. 

Where free machining characteristics are required, this may be achieved by additions of cadmium, antimony, tin or lead (e.g. BS 4300/5). Materials for electrical use are of special composition (BS 2627, 3988), while bearings are manufactured from Al-Sn alloys. 

Further additions of bismuth, cadmium, and antimony to the tin-lead alloys result in the low inching or "fusible" alloys widely used as safety... 

The dimethylglyoxime method has been used for determination of Ni in foodstuffs [10], platinum-group metals [69], iron ores [70], niobium, tantalum, molybdenum, and tungsten [71], steel [72], sewage [73], and aluminium alloys [74]. Dimethylglyoxime in the presence of oxidant was used for determining Ni in foodstuff [75], sea-water [76], plants [77], steel [5], lead and antimony [78], copper alloys [79], zinc and cadmium [80], and tungsten and its... 

Other basic dyes have been used in the determination of thallium in soils [61], antimony and cadmium [27], lead and its alloys [29,31], zinc and its alloys [28], and tungsten [32]. 

Other pyrophoric alloys are prepared by mixing the misch metal with titanium, boron, cadmium, lead, manganese, antimony, mercury, etc. Steam states that 200 tons of ceria are used annually in the manufacture of pyrophoric alloys. 

The basis for the performance of the alloy in VRLA batteries is corrosion of the lead-cadmium-antimony alloy to produce antimony in the corrosion layer of the positive grid, which thus eliminates the antimony-free eifect of pure lead or lead-calcium alloys. During corrosion, small amounts of antimony and cadmium present in the lead matrix are introduced into the corrosion product and thereby dope it with antimony and cadmium oxides. The antimony and cadmium give excellent conductivity through the corrosion product. The major component of the alloy, the CdSb intermetallic alloy, is not significantly oxidized upon float service, but may become oxidized in cycling service. 

Analyses of bullion lead from primary and secondary sources are given in Table 15.2. The data show that the main impurities found in secondary lead are the major constituents of the lead alloys used in the construction of the battery, namely, antimony, tin, arsenic, and copper, whilst minor contaminants include nickel, cadmium, sulfur, bismuth, and silver. 

Potassium or sodium-potassium alloy mixed with ammonium nitrate and ammonium sulfate results in explosion (NFPA 1986). Violent reactions may occur when a metal such as aluminum, magnesium, copper, cadmium, zinc, cobalt, nickel, lead, chromium, bismuth, or antimony in powdered form is mixed with fused ammonium nitrate. An explosion may occur when the mixture above is subjected to shock. A mixture with white phosphorus or sulfur explodes by percussion or shock. It explodes when heated with carbon. Mixture with concentrated acetic acid ignites on warming. Many metal salts, especially the chromates, dichromates, and chlorides, can lower the decomposition temperature of ammonium nitrate. For example, presence of 0.1% CaCb, NH4CI, AICI3, or FeCb can cause explosive decomposition at 175°C (347°F). Also, the presence of acid can further catalyze the decomposition of ammonium nitrate in presence of metal sulfides. 

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