Cyanide borate salts

Sodium Hydrosulfide Solution Sodium Bisulfite Sodium Borate Sodium Borohydride Sodium Cacodylate Hexadecyl Sulfite, Sodium Salt Sodium Chlorate Sodium Chromate Sodium Chromate Sodium Cyanide... 

Zinc forms a wide variety of other salts, many by reaction with the adds, though some can only be obtained by fusing the oxides together. The salts include arsenates (ortho, pyro, and meta), the borate, bromate, chlorate, chlorite, various chromates, cyanide, iodate. various periodates, permanganate, phosphates (ortho, pyro, meta, various double phosphates 1. die selenate, selenites, various silicates, fluosilicate. sulfate, sulfite, and duocyanate. 

There are several salts that behave in this way at atmospheric temperatures, the more important being ammonium acetate potassium bromate, carbonate, cyanide, ferricyanide, ferrocyanide, iodate, and permanganate disodium hydrogen phosphate and sodium borate and carbonate.4 In the case of potassium chlorate the points L and S appear to be practically coincident, whilst for the majority of salts the point S lies somewhere to the left of L, namely at S —that is to say, saturation occurs before the limiting concentration is reached. Generally speaking, at the ordinary temperature, concentrated solutions of salts are less corrosive than distilled water—that is, the point S lies below the level of A, exceptions being 5 ammonium sulphate, aluminium... 

Anions of very weak acids such as arsenite, borate, carbonate, cyanide and silicate exist as anions only in basic solution. It is therefore necessary to use a basic eluent to separate these anions. A solution of sodium hydroxide can be used. Detection with sodium hydroxide is different than with the organic salt and acid eluents. Since the hydroxide ion is more mobile and has a higher equivalent conductance than most other anions, the peaks for the sample anions appear as negative peaks (decreased conductance). However, the peak height (or area) is still a function of the amount of sample anion and the sensitivity is even better than with the more acidic eluents where positive peaks are obtained. 

Light induced electron transfer from an amine to an excited arene leading to a contact radical ion pair is proposed to account for the products observed when 9,10-dicyanoanthracene is irradiated in wet benzene in the presence of an a-aminoketone. The non-polar solvent maintains the proximity of the radical ion pair which would normally then undergo non-productive back electron transfer however, in this case the ion pair reacts, ultimately to furnish 9,10-dihydro-9,10-dicyanoanthracene along with products of fragmentation of the a-aminoketone. Alkyl borate and borohydride salts can also serve as electron donors in the photoreduction of aryl cyanides and aryl halides and an abstract of a report on this topic has appeared. ... 

Trialkyl- and triarylboranes react with various sodium compounds, e.g., the hydride, cyanide, hydroxide, and amide as well as the allfyls, aryls, alcoholates, and phenolates, under mild conditions to form stable complex salts (borates) which contain four-coordinate boron as the central atom in the anion 1-4... 

Sodium is the alkali metal of most commercial importance by far, and the principal sodium compounds of industrial and commercial importance are the chloride (NaCl), the anhydrous carbonate (i.e., soda ash, Na COj), hydrogenocarbonate (i.e., baking soda, NaHCOj), the hydroxide (i.e., caustic soda, NaOH), and the sulfate (Na SO. lOH O, Glauber salt). Large amounts of sodium chloride are, for instance, used in the production of bulk quantities of other industrial chemicals. To a lesser extent sodium cyanide, sodium peroxide, sodium sulfide, sodium borates, sodium phosphates, and sodium alkyl sulfates are also industrially produced. Nevertheless, the aim of this book is not to detail the uses of sodium compounds, which are extensively described in comprehensive industrial inorganic chemistry textbooks thus only the uses and applications of metallic sodium are listed in Table 4.15. 

Cobalt(II) oxide and hydroxide are insoluble, the acetate and nitrate dehques-cent the sulfate, efflorescent the chloride, hygroscopic. The borate, carbonate, cyanide, oxalate, phosphates, sulfide and hexacyanoferrate(ll and III) are insoluble. The ordinary cobalt(II) ammines and the hexacyanocobaltate(III) salts of Alk and Ae are soluble, those of the d-block and Ag" ions insoluble. 

Salt Solutions. Titanium alloys are highly resistant to practically all salt solutions over the pH range of 3 to 11 and to temperatures well in excess of boiling. Titanium withstands exposure to solutions of chlorides (Ref44,45), bromides, iodides, sulfites, sulfates, borates, phosphates, cyanides, carbonates, bicarbonates, and anunonium compoimds. Corrosion rate values for titanium alloys in these various salt solutions are generally less than 0.03 mm/yr (1.2 mils/yr). 

Seawater and salt solutions. Titanium alloys exhibit excellent resistance to most salt solutions over a wide range of pH and temperatures, (jood performance can be expected in sulfates, sulfites, borates, phosphates, cyanides, carbonates, and bicarbonates. Similar results can be expected with oxidizing anionic salts such as nitrates, molybdates, chromates, permanganates, and vanadates and also with oxidizing cationic salts including ferric, cupric, and nickel compounds. 

From the final pond the concentrated brine (Table 1.3) with a density of about 1.25 g/cc was pumped nearly 4.8 km (3 mi 1.5 mi in 1967, Gadsby, 1967) to the processing plant in the town of Silver Peak. The plant had been converted from a silver ore cyanide-leach plant that had operated there from 1864-1961. In the conversion all of the tanks and settlers were rubber lined to reduce iron contamination in the product, and considerable new equipment was added. The solar pond brine was first reacted with lime to remove most of the residual magnesium and some of the sulfate and borate ions, and then a small amount of soda ash was added to precipitate most of the calcium from the lime reactions. The slurry from these operations was settled and filtered, and the overflow solution sent to storage tanks. From there the brine was pumped through filter presses to be totally clarified, and then heated to 93°C (200°F lithium carbonate has an inverse solubility) and reacted with dry soda ash and hot wash and make-up waters to precipitate the lithium carbonate product. Extra water was added to prevent salt from crystallizing, since the pond brine was samrated with salt. The lithium carbonate slurry was thickened in a bank of cyclones, and the underflow fed to a vacuum belt filter where it was washed and dewatered. The cyclone overflow and filtrate were... 

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