Potassium chloride density

Salt Substitutes. As a result of concern about the relationship between dietary sodium and hypertension, some salt producers and food companies have developed salt substitutes or low sodium products. Mixtures of sodium chloride and potassium chloride, herbs and spices, as well as modified salt crystals of lower density are marketed in response to a limited consumer demand for reduced-sodium products. This amounts to about 2% of user salt purchases. 

Prepared saltwater completion fluids are made of fresh surface water, with sufficient salts added to produce the proper salt concentration. Usually, the addition of 5 to 10% NaCl, 2% CaClj, or 2% KCl is considered satisfactory for clay inhibition in most formations. Sodium chloride solutions have been extensively used for many years as completion fluids these brines have densities up to 10 Ib/gal. Calcium chloride solutions may have densities up to 11.7 lb/ gal. The limitations of CaClj solutions are (1) flocculation of certain clays, causing permeability reduction, and (2) high pH (10 to 10.5) that may accelerate formation clays dispersion. In such cases, CaC12-based completion fluids should be replaced with potassium chloride solutions. Other clear brines can be formulated using various salts over wide range of densities, as shown in Figure 4-123 [28]. 

Density ppg Fresh Water gal/bbi final Potassium Chloride Ib/bbl final... 

The electrolyte is made by in situ chlorination of vanadium to vanadium dichloride in a molten salt bath. Higher valent chlorides are difficult to retain in the bath and thus are not preferred. The molten bath, which is formed by sodium chloride or an equimolar mixture of potassium chloride-sodium chloride or of potassium chloride-lithium chloride or of sodium chloride-calcium chloride, is contained in a graphite crucible. The crucible also serves as an anode. Electrolysis is conducted at a temperature about 50 °C above the melting point of the salt bath, using an iron or a molybdenum cathode and a cathode current density of 25 to 75 A dnT2. The overall electrochemical deposition reaction involves the formation and the discharge of the divalent ionic species, V2+ ... 

Tests show that the presence of soil reduces the toxicity of copper to the soil-dwelling nematode Caenorhabditis elegans copper toxicity to nematodes increases with increasing densities of bacteria and increasing concentrations of sodium chloride or potassium chloride (Donkin and Dusenbery 1993). Terrestrial isopods efficiently assimilate and store copper as detoxihed granules in the hepatopancreas this activity is in contrast to many species of marine crustaceans that are unable to assimilate, detoxify, or otherwise regulate copper (Weeks and Rainbow 1993). 

Molecular weights.—The composition of the alkali chlorides has been established by analyses. These salts contain alkali, R, and chlorine, Cl, in the proportion 1 1. Consequently, the mol. formulse are represented by RnCln. The difficult volatility of sodium chloride—contrasted with say mercuric chloride—suggests a complex molecule. W. Nernst 78 found the vapour density of both sodium and potassium chlorides, at 2000°, corresponded with the respective formula NaCl and KC1 for the vapours of these salts. L. Riigheimer found that the effect of sodium chloride on the b.p. of bismuth trichloride corresponded with the simple formula NaCl and E. Beckmann obtained a similar result from the effect of sodium, potassium, rubidium, and csesium chlorides on the f.p. of mercuric chloride. 

Serial dilutions are recommended to ensure accurate measurements of highly concentrated, high density, or dried samples. Perform a weight-by-volume dilution with distilled water to obtain a single-strength solution (e.g., usually around 10° Brix for fruit juices unit hi,4), followed by a second dilution using 0.025 M potassium chloride buffer, pH 1.0. Both dilution factors must be considered when calculating monomeric anthocyanin content. 

A solution of 4.15 g. (0.01 mol) of potassium tetrachloro-platinate(II) in 50 ml. of water is placed in a 250-ml., glass-stoppered Erlenmeyer flask. Two and one-tenth milliliters (1.76 g. = slightly less than 0.02 mol) of diethyl sulfide (density, 0.837) is addedf to this solution in small portions, the mixture being shaken vigorously after each addition to ensure complete reaction. J The bright yellow precipitate is immediately separated from the reddish solution by suction filtration, washed at once with several 5-ml. portions of ice-cold alcohol, and then washed with several 5-ml. portions of cold water to remove the potassium chloride. The crystals are dissolved in a minimum amount (ca. 6 ml.) of hot ethanol and the solution cooled in an ice-salt bath. The bright yellow needles are separated by suction filtration and air-dried. The yield is 2.3 g. (51.5%). Anal. Calcd. 

Chloroprene (boiling point 59.4°C, density 0.9583) is, chemically, a chlorovinyl ester of hydrochloric acid and can be manufactured by polymerizing acetylene to vinyl acetylene using a weak solution containing ammonium chloride (NH4C1), cuprous chloride (Cu2Cl2), and potassium chloride (KC1) as catalyst. The off-gas from the reactor has its water condensed out and is then fractionated. Aqueous hydrochloric acid at 35 to 45 °C is then reacted with the vinyl acetylene in the presence of cupric chloride to give chloroprene (2-chloro-l,3-butadiene). 

When the operation started, the iron tank and the individual boxes were filled with saturated solution of sodium (or potassium) chloride while solid salt was put into the stoneware cylinders. The level of electrolyte in tho anode boxes was always somewhat higher than in the tank. During electrolysis the temperature was kept at 85 °C by steam heating steam entered the heating element of the tank through piping H. The voltage across the electrolyzer was 3.5 to 4.0 V. The total current load was about 2500 A which corresponded to a current density of some 2 A/sq. dm. 

A few compounds of cobalt and tin have been described. By fusing together at high temperatures an excess of stannic oxide and cobaltous oxide, using potassium chloride as a flux, Basic Cobalt Stannate, CoSnO,.CoO or Co2Sn04, is obtained.1 The potassium chloride is removed from the cooled mass with water, whilst warm dilute hydrochloric acid effects the solution of the stannate. The pure salt is dark green in colour density 6-30 at 18° C. 

The crystals obtained in this way are red in colour, and isomorphous with the corresponding chlor-platinate. Density 2-738. On heating they turn black, but regain their red colour on cooling. They are readily reduced on warming in a current of hydrogen gas, wdiilst ignition converts them first into the chlor-palladite and finally into potassium chloride and metallic palladium. 

When ignited, the salt decomposes, yielding a mixture of spongy platinum and potassium chloride. The reaction is not readily completed in air, but in a current of hydrogen the decomposition is quantitatively exact. The density of potassium chlor-platinate is 3-499.4... 

The method most generally applied to the isolation of lithium is based on the decomposition of the fused chloride by electrolysis, modifications in practical details having been introduced by various experimenters. Bunsen and Matthiessen1 passed the current from six Bunsen cells through the fused chloride contained in a porcelain crucible, with a carbon rod as anode and an iron wire as cathode. Troost employed a similar method. Guntz2 mixed lithium chloride with potassium chloride, but his product contained 1-3 per cent, of potassium. His current was 10 amperes at 20 volts, with a cathode of iron wire 3-4 mm. in diameter. Borchers3 added chlorides of other alkali-metals and alkaline-earth-metals and a small proportion of ammonium chloride, and employed a current density of 10 amperes per 100 sq. cm. Tucker 4 electrolyzed the chloride without the addition of other material. 

Lithium antimonide, Li3Sb.—Since the direct combination of lithium and antimony is very violent, Lebeau 5 recommends preparing the antimonide by the electrolysis of a fused mixture of lithium and potassium chloride with an iron cathode covered with antimony. It is a dark-grey, crystalline substance of a very reactive nature. Its density at 17° C. is 3 2, and its melting-point is 9503 C. The compound is also formed by the action of antimony on a solution of lithium in liquefied ammonia.6... 

Many properties of electrolytic solutions are additive functions of the properties of the respective ions this is at once evident from the fact that the chemical properties of a salt solution are those of its constituent ions. For example, potassium chloride in solution has no chemical reactions which are characteristic of the compound itself, but only those of potassium and chloride ions. These properties are possessed equally by almost all potassium salts and all chlorides, respectively. Similarly, the characteristic chemical properties of acids and alkalis, in aqueous solution, are those of hydrogen and hydroxyl ions, respectively. Certain physical properties of electrolytes are also additive in nature the most outstanding example is the electrical conductance at infinite dilution. It will be seen in Chap. II that conductance values can be ascribed to all ions, and the appropriate conductance of any electrolyte is equal to the sum of the values for the individual ions. The densities of electrolytic solutions have also been found to be additive functions of the properties of the constituent ions. The catalytic effects of various acids and bases, and of mixtures with their salts, can be accounted for by associating a definite catalytic coefl5.cient with each type of ion since undissociated molecules often have appreciable catalytic properties due allowance must be made for their contribution. 

The silver nitrate is purified by repeated crystallization from acidified solutions, followed by fusion. The purity of the salt is proved by the absence of the so-called volume effect, the weight of silver deposited by a given quantity of electricity being independent of the volume of liquid in the coulometer this means that no extraneous impurities are included in the deposit. The solution of silver nitrate employed for the actual measurements should contain between 10 and 20 g. of the salt in 100 cc. it should be neutral or slightly acid to methyl red indicator, after removal of the silver by neutral potassium chloride, both at the beginning and end of the electrolysis. The anode should be of pure silver with an area as large as the apparatus permits the current density at the anode should not exceed 0.2 amp. per sq. cm. To prevent the anode slime... 

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