Chlorides potassium

Potassium chloride is used as an essential nutrient and as a salt substitute. 

Potassium as a nutrient lowers blood pressure, prevents bone loss, and reduces the risk of kidney stones. Some of these effects are due to the loss of sodium in the urine when potassium is ingested. 

In salt substitutes, the metallic or bitter taste of potassium chloride is often masked by other ingredients, such as the amino acid L-lysine, tricalcium phosphate, citric acid, and glutamic acid. 

Potassium chloride (poe-TAS-ee-yum KLOR-ide) occurs as a white or colorless crystalline solid or powder. It is odorless, but has a strong saline (salty) taste. It occurs naturally in the minerals sylvite, carnallite, kainite, and sylvinite. It also occurs in sea water at a concentration of about 0.076 percent (grams per milliliter of solution). Potassium chloride is the most abundant compound of the element potassium and has the greatest number of applications of any salt of potassium. By far the most important application of potassium chloride is in the manufacture of fertilizers. 

All of the major sources of potassium chloride have their origin in sea water. Sea water is a solution of a number of salts dissolved in water. The most important of those salts are sodium chloride (about 2.3 percent), magnesium chloride (about 0.5 percent), sodium sulfate (about 0.4 percent), 

Potassium chloride. Turquoise atom is potassium and green atom is chlorine. Potassium atom is positively charged. Chlorine atom is negatively charged, publishers 

Any one of the salts present in a sea salt deposit—including potassium chloride-can be extracted by a common procedure. The minerals that make up the deposit are crushed and dissolved in hot water. The solution is then allowed to cool very slowly. As it cools, each of the dissolved salts crystallizes out at a specific temperature, is removed from the solution, and is purified. Since potassium chloride is much more soluble in hot water than in cold water, it crystallizes out after other salts have been removed. 

One use of potassium chloride is as a lethal injection for prisoners who have been given the death penalty. The chemical interferes with normal heart function and causes a heart attack within five 

BP Potassium chloride JP Potassium chloride PhEur Kalii chloridum USP Potassium chloride 

Chloride of potash chloropotassuril dipotassium dichloride E508 potassium monochloride. 

Potassium chloride is widely used in a variety of parenteral and nonparenteral pharmaceutical formulations. Its primary use, in parenteral and ophthalmic preparations, is to produce isotonic solutions. 

Potassium chloride is also used therapeutically in the treatment of hypokalemia. 

Many solid-dosage forms of potassium chloride exist including tablets prepared by direct compression and granulation effervescent tablets coated, sustained-release tablets sustained-release wax matrix tablets micro-capsules pellets and osmotic pump formulations.  

Data reported for the protolysis constant of water in potassium chloride media are listed in Table 5.16. The data have been acquired across a temperature range of0-300 C, with a number of studies obtaining data at 25 C and the data at other temperatures coming from Sweeton, Mesmer and Baes (1974). 

Lobo (1989) presented osmotic coefficient data for KCl solutions from 0 to 250 °C. Equation (5.18) was used to determine water activity data from the available osmotic coefficient data. At all temperatures, the dependence of the water activity data on ionic strength in KCl solutions can be described by Eq. (5.19). Values derived for and in Eq. (5.19) at various temperatures (0-250 °C) are listed in Table 5.17. 

The data listed in Table 5.17 can be described by Eq. (5.22). The values derived 

The ionic strength and temperature dependence of the protolysis constant of water in potassium chloride media were determined using Eq. (5.17). The ion interaction coefficients, and As2, are temperature dependent and were described by using Eqs. (5.23) and (5.24). The data derived for these constants in potassium chloride media are listed in Table 5.19. 

TCQ / (reported) Medium / (mol kg ] 1 (molkg ) log/f (reported) logK (accepted) References 

INTRODUCTION This data sheet summarizes properties of single crystal potassium chloride. 

MECHANICAL PROPERTIES, (298 K) Young s Modulus, (psi) 4, 30 x 10 Hardness, (Knoop) 

Smakula, et al., Harshaw Optical Crystals , The Harshaw Chemical Co., Cleveland, (1967). 

Optical Engineering Handbook , General Electric Co., Scranton, Pa., (1963). 

Four types of separation process, also in combination  

Dissolution processes exploit the different solubilities of the salts 

Extraction of potassium salts occurs mainly by mining (in the Federal Republic of Germany currently to a depth of ca. 1200 m), but leaching processes (solution mining, with one plant each in Canada and Utah/USA) and direct extraction from lakes (Dead Sea Great Salt Lake, Utah Searles Lake, California Lake McLoed, Australia) are also utilized. 

The solid salt has to be more or less strongly ground, depending upon the degree of fusion, before it can be further processed. Potassium chloride can be separated from the salt mixtures by  

These processes are also combined with one another. In dissolution processes, the differences in solubility of the various constituents of the raw salt in water are exploited to attain high percentage potassium chloride. The particular process used depends upon the type of salt mixture, but energy consumption, disposal of byproducts etc. are also important. 

Mole % KCl Specific heat, cal/(g C) Mole % NaGl Specific heat. cal/(g-°C)  

Discussions of chlor-alkali technology and production usually focus on the production of caustic soda from NaCl. The use of KCl to produce caustic potash, an application that accounts for only a few percent of chlorine production, is often ignored. The authors have made a conscious attempt not to do this. Therefore, this section discusses sources and recovery of KCl. The comprehensive discussion of the potash industry and the processing of ore to cormnercial forms of KCl by Zandon, Schoeld, and McManus [28] is the basis for much of what follows. 

Sources. The world produces about 30 million tons of potash each year. This is expressed as K2O and includes all primary potassium mineral products. Besides KCl, these include the sulfate and mixed potassium-magnesium sulfates. The major outlet for potash and agricultural fertilizers accounts for about 95% of production. Known 

KCl is the most important form of potash and is our main interest here. While deposits of sodium chloride are essentially crystalline NaCl with accompanying impurities, potassium chloride frequently exists in mixed ores. Much of it occurs as sylvinite, a mechanical mixture of sylvite (KCl) and halite (NaCl). Sylvite crystals are quite similar 

Lake deposits may be in the form of brine or of crystallized salts. Pure KCl seldom is obtained from any of these, and the same sorts of beneficiation are used for all materials regardless of their sources. 

Most of the air for flotation is brought into the mass by the action of agitators. It may be supplemented by addition of compressed air. 

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CH2CI-CO-CH3. Colourless lachrymatory liquid b.p. 119°C. Manufactured by treating propanone with bleaching powder or chlorine. It is used as a tear gas and is usually mixed with the more potent bromoacetone. chloro acids Complex chloroanions are formed by most elements of the periodic table by solution of oxides or chlorides in concentrated hydrochloric acid. Potassium salts are precipitated from solution when potassium chloride is added to a solution of the chloro acid, the free acids are generally unstable. 

The examples in the preceding section, of the flotation of lead and copper ores by xanthates, was one in which chemical forces predominated in the adsorption of the collector. Flotation processes have been applied to a number of other minerals that are either ionic in type, such as potassium chloride, or are insoluble oxides such as quartz and iron oxide, or ink pigments [needed to be removed in waste paper processing [92]]. In the case of quartz, surfactants such as alkyl amines are used, and the situation is complicated by micelle formation (see next section), which can also occur in the adsorbed layer [93, 94]. 

Fig. XVn-14. Adsorption of nitrogen on potassium chloride at 79 K, plotted according to various equations. (Data from Ref. 82.)...

Potassium chloride actually has the same stnicture as sodium chloride, but, because the atomic scattering factors of potassium and chlorine are almost equal, the reflections with the indices all odd are extremely weak, and could easily have been missed in the early experiments. The zincblende fonn of zinc sulphide, by contrast, has the same pattern of all odd and all even indices, but the pattern of intensities is different. This pattern is consistent with a model that again has zinc atoms at the comers and tlie face centres, but the sulphur positions are displaced by a quarter of tlie body diagonal from the zinc positions. 

We will focus on one experimental study here. Monovoukas and Cast studied polystyrene particles witli a = 61 nm in potassium chloride solutions [86]. They obtained a very good agreement between tlieir observations and tire predicted Yukawa phase diagram (see figure C2.6.9). In order to make tire comparison tliey rescaled the particle charges according to Alexander et al [43] (see also [82]). At high electrolyte concentrations, tire particle interactions tend to hard-sphere behaviour (see section C2.6.4) and tire phase transition shifts to volume fractions around 0.5 [88]. 

A furtlier problem is tire influence of tire ratlier unusual—from tire physiological viewpoint—salt conditions necessary for crystallization. It should not be presumed tliat proteins embedded in a crystal are in tlieir most common native stmcture. It is well known tliat, witli tire exception of sodium or potassium chloride, which are not very useful for inducing crystallization, salts change key protein parameters such as tire melting temperature [19]. 

Thus potassium is obtained by heating potassium chloride with sodium, and barium by reduction of barium oxide with aluminium. 

Sodium sulphate crystallises out in hydrated form (common ion effect) and is filtered off on concentration, sodium dichromate is obtained. For analytical purposes, the potassium salt. K2Cr20-. is preferred potassium chloride is added and the less soluble potassium dichromate obtained. 

Detection of Potassium in the presence of Sodium. Add a cold saturated aqueous solution of sodium picrate to a solution of potassium chloride. A rapid precipitation of the less soluble potassium picrate occurs, even from a i°o solution of potassium chloride. 

If the third substance dissolves in only one of the liquids, it is found that their mutual solubilities are decreased and the C.S.T. is generally raised. For example, a concentration of 0 15 mol of potassium chloride per litre of water raises the C.S.T. of the water - phenol system by about 12° a similar concentration of naphthalene in the phenol produces a rise of about 30°. 

The impurity is potassium chloride. The approximate acid content is determined by heating a weighed sample of the acid in a crucible gently at first and finally at a red heat until no trace of black residue remains, and weighing the white residual potassium chloride. 

The element is much more abundant than was thought several years ago. It is now considered to be the 16th most abundant element in the earth s crust. Rubidium occurs in pollucite, leucite, and zinnwaldite, which contains traces up to 1%, in the form of the oxide. It is found in lepidolite to the extent of about 1.5%, and is recovered commercially from this source. Potassium minerals, such as those found at Searles Lake, California, and potassium chloride recovered from the brines in Michigan also contain the element and are commercial sources. It is also found along with cesium in the extensive deposits of pollucite at Bernic Lake, Manitoba. 

Strontium is found chiefly as celestite and strontianite. The metal can be prepared by electrolysis of the fused chloride mixed with potassium chloride, or is made by reducing strontium oxide with aluminum in a vacuum at a temperature at which strontium distills off. Three allotropic forms of the metal exist, with transition points at 235 and 540oC. 

Several methods are available for producing thorium metal it can be obtained by reducing thorium oxide with calcium, by electrolysis of anhydrous thorium chloride in a fused mixture of sodium and potassium chlorides, by calcium reduction of thorium tetrachloride mixed with... 

Sylvite, see Potassium chloride Szmikite, see Manganese(II) sulfate hydrate... 

A precipitation reaction occurs when two or more soluble species combine to form an insoluble product that we call a precipitate. The most common precipitation reaction is a metathesis reaction, in which two soluble ionic compounds exchange parts. When a solution of lead nitrate is added to a solution of potassium chloride, for example, a precipitate of lead chloride forms. We usually write the balanced reaction as a net ionic equation, in which only the precipitate and those ions involved in the reaction are included. Thus, the precipitation of PbCl2 is written as... 

The electrolysis of potassium chloride [7447-40-7] KCl, to produce chlorine and potassium hydroxide in membrane cells requires similar but unique membranes. Commercial membranes currendy employed in high performance membrane electroly2ers include Du Pont s Nafion 900 series and Asahi Glass s Plemion 700 series. 

Potassium Chloride. The principal ore encountered in the U.S. and Canadian mines is sylvinite [12174-64-0] a mechanical mixture of KCl and NaCl. Three beneficiation methods used for producing fertilizer grades of KCl ate thermal dissolution, heavy media separation, and flotation (qv). The choice of method depends on factors such as grade and type of ore, local energy sources, amount of clay present, and local fuel and water availabiUty and costs. 

Potassium Nitrate. Potassium nitrate, known but Httle used as a fertilizer for many years, may be reclaimed as a by-product of the production of sodium nitrate from natural deposits of caflche in Chile. KNO also has been produced by the double decomposition reaction between sodium nitrate and potassium chloride ... 

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