Of calcium chloride solutions

Viscosity is an important property of calcium chloride solutions in terms of engineering design and in appHcation of such solutions to flow through porous media. Data and equations for estimating viscosities of calcium chloride solutions over the temperature range of 20—50°C are available (4). For example, at 25°C and in the concentration range from 0.27 to 5.1 molal (2.87—36.1 wt %) CaCl2, the viscosity increases from 0.96 to 5.10 mPa-s (=cP). 

There are 10 producers of calcium chloride solutions in the United States, three of these also make a dry product. Solution production is centered around Michigan (brines), California and Utah (brines), and Louisiana (by-product acid). The majority of dry calcium chloride is made in Michigan, lesser quantities in Louisiana, and minor quantities in California. Production involves removal of other chlorides (primarily magnesium) by precipitation and filtration followed by concentration of the calcium chloride solution, either for ultimate sale, or for feed for dry product. Commercial dry products vary by the amount of water removed and by the nature of the drying equipment used. Production and capacity figures for the United States are indicated in Table 2. 

Boil the tartaric acid and caustic soda solution for three hours in a round flask (I litre), or preferably in a tin bottle furnished with reflu. condenser. The use of a tin vessel obviates certain clitli-cultiesof filtration which the solution of the silica by the action of the alkali on the glass entails. The liquid, after boilinjg, is carefully neutralised with cone, hydrochloric acid (it is acl is-able to remove a little of the solution beforehand in case overshooting the mark) and an excess of calcium chloride solution is added to the hot liquid. The mixture is left overni hl. and the calcium salts filtered off at the pump, washed with water, and well pressed. 

When the temperature of the plasma reaches about 5° to 8°C, the calculated quantity of calcium chloride solution is added in amount which is from 0.2 to 0.3% in excess of that needed to react with and precipitate the anticoagulant. The temperature of the plasma is allowed to rise to about 24°C. At 18° to 24°C strands of fibrin begin to appear and the... 

The solution is cooled and then diluted with 450 cc. of water. The oily layer of chloronitrile is collected in about 80 cc. of chloroform and Separated from the water solution. The chloroform solution is washed with about 125-150CC. of calcium chloride solution (prepared by adding one volume of water to an equal volume of a saturated solution of crystallized calcium chloride) and once with 125-150 cc. of water, and then dried over fused calcium chloride. 

Prolonged action of calcium chloride solution upon the zinc coating of a galvanised iron vessel caused slow evolution of hydrogen, which became ignited and exploded. 

Potassium Citrate Dissolve 1 g in a mixture of 1.5 ml DW and 2.5 ml dilute HC1, add 4 ml alcohol and 4 drops of calcium chloride solution, and allow to stand for 1 hour. The mixture remains clear. 

Traces of calcium can be removed from solutions of sodium salts by precipitation at pH 9.5-10 as its 8-hydroxyquinolinate. The excess of 8-hydroxyquinoline acts as a collector. The magnesium content of calcium chloride solutions can be reduced by making them about O.IM in sodium hydroxide and filtering. 

Numerous studies on the thermodynamics of calcium chloride solutions were published in the 1980s. Many of these were oriented toward verifying and expanding the Pitzer equations for determination of activity coefficients and other parameters in electrolyte solutions of high ionic strength. A review article covering much of this work is available (7). Application of Pitzer equations to the modeling of brine density as a function of composition, temperature, and pressure has been successfully carried out (8). 

Ammonium Carbonate. — On adding 3 cc. of calcium chloride solution to 10 cc. of the ammonium dithiocarbonate solution, no precipitate should form, even on warming. 

Oxalic Acid. — The solution of 2 cc. of hydrogen peroxide in 10 cc. of water should not become turbid on the addition of calcium chloride solution. 

Viscosity is an important properly of calcium chloride solutions in terms of engineering design and in application of such solutions to flow-through porous media. Data and equations for estimated viscosities of calcium chloride solutions over the temperature range of 20-50°C are available. 

Permanent hardness of water cannot be removed by boiling. Let us see how we can remove permanent hardness by conducting a simple experiment. Take two identical glass beakers. Name them beaker 1 and beaker 2. Fill 100 ml of tap water in both the beakers. Add 20 ml of calcium chloride solution (or a little solid CaCl2) to both the beakers. Mix well. Add about 20 ml of sodium carbonate solution (or a little Na2C03) to beaker 2. Add about 10 ml of soap solution to both the beakers. 

When the temperature of the plasma reaches about 5° to 8°C, the calculated quantity of calcium chloride solution is added in amount which is from 0.2 to... 

This treatment removes unoxidized ethyl lactate. Each shaking should be continued for 5 minutes. It is convenient to separate the layers by centrifuging. Droplets of calcium chloride solution should not be present in the oil when it is to be distilled, or some polymerization will occur. 

This can be prepared in several different ways. Commonly dry Castile soap is dissolved in 80 per cent, alcohol in such proportions as will yield a solution well above the desired final concentration 100 grams per litre is a convenient ratio. After allowing this solution to stand at rest for several days for the deposition of undissolved matter, a quantity of the clear liquid is withdrawn (usually 75-100 c.c. per litre of final solution), and so diluted with 80 per cent, alcohol as to produce a solution which on titration with a known weight of calcium chloride solution under the standard conditions will give results in accordance with Clark s table. The calcium chloride solution is best prepared by dissolving 0-2 grams of Iceland spar in dilute hydrochloric acid excess of acid is removed by evaporation on a water bath and the solution then diluted to 1 litre with distilled water. A mixture of 25 c.c. of this solution, mixed with 25 c.c. of water, should require 7-8 e.e. of Clark s standard solution for the production of a permanent lather. 

After filtration, addition of sodium sulphide to the clear solution effects the precipitation of the three metals, cobalt, nickel, and manganese, as sulphides. Digestion with the calculated quantity of ferric chloride oxidises the manganese sulphide to sulphate, which passes into solution. The residue consists of cobalt and nickel sulphides, which are washed and converted into their soluble sulphates by roasting. The sulphates are extracted with water, and converted into chlorides by addition of calcium chloride solution. Their separation is effected g.s follows The requisite fraction of the chloride solution is precipitated with milk of lime, and the insoluble hydroxides of nickel and cobalt thus obtained are oxidised to the black hydroxides by treatment with chlorine. The. washed precipitate is then introduced into the remainder of the chloride solution, and the whole is well stirred and heated, when the black hydrated oxide of nickel passes, into solution, displacing tlm Remainder of. the cobalt from the solution, into. the precipitate.. The final product is thus a suspension of hydrated peroxide.of cobalt,in p. solution of nickel chloride, from which idle cobalt precipitate is removed by filtration, washed, and ignited, to the black oxide. 

The work presented here addresses this question for a laboratory ion-exchange system that is relatively simple. Effluent concentration histories were obtained for calcium and chloride ions during miscible displacement of calcium chloride solutions through vertical columns containing homogeneous, repacked sandy soil that was water-saturated. Calcium self-exchange was the... 

Miscible displacement of calcium-chloride solutions through water-saturated laboratory soil columns was studied for a wide range of constant water-flow rates. Calcium- and chloride-effluent... 

Boiling point of calcium chloride solution, °C Solubility, g per 100 g of water Boiling point of calcium chloride solution, °C Solubility, g per 100 g of water... 

Addition of calcium chloride solution to sodium tungstate solution. This reaction was used on a large scale in former times as purification step (precipitation of artificial scheelite). 

In a chemical equation, the numbers in front of the separate atoms, ions or molecules are known as coefficients they indicate exactly how many of the atoms, ions or molecules react with another type of atoms, ions or molecules in order for a complete reaction. As an example, let us look at the well-known reaction of calcium chloride solution with silver nitrate solution to form insoluble silver chloride ... 

The following example of advective transport in the presence of a cation exchanger is derived from a sample calculation for the program phreeqm (Appelo and Postma, 1993, example 10.13, pp. 431 134). The chemical composition of the effluent from a column containing a cation exchanger is simulated. Initially, the column contains a sodium-potassium-nitrate solution in equilibrium with the cation exchanger. The column is then flushed with three pore volumes of calcium chloride solution. Calcium, potassium, and sodium react to equilibrate with the exchanger at all times. 

Directions (a) Bubble carbon dioxide from the generator you used in Experiment 38 h into 10 c.c. of calcium chloride solution. (1) How does the result differ from that obtained when carbon dioxide is passed into calcium hydroxide (2) Explain the cause of this difference. (3) How can calcium carbonate be prepared from calcium chloride Try the method which you suggest. (4) What leads you to believe that the substance which you have obtained is calcium carbonate ... 

Into each of two test tubes put 5 c.c. of a solution of disodium orthophosphate and add to one a few drops of silver nitrate solution and to the other a few drops of calcium chloride solution. Kepeat the foregoing tests with the pyrophosphate and metaphosphate solutions prepared in (a) and (5). (2)... 

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