Potassium calcium chloride solutions

Separate the ketone layer from the water, and redistil the lattCT rmtil about one third of the material has passed over. Remove the ketone after salting out any dissolved ketone with potassium carbonate (5). Wash the combined ketone fractions four times with one third the volume of 35-40 per cent, calcium chloride solution in order to remove the alcohol. Dry over 15 g. of anhydrous calcium chloride it is best to shake in a separatory funnel with 1-2 g. of the anhydrous calcium chloride, remove the saturated solution of calcium chloride as formed, and then allow to stand over 10 g. of calcium chloride in a dry flask. Filter and distil. Collect the methyl n-butyl ketone at 126-128°. The yield is 71 g. 

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]. 

A white precipitate forms when 2.00 X 10 mL of 0.200 M potassium phosphate solution is mixed with 3.00 X 10 mL of 0.250 M calcium chloride solution. Write the net ionic equation that describes this process. Calculate the mass of the precipitate that forms, and identify the ions remaining in solution. 

Caicium halides are relatively stable there is the possibility of a violent reaction in the presence of a more electropositive alkaline metal eg detonation on impact of a mixture of calcium bromide and potassium. Calcium chloride has a very high enthalpy of solution in water. When dissolved in large quantities in hot water this causes the solution to boil vigorously, creating emissions. 

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. 

Parenterais The most important criterion for parenterals is that they have to be sterile for injection or infusion administration. Excipients are added to make parenterals isotonic with blood, improve solubility, and control pH of the solution. The solvent vehicles include water-for-injection, sterile sodium chloride, potassium chloride, or calcium chloride solution, and nonaqueous solvents such as alcohol, glycol, and glycerin. Preservatives, antioxidants, and stabilizers are normally added to enhance the properties of the drug product. 

Calcium Metavanadate, Ca(V03)2.3H20, gives rise to bright yellow needles when a solution of ammonium metavanadate is boiled with calcium chloride solution and precipitated with alcohol.6 The tetra-hydrate, Ca(V03)2.4H20, is prepared by allowing a mixture of potassium metavanadate and calcium chloride to evaporate for several days.7 Anhydrous calcium metavanadate is a white, porous substance, which is unaffected by strong heating, but is readily decomposed by acids to yield vanadium pentoxide.8 It is much more soluble in water than strontium metavanadate. 

The grade of ethyl acetate used in the preparation is very important. The absolute ethyl acetate (99.7 per cent) sold by the U. S. Industrial Alcohol Company is very satisfactory. If tips grade is not available the ordinary ester may be purified by washing first with sodium carbonate solution, then with saturated calcium chloride solution and finally drying over anhydrous potassium carbonate. 

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. 

The acid salt, (C,H,N,0,),Ca, is obtained by decomposing a boiling solution of arid potassium urate with calcium chloride solution. It crystallizes in needles, soluble in 603 parts of cold H,0 and in 276 po of boiling H,0. It occurs occasionally in urinary sediments and calculi, and in chalk-stones. ... 

Prepare an O.lM calcium chloride solution, also a standard soap solution. For the latter, an 0.04M solution of potassium palmitate is highly satisfactory. It can be made by dissolving the required amount of pure palmitic acid in n-propyl alcohol, adding somewhat less than its equivalent of potassium hydroxide dissolved in n-propyl alcohol, adding to the solution an equal volume of water and a little phenolphthalein, and completing the neutralization with aqueous potassium hydroxide until the phenophthalein is just turned pink. The solution when ready should contain about equal amounts of water and n-propyl alcohol. 

The TFC-SR membrane exhibits the lowest negative charge in calcium chloride solution. This could be due to the presence of divalent positive cations. Potassium chloride and sodium hydrogen carbonate both show an identical zeta potential. The more concentrated sodium chloride solution induces the most negative potential, very similar to those reported in Figure 7.4 for the mixed background electrolyte. 

Oxalate in the presence of fluoride both calcium fluoride and calcium oxalate are precipitated by 0.5m calcium chloride solution in the presence of 2m acetic acid. The fluoride may be identified in the usual manner with concentrated sulphuric acid. The oxalate is most simply detected by dissolving a portion of the precipitate in hot m sulphuric acid and then adding a few drops of a 0.004m solution of potassium permanganate. The latter will be decolourized if an oxalate is present. 

The titre of the sodium and potassium composition was carried out in emission flame photometry and for calcium in atomic absorption. By means of this method we determined the total quantity of sodium, potassium and calcium to be compared with the result obtained by the electrodes (ISE) both at 37 C and 25 C the electrodes have been previously standardized with pure sodium, potassium and calcium chloride solutions. 

Deliquescence and efflorescence. A substance is said to deliquesce (Latin to become liquid) when it forms a solution or liquid phase upon standing in the air. The essential condition is that the vapour pressure of the saturated solution of the highest hydrate at the ordinary temperature should be less than the partial pressure of the aqueous vapour in the atmosphere. Water will be absorbed by the substance, which gradually liquefies to a saturated solution water vapour will continue to be absorbed by the latter until an unsaturated solution, having the same vapour pressure as the partial pressure of water vapour in the air, is formed. In order that the vapour pressure of the saturated solution may be sufficiently low, the substance must be extremely soluble in water, and it is only such substances (e.g., calcium chloride, zinc chloride and potassium hydroxide) that deliquesce. 

The analytical reagent grade is suitable for most purposes. The commercial substance may be purifled by shaking for 3 hours with three portions of potassium permanganate solution (5 g. per litre), twice for 6 hours with mercury, and Anally with a solution of mercuric sulphate (2-5 g. per litre). It is then dried over anhydrous calcium chloride, and fractionated from a water bath at 55-65°. The pure compound boils at 46-5°/760 mm. 

---