Calcium chloride naming

How many grams of chlorine gas can be produced from the electrolytic decomposition of 874 g of calcium chloride Name and calculate the mass (in g) of the other product. 

Brines maybe, as the name suggests, solutions of inorganic salts in water, and the two in general use are sodium chloride and calcium chloride. Of these, the former is compatible with most foodstuffs and can be used in direct contact or in circumstances where the brine may come into contact with the product. Calcium chloride has an unpleasant taste and cannot be permitted to contaminate foods. 

Reaction in the absence of catalyst. Assemble in a fume cupboard a 500-ml three-necked flask equipped with a sealed stirrer unit, a double surface reflux condenser and a separatory funnel fit the condenser and the funnel with calcium chloride guard-tubes. Place 179 g (109.5 ml, 1.5 mol) of redistilled thionyl chloride in the flask and 51 g (62.5 ml, 0.5 mol) of hexan-l-ol, b.p. 156-158 °C, in the separatory funnel. Add the alcohol with stirring during 2 hours there is a slight evolution of heat, sulphur dioxide is evolved and the liquid darkens considerably. When all the alcohol has been added, reflux the mixture for 2 hours. Rearrange the apparatus for distillation, and distil slowly the excess of thionyl chloride passes over below 80 °C, followed by a small fraction up to 120 °C and finally the crude 1-chlorohexane at 132— 134 °C. Wash the last-named successively with water, 10 per cent sodium carbonate solution, and twice with water. Dry with anhydrous calcium chloride and distil through a short fractionating column. Pure 1-chlorohexane passes over at 133-134 °C. The yield is 36 g (60%). 

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. 

If the HC1 added was in excess of the CO2, the resultant ocean would have a high content of calcium chloride, but the pH would still be near neutrality. If the CO2 added was in excess of the Cl, Ca would be precipitated as the carbonate until it reached a level approximately that of the oceans today, namely, a few hundred parts per million. 

In the JDaubine-Roy process 3 air is made to ascend a tower and during the process to pass through trays of calcium chloride, the temperature of which is kept low (namely, 4° to 5° C.) by means of water coolers. The limits of hydration range from the monohydrate to the oetahydrate thus... 

This simple hydration theory cannot explain all the known phenomena, as, for example, the opposite effects of calcium chloride and zinc chloride on the colours. Engel2 therefore assumed that the observed colours were due to certain double salts present in the solutions. In the case of pure cobalt chloride, hydrolysis was supposed to occur on heating the solution, the hydrochloric acid liberated uniting with unchanged cobalt chloride and as an explanation of the colour change this is almost certainly incorrect. Ostwald 3 suggested a simple ionic explanation, namely, that the red colour is that of the cobalt cation, and the blue that of the undissociated salt. This is certainly not a complete explanation, and seems to necessitate a very marked decrease in ionisation with rise of temperature, which experiment, so far, does not support.4... 

Give the common name of each of the above compounds (except calcium chloride). 

NOTE.—(a) The ether is shaken with a solution of sodium hydroxide to remove the sulphur dioxide formed as a result of the reduction of the sulphuric acid by the alcohol or by the carbon that separates. The treatment with sulphuric acid removes the alcohol and nearly all the water. The method outlined above can be carried out more rapidly than the one commonly used, namely shaking with a solution of calcium chloride to remove alcohol and then drying first with anhydrous calcium chloride and then with sodium. 

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