Clear carbonated soda

If all went well, cloudiness happened. When you blow bubbles into clear calcium hydroxide, it turns cloudy. When you pour clear calcium hydroxide into clear carbonated soda, the solution turns cloudy. The explanation for both of these is that you observed an acid-base reaction. In each case, the cloudiness came from the interaction of an acid—carbonic acid (H COj)—and a base—calcium hydroxide. A carbonated soda already has carbonic acid in it. When you blow bubbles into calcium hydroxide, the carbon dioxide (CO ) from your breath interacts with the water in the calcium hydroxide solution to form H COj. Here s the balanced equation for the interaction of carbonic acid and calcium hydroxide ... 

Now take some of the clear, carbonated soda that was a suggested purchase in the Shopping List and Solutions and add the purple-cabbage indicator. You should observe a pale pink solution. Carbonated soda... 

Reaction —Dissolve a small quantity of the n-o ime in a few diops of acetic anhydride, waim if necessary, and cool quickly by adding a little ice. Add to the clear solution solid sodium carbonate and a little caustic soda solution. The solution becomes clear on shaking or warming. 

The reactions in Table 13.8 show that carbon dioxide is a common product in many neutralization reactions. This is clearly displayed when a drop of vinegar (acetic acid) is added to baking soda (sodium bicarbonate). Some aspirin includes an antacid in their formulation to neutralize some of the acidity imparted by the aspirin (acetylsalicylic acid). These are commonly referred to as buffered aspirins. 

E. W. Hilgard verified the conclusion and suggested the reaction as an explanation of the formation of natural soda but G. Lunge showed that dil. soln. are required, and on evaporation, the reaction is reversed. H. Taylor (1851) used barium bicarbonate under similar conditions and R. von Wagner showed that a clear soln. of barium bicarbonate decomposes sodium sulphate, forming barium sulphate and sodium bicarbonate, and that a comparatively small proportion of the bicarbonate will complete the reaction between barium carbonate and sodium sulphate. 

To proceed with the fusion. It has been stated that tho mixture above-mentioned, when introduced into the crucible, should not fill more than two-thirds of its capacity. This precaution is necessary on account of the effervescence which will take place, owing to tho displacement of the carbonic acid from the carbonate of soda by the silica, and the combination, of the carbon with the oxygen of the litharge. The heat is continued till perfect fusion is effected, and towards the last the temperature is raised to bright redness, until no further effervescence occurs, and a clear liquid homogeneous dag is obtained. The crucible must then be immediately removed from the fire, otherwise the... 

IN A CUSTARD CUP, DISSOLVE 1 TEASPOON SAL SODA (WASHING SODA, SODIUM CARBONATE) IN 50 ml WATER. HEAT SLIGHTLY. ADD SLAKED LIME MIXED WITH WATER. STIR. CHEMICAL REACTION PRODUCES SODIUM HYDROXIDE AND CALCIUM CARBONATE. FILTER. CLEAR LIQUID CONTAINS THE SODIUM HYDROXIDE (LYE). THE jCAL-CIUM CARBONATE IS HELD BACK BY THE FILTER. 

For the treatment of camotite several methods are available. The method recommended by the United States Bureau of Mines2 is as follows The ore is leached with concentrated nitric acid at 100° C., neutralised with caustic soda, and barium chloride and sulphuric acid added to the solution to precipitate the radium as barium-radium sulphate. The precipitate settles in three or four days, after which time the clear liquid is decanted into tanks and is treated with excess of boiling sodium carbonate solution in order to precipitate any iron, aluminium and chromium present. The solution now contains sodium uranyl carbonate and sodium vanadate. It is nearly neutralised with nitric acid, and caustic soda is added in sufficient quantity to precipitate the uranium as sodium uranate. After filtering, the remaining solution is neutralised with nitric acid and ferrous sulphate added, whereupon iron vanadate is thrown down. By this method it is claimed that 90 per cent, of the radium, all the uranium, and 50 per cent, of the vanadium in the camotite are recovered. 

When extremely poor control is exercised over lime-soda softening, the pH of the treated water can often rise and fall, and may rise to exceed pH 11.0 to 11.5 on occasion. This is clearly unacceptable and will dramatically increase the risk of carbonate fouling, thus tending to make subsequent treatment and control of the cooling system extremely difficult (on the premise that chemical and services treatment programs can be developed for almost any quality of cooling system makeup water, as long as the water quality remains reasonably consistent). 

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