A Practical Course in Agricultural Chemistry by D. W. Gilchrist Shirlaw and J. E. Nichols (Auth.)

By D. W. Gilchrist Shirlaw and J. E. Nichols (Auth.)

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Extra resources for A Practical Course in Agricultural Chemistry

Example text

From the slide rule at the above temperature and pressure, 100 ml of carbon dioxide are equivalent to 420 mg calcium carbonate. Therefore 35 ml carbon dioxide are equivalent to 147 mg calcium carbonate — this in 25 g of soil. Therefore percentage calcium carbonate = =0-59. 15. THE DETERMINATION OF CARBONATE BY TITRATION The third method for determining calcium carbonate depends on the neutralization of a standard volume of normal hydrochloric acid and back titration with standard sodium hydroxide.

Let the value of the titre be 10 ml; then 50 ml of the reaction solution would be equivalent to 20 ml of N / 1 0 alkali; this is equivalent to 20 ml of N / 1 0 acid, and therefore 5 ml of N acid have been neutralized by the calcium carbonate in the soil. From the reaction equation: 2HC1 + C a C 0 3 -» CaCl 2 + H 2 0 + C 0 2 2 X 35-5 g of hydrochloric acid = 100 g of calcium carbonate Therefore 11. of normal hydrochloric acid = 50 g of calcium carbonate THE ANALYSIS OF SOILS 31 and 5 ml N / 1 0 hydrochloric acid = n g of calcium carbonate = 0-25 g.

Approximately 10 g of soil (more for soils known to contain little carbonate and less for calcareous soils) are accurately weighed out and placed in the 250-ml flask. 2. About 15 ml of 30 per cent hydrochloric acid are placed in the sample bottle and this is carefully placed in the 250-ml flask. 3. T h e flask is attached to the rest of the apparatus, care being exercised that all the rubber connections are gas tight. 4. T h e flask is now tilted so that the acid comes into contact with the soil.

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