chemistry world

Estimation of Carbon and Hydrogen

Carbon and hydrogen present in an organic compound are estimated by 'Liebig's method'.

Principle

These elements are estimated by its combustion in an atmosphere of pure oxygen to form carbon dioxide (CO₂) and water (H₂O).

Apparatus

The apparatus used for the estimation of carbon and hydrogen consists of a long hard-glass combustion tube packed with copper oxide and coarse copper oxide. Left end of the combustion tube is connected to the oxygen supply, while at the other end, two pre-weighed absorption tubes are placed. One of the absorption tube is packed with magnesium perchlorate which absorbs water vapour, and the other is packed with KOH or asbestos which absorbs CO₂.

Fig:16.15 Apparatus for the estimating carbon and hydrogen

Procedure

A small quantity (0.2 to 0.3 g) of the organic compound is placed in a porcelain / platinum boat. The boat is placed in the combustion tube and is heated at 400^o to 450^oC. Pure dry oxygen is slowly passed through the tube. Combustion is complete in 8 to 10 hours. It results in the formation of CO₂ and H₂O from the carbon and hydrogen in the compound. They are absorbed in the absorption tubes at the end.

The absorption tubes are removed and weighed to determine the amount of CO₂ and H₂O formed in the reaction. The masses and the percentages of C and H in the compound are calculated as follows.

Calculations

Let,

The mass of the organic compound taken be = W g

Increase in the mass of magnesium perchlorate tube = W₁ g

Increase in the mass of the KOH tube = W₂ g

So,

Mass of water formed = W₁ g

Mass of carbon dioxide formed = W₂ g

Estimation of Nitrogen

Nitrogen can be estimated by either of the two methods:

Dumas' method

Kjeldahl's method

Dumas' method

A known mass of the organic compound is heated with cupric oxide in an atmosphere of carbon dioxide. The carbon and hydrogen in the compound are oxidised to carbon dioxide and water respectively, while nitrogen is set free. Any oxide of nitrogen produced during this process, is reduced back to free nitrogen by heated copper gauze. The gaseous mixture consisting of CO₂, H₂O and N₂ is collected over an aqueous solution of potassium hydroxide. All the gases except nitrogen are absorbed by the solution. The volume of gas (nitrogen) collected is measured. From the volume of nitrogen obtained the percentage of nitrogen in the compound is calculated.

Fig:16.16 Apparatus for the estimation of nitrogen by Dumas' method

Calculations

Let,

The mass of the organic compound taken be = W g

Volume of nitrogen collected = V₁ g

Atmospheric pressure = P mm Hg

Temperature at which gas is collected = T₁ K

Therefore,

Pressure of the N₂ gas, P₁ = (P - p) mm of Hg

(1 mol of N₂ = 28 g = 22400 mL)

Therefore,

Kjeldahl's method

Kjeldahl's method is a faster method than Dumas' method. However, this method is used only for those organic compounds that are converted quantitatively to ammonium sulphate on heating strongly with concentrated sulphuric acid.

Kjeldahl's method cannot be used for the organic compounds,

Containing nitrogen in the ring, e.g., pyridine, quinoline etc.

Containing nitro (-NO₂) and diazo (-N = N-) groups.

Kjeldahl's method involves two steps:

Digestion

A known mass (0.3 to 0.5 g) of the given organic compound is digested with concentrated H₂SO₄, in presence of a small quantity of potassium sulphate and copper sulphate in a Kjeldahl's flask. Potassium sulphate raises the boiling point of sulphuric acid and copper sulphate catalyzes the digestion. In 3 to 4 hours, the organic compound is completely decomposed to form ammonium sulphate.

The method consists of heating a substance with sulphuric acid, which decomposes the organic substance by oxidation to liberate the reduced nitrogen as ammonium sulphate. In this step potassium sulphate is added to increase the boiling point of the medium (from 337 °C to 373 °C) . Chemical decomposition of the sample is complete when the initially very dark-coloured medium has become clear and colourless.

The solution is then distilled with a small quantity of sodium hydroxide, which converts the ammonium salt to ammonia. The amount of ammonia present, and thus the amount of nitrogen present in the sample, is determined by back titration. The end of the condenser is dipped into a solution of boric acid. The ammonia reacts with the acid and the remainder of the acid is then titrated with a sodium carbonate solution by way of a methyl orange pH indicator.

Degradation: Sample + H₂SO₄ → (NH₄)₂SO₄(aq) + CO₂(g) + SO₂(g) + H₂O(g)

Liberation of ammonia: (NH₄)₂SO₄(aq) + 2NaOH → Na₂SO₄(aq) + 2H₂O(l) + 2NH₃(g)

Capture of ammonia: B(OH)₃ + H₂O + NH₃ → NH₄⁺ + B(OH)₄⁻

Back-titration: B(OH)₃ + H₂O + Na₂CO₃ → NaHCO₃(aq) + NaB(OH)₄(aq) + CO₂(g) + H₂O

Distillation

The digested reaction mixture, on cooling, is transferred to a round bottomed distillation flask, and distilled with a concentrated alkali solution (NaOH). Ammonia produced is absorbed in a known volume of HCl solution of a known strength.

The un-neutralised HCl is then back-titrated against a standard alkali. From the acid consumed, the amount of ammonia produced and hence the mass of nitrogen is calculated.