From Sodium Ethyl Sulfate [4]
1.5 mole sodium nitrite (103.5g) is intimately mixed with 1 mole of sodium ethyl sulfate (158g) and 0.0625 moles of K2CO3 (8.6g). The mixture is then heated to 125-130°C, at which temperature the nitroethane distills over as soon as it is formed. The heating is discontinued when the distillation flow slackens considerably, and the crude nitroethane is washed with an equal amount of water, dried over CaCl2, and if needed, decolorized with a little activated carbon. The nitroethane is then re-distilled, collecting the fraction between 114-116°C. Yield 46% of theory.
1. Could the K2CO3 in this synthesis be replaced with NaHCO3?
2. What is the purpose of K2CO3 in this reaction?
3. Also the three solid powders are mixed without use of a liquid?
4. Also how would one calculate the yield (46%) in grams?
Preparation of Sodium Ethyl Sulfate
Method 1 [1]
To prepare the sodium salt of ethyl hydrogen sulfate, a mixture of alcohol and H2SO4 is boiled under reflux, cooled, and an excess of calcium carbonate is added. The ethyl hydrogen sulfate is converted into the soluble calcium ethyl sulfate, whilst the excess of H2SO4 is removed as insoluble calcium sulfate. The aqueous filtrate is then mixed with just sufficient sodium carbonate to give sodium ethyl sulfate, the insoluble calcium carbonate being now filtered off. The solution of sodium ethyl sulfate can be concentrated on the water-bath without appreciable hydrolysis, and the sulfate finally crystallized out.
5. Can Calcium Carbonate in this reaction be substituted with Calcium Oxide, molar ratios adjusted?
6. Also, can the Sodium Carbonate in this reaction be replaced with NaHCO3, molar ratios adjusted?
Thanks again,
Just need to confirm what can bee replaced with what...