Question

What happens when a solution of sodium hydrogen carbonate is heated? Write the chemical equation of the reaction involved.

Answer 1

It would gradually turn into a solution of sodium carbonate.

It would gradually turn into a solution of sodium carbonate.The hydrogencarbonates (bicarbonates) are not as stable as the carbonates. In aqueous solution of a bicarbonate the following equilibrium exists:

It would gradually turn into a solution of sodium carbonate.The hydrogencarbonates (bicarbonates) are not as stable as the carbonates. In aqueous solution of a bicarbonate the following equilibrium exists:2HCO3(-) + H2O = CO3(2-) + CO2 + H2O

It would gradually turn into a solution of sodium carbonate.The hydrogencarbonates (bicarbonates) are not as stable as the carbonates. In aqueous solution of a bicarbonate the following equilibrium exists:2HCO3(-) + H2O = CO3(2-) + CO2 + H2OOn prolonged boiling of the solution, the bicarbonate will almost entirely get converted to the more stable carbonate with the liberation of carbon dioxide, just like it happens when the pure or dry salt is heated.

It would gradually turn into a solution of sodium carbonate.The hydrogencarbonates (bicarbonates) are not as stable as the carbonates. In aqueous solution of a bicarbonate the following equilibrium exists:2HCO3(-) + H2O = CO3(2-) + CO2 + H2OOn prolonged boiling of the solution, the bicarbonate will almost entirely get converted to the more stable carbonate with the liberation of carbon dioxide, just like it happens when the pure or dry salt is heated.So, the solution becomes that of sodium carbonate on continued heating

It would gradually turn into a solution of sodium carbonate.The hydrogencarbonates (bicarbonates) are not as stable as the carbonates. In aqueous solution of a bicarbonate the following equilibrium exists:2HCO3(-) + H2O = CO3(2-) + CO2 + H2OOn prolonged boiling of the solution, the bicarbonate will almost entirely get converted to the more stable carbonate with the liberation of carbon dioxide, just like it happens when the pure or dry salt is heated.So, the solution becomes that of sodium carbonate on continued heatingI'm guessing that you should get Na2CO3 as a white solid if you heat the solution at a high temperature (about 200°C)

It would gradually turn into a solution of sodium carbonate.The hydrogencarbonates (bicarbonates) are not as stable as the carbonates. In aqueous solution of a bicarbonate the following equilibrium exists:2HCO3(-) + H2O = CO3(2-) + CO2 + H2OOn prolonged boiling of the solution, the bicarbonate will almost entirely get converted to the more stable carbonate with the liberation of carbon dioxide, just like it happens when the pure or dry salt is heated.So, the solution becomes that of sodium carbonate on continued heatingI'm guessing that you should get Na2CO3 as a white solid if you heat the solution at a high temperature (about 200°C)Going by the chemical reaction :

It would gradually turn into a solution of sodium carbonate.The hydrogencarbonates (bicarbonates) are not as stable as the carbonates. In aqueous solution of a bicarbonate the following equilibrium exists:2HCO3(-) + H2O = CO3(2-) + CO2 + H2OOn prolonged boiling of the solution, the bicarbonate will almost entirely get converted to the more stable carbonate with the liberation of carbon dioxide, just like it happens when the pure or dry salt is heated.So, the solution becomes that of sodium carbonate on continued heatingI'm guessing that you should get Na2CO3 as a white solid if you heat the solution at a high temperature (about 200°C)Going by the chemical reaction :2NaHCO3 → Na2CO3 + H2O + CO2

It would gradually turn into a solution of sodium carbonate.The hydrogencarbonates (bicarbonates) are not as stable as the carbonates. In aqueous solution of a bicarbonate the following equilibrium exists:2HCO3(-) + H2O = CO3(2-) + CO2 + H2OOn prolonged boiling of the solution, the bicarbonate will almost entirely get converted to the more stable carbonate with the liberation of carbon dioxide, just like it happens when the pure or dry salt is heated.So, the solution becomes that of sodium carbonate on continued heatingI'm guessing that you should get Na2CO3 as a white solid if you heat the solution at a high temperature (about 200°C)Going by the chemical reaction :2NaHCO3 → Na2CO3 + H2O + CO2Usually, solid sodium bicarbonate decomposes in correspondence to the above equation. I do have sodium bicarbonate solution in the lab, will try heating it and let you know.

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