1.) Acidification of sodium bicarbonate (NaHCO3) produces carbon dioxide in a 2-

Question

1.) Acidification of sodium bicarbonate (NaHCO3) produces carbon dioxide in a 2-step process. The first step produces carbonic acid (H2CO3). Wtite and balance the molecular equation for the first step of the reaction of sodium bicarbonate with HF.

The second step is the decomposition of carbonic acid to carbon dioxide. Write and balance the molecular equation for the second step.

Now write the overall net ionic equation for the acidification of NaHCO3 to produce CO2.

What is the molar ratio of CO2 produced to NaHCO3 decomposed?

What mass of CO2 will be produced by the complete decomposition of 1346 mg of NaHCO3?

Explanation / Answer

First Step: NaHCO3(s) + HF(aq) ? NaF(aq) + H2CO3(aq)
Second Step: H2CO3(aq) ? H2O + CO2(g)
Net Ionic Equation HCO3^-(aq) + H^+(aq) ? H2O + CO2(g)
HF should never be used as a typical acid (use HCl) as it causes severe burns by a unique mechanism. It also eats glass.
2. molar ratio produced = 1:1
3. NaHCO3 mol. wt . = 84

moles = 1346/ 84 = 16 = moles of CO2
mass of CO2 = 16 * 16 = 704 g

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