Acodofocation of sodium bicarbonate(NaHCO 3 ) produces carbon dioxide in a two-s

Question

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

The second step is the decompostion of a carbonic acid to ccarbon dioxide. Write and balance the molecular equation for the second step.

Now write the overall net ionic equation for te 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 decompostion of 1346 mg of NaHCO3?

Explanation / Answer

Answer –

The balance molecular equation for the first step of the reaction of sodium bicarbonate with HF –

     NaHCO3(aq)+ HF(aq) ------> H2CO3(aq)+ NaF(aq)

The balance molecular equation for the second step –

H2CO3(aq) <-----> CO2(g)+ H2O(l)

The overall net ionic reaction –

Total ionic reaction –

Na+(aq) + HCO3-(aq) + H+(aq) + F-(aq) ------> Na+(aq) + F-(aq) + CO2(g) + H2O(l)

Net ionic reaction -

HCO3-(aq) + H+(aq) -----> CO2(g) + H2O(l)

Given, mass of NaHCO3(aq) = 1346 mg

We need to convert it in to mg to g

1 mg = 0.001 g

1346 mg = ?

= 1.346 g

Moles of NaHCO3 = 1.346 g / 84.006 g.mol-1

                             = 0.0160 moles

From the above balanced equation –

1 moles of NaHCO3 = 1 moles of CO2

So, 0.0160 moles of NaHCO3 = ?

= 0.0160 moles CO2

Mass of CO2 = 0.0160 moles * 44.009 g/mol

                      = 0.705 g

                      = 705 mg

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

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