If 19.2 g sodium carbonate is obtained from the thermal decomposition of 75.0 g of sodium hydrogen carbonate according to the unbalanced equation,
NaHCO3 → Na2CO3 + H2O + CO2
What is the percent yield?

What is your attempt?

Did you try to find out the number of grams of Na2CO3 that you should be getting from heating 75.0 g of NaHCO3?

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Originally Posted by brittw27

If 19.2 g sodium carbonate is obtained from the thermal decomposition of 75.0 g of sodium hydrogen carbonate according to the unbalanced equation,
NaHCO3 → Na2CO3 + H2O + CO2
What is the percent yield?

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The yield would be 19.88 Carbonic acid, it all turns to an acid.

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NaHCO3 does not turn to carbonic acid... it gets decomposed by environmental heat.

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Originally Posted by Unknown008

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NaHCO3 does not turn to carbonic acid... it gets decomposed by environmental heat.

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How so?

The equation you posted in your very first post says so.

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Originally Posted by Unknown008

The equation you posted in your very first post says so.

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Sodium Bicarbonate, baking soda... is what we are talking about... it can be either a weak base or acidic. It's a weak base, and it can be an acid.

In neutral solutions it ionizes to Na+ + HCO3-.
The HCO3- can either donate its proton (acid) or accept another (base).
In strong basic solution:
HCO3- + OH- --> CO32- + H2O
In strong acidic solution:
HCO3- + H+ --> H2CO3

Yes, but in this case, there is no acid nor base to react with. NaHCO3 is thus not reacting with an acid/base, but is decomposing.