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Why is it necessary to expel dissolved carbon dioxide liberated during the reaction of sodium carbonate and HCl?
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+ Chemical reactions
+ Chemistry
+ Carbon dioxide
+ Hydrochloric acid
Posted by
Nina Lanyon
Why is it necessary to expel dissolved carbon dioxide liberated during the reaction of sodium carbonate and HCl?
Not sure why it would be necessary, unless you're trying to accelerate the reaction for some reason. Heating the solution should ‘boil off’ any dissolved CO2 gas. However, dissolved CO2 gas does lower pH some, since it forms a weak acid. I do recall heating a solution once in chemistry to boil off any dissolved CO2. Can't remember what the experiment was though… ?
Not sure why it would be necessary, unless you're trying to accelerate the reaction for some reason. Heating the solution should ‘boil off’ any dissolved CO2 gas. However, dissolved CO2 gas does lower pH some, since it forms a weak acid. I do recall heating a solution once in chemistry to boil off any dissolved CO2. Can't remember what the experiment was though… ?
Probably you forgot to say that you refer to an acid-base titration?
In that case you have to dispose all of [math]CO_2[/math] because it's a (week) acid and you couldn't find the exact titration's final point if you didn 't do it.
Probably you forgot to say that you refer to an acid-base titration?
In that case you have to dispose all of [math]CO_2[/math] because it's a (week) acid and you couldn't find the exact titration's final point if you didn 't do it.
Not sure why it would be necessary, unless you're trying to accelerate the reaction for some reason. Heating the solution should ‘boil off’ any dissolved CO2 gas. However, dissolved CO2 gas does lower pH some, since it forms a weak acid. I do recall heating a solution once in chemistry to boil off any dissolved CO2. Can't remember what the experiment was though… ?
Na2CO3(s) + 2HCl(aq) > 2NaCl(aq) + H2CO3(aq) (weak, carbonic acid)
H2CO3(aq) + heat > CO2(g) + H2O (solution pH is raised)
Not sure why it would be necessary, unless you're trying to accelerate the reaction for some reason. Heating the solution should ‘boil off’ any dissolved CO2 gas. However, dissolved CO2 gas does lower pH some, since it forms a weak acid. I do recall heating a solution once in chemistry to boil off any dissolved CO2. Can't remember what the experiment was though… ?
Na2CO3(s) + 2HCl(aq) > 2NaCl(aq) + H2CO3(aq) (weak, carbonic acid)
H2CO3(aq) + heat > CO2(g) + H2O (solution pH is raised)
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Probably you forgot to say that you refer to an acid-base titration?
In that case you have to dispose all of [math]CO_2[/math] because it's a (week) acid and you couldn't find the exact titration's final point if you didn 't do it.
<>
Probably you forgot to say that you refer to an acid-base titration?
In that case you have to dispose all of [math]CO_2[/math] because it's a (week) acid and you couldn't find the exact titration's final point if you didn 't do it.
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