but at normal temps and pressures, youll get gaseous CO2 bubbling off.......
Both the text book and your professor are correct, however your professor could've at least elaborated and explained further. Not every base has an OH- group attached, e.g. ClO3^-, HS^- etc, so I can see how that mislead you.
Sodium carbonate is soluble so the total ionic equation is:
2Na^+(aq) + CO3^2-(aq) + 2H^+(aq) + 2Cl^-(aq) → 2Na^+(aq) + 2Cl^-(aq) + CO2(g) + H2O(l)
The step in eq.1 is omitted because it's an intermediate.
The net ionic is:
CO3^2-(aq) + 2H^+(aq) → CO2(g) + H2O(l)
A base is a substance that accepts the H+ ion (bronstead-lowry theory- acid is one that donates)
This can be OH- as you said, however it can be other ions such as carbonates:
CO3(2-) accepts 2H+ -----> CO2 + H2O
The ionic eq is:
2Na(+) CO3(2-) + 2H(+) 2Cl(-) ---> CO2 + H2O + 2Na(+) 2Cl(-)
Get rid of spectator ions
to leave
CO3(2-) + 2H(+) ---> CO2 + H2O
H2CO3 is just CO2 dissolved in H2O! in a closed system, this is what you might get, but at normal temps and pressures, you'll get gaseous CO2 bubbling off.
