Is bicarbonate (HCO3−) acidic ?



Answer:
No,it's a base
No. Since it's an anion, it's a proton acceptor, and that makes it a base.
H2CO3 is weakly acidic.However as it donates H+ to form HCO3-,the former one is acidic and the latter one is a base.
Yes, in the sense of a Lowery-Bronsted acid, HCO3− still has one proton it can donate. The acid dissociation constant for this donation is quite small 4.7 X 10^-11 compared even to the first dissociation constant for H2CO3 at 4.5 X 10^-7. The salt of a weak acid and strong base will be basic because of the hydrolysis reaction, so we expect a solution of NaHCO3 to be basic since it comes from NaOH (strong base) and H2CO3 (weak acid).
"Kentucky" got downed, but his answer was essentially correct, so I gave him a thumbs up, and I hope you will give him the ten points he deserves. I'm answering because I don't think you need the numbers -- I sense that you need the ideas.

Bicarbonate is acidic ... but like many weak bases it is only acidic if there is a stronger base around to accept the proton from it. Hydroxide, for example:

OH(-) + HCO3(-) = H2O + CO3(2-)

But if you just dissolve sodium bicarbonate (baking soda!) in water, the solution will become more basic, because bicarbonate is *also* a weak base:

H2O + HCO3(-) = OH(-) + H2CO3
Yes, in the sense of a Lowery-Bronsted acid, HCO3− still has one proton it can donate. The acid dissociation constant for this donation is quite small 4.7 X 10^-11 compared even to the first dissociation constant for H2CO3 at 4.5 X 10^-7. The salt of a weak acid and strong base will be basic because of the hydrolysis reaction, so we expect a solution of NaHCO3 to be basic since it comes from NaOH (strong base) and H2CO3 (weak acid).

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