NaHCO3 is acidic salt but shows basic nature in aqueous solution = Why?

You cannot claim that NaHCO3 is an acid salt because of the H in the formula. Is NaOH also an acid salt for this reason? In order to be an acid salt it must produce or cause the production of an ionisable H+ . NaHCO3 does not do this. The reaction equation of NaHCO3 in water is:
NaHCO3 + H2O → Na+ OH- + H2CO3.
The H2CO3 is unstable and breaks down to CO2 and H2O
The basicity of the solution comes from the OH- ions produced.

Is Nahco3 A Salt

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1 NaOH ( strong base) ascorbic acid ( weak acid) NaHC6H6O6 => basic 2 NaOH ( strong base) HCl ( strong acid) NaCl => neutral 3 NH3 ( weak base) HCl ( strong acid) NH4Cl => acidic 4 NaOH ( strong base) citric acid ( weak acid) sodium citrate => basic 5 NH3 ( weak base) H2SO4 ( strong acid) (NH4)2SO4 => acidic

There is no such term as "ACIDIC SALT"....it is "ACID SALT"......Sodium bicarbonate(NAHCO3)...is an "ACID SALT" and not and "ACIDIC SALT"....but it dissolves in water to form a mild basic solution..this is because:
NAHCO3 is formed by PARTIAL NEUTRALIZATION of carbonic acid by Sodium hydroxide....

CARBONIC ACID is an weak acid while SODIUM HYDROXIDE is a strong alkali....

so when they form the salt....sodium hydroxide being stronger than carbonic acid produces a salt which is also of basic nature but NOT as basic as sodium hydroxide cause it is partially neutralized by carbonic acid....

Similarily if a strong acid and a weak base reacts to form a salt...the salt produced will be acidic in nature(WHEN DISSOLVED IN WATER).........
This phenomenon is called Hydrolysis of salts....I hope it's given in ur book.....

Interesting. I agree with Trevor in that I wouldn't have called NaHCO3 an acidic salt, but that is because I know this compound is called sodium bicarbonate and it is a basic salt.

Nevertheless. There are 3 compounds to consider here: H2CO3, NaHCO3 and Na2CO3. H2CO3 is carbonic acid and essentially has two protons which it can and will donate as an acid. Na2CO3 is sodium carbonate, and it may be considered as carbonic acids conjugate base. If you were to write it as a salt with the associated charges it would 2Na+ and (CO3)2-.

The interemediate stage is where carbonic acid loses one hydrogen and becomes sodium bicarbonate, NaHCO3. NaHCO3 can still lose one hydrogen, gain one sodium and become sodium carbonate hence its relative 'acidity' to sodium carbonate. However, when you write sodium bicarbonate as a salt with its relative charges it becomes Na+ and HCO3-. This HCO3- is still a conjugate base of H2CO3, and hence dissolved in water, it will ultimately make the water basic.

Realistically, it may do this in a couple of ways: It may break down to produce CO2 and OH- ions, thus increasing the pH, or it may break down to produce CO2 and H2O and thus remove H+ ions from the water, thus increasing the pH.

Hope this helps!