Question

Sodium bicarbonate can react with:
(A)$N{{a}_{2}}C{{O}_{3}}$
(B)$NaOH$
(C)$NaH$
(D)$HCl$

Answer 1

Hint: Strong acids react with weak bases to form salt and water. This type of acid-base reaction is called neutralization reaction and leads to the formation of various salts.

Complete step by step solution: Sodium bicarbonate has the formula $NaHC{{O}_{3}}$. It acts as a weak base due to its inability to produce much hydrogen ion in an aqueous solution. This property makes it a useful reactant in the neutralization reaction where it reacts with a strong acid.
\[NaHC{{O}_{3}}\] does not react with weaker acids like sodium carbonate $N{{a}_{2}}C{{O}_{3}}$, sodium hydroxide $NaOH$, and sodium hydride, as these are basic in nature and does not act as acids for a neutralization reaction to occur.
So, sodium bicarbonate $NaHC{{O}_{3}}$ reacts with a strong acid like hydrochloric acid $HCl$, to produce salt, water and carbon dioxide in a neutralization reaction. The reaction is as follows:
\[NaHC{{O}_{3}}+HCl\to NaCl{{H}_{2}}O+C{{O}_{2}}\]
This reaction produces sodium chloride $NaCl$ as a salt along with water and carbon dioxide.

Hence, option (D) is correct.

Additional information: sodium bicarbonate when mixed with water is used as an antacid. It acts as an acidity regulator and treats the acidity condition in humans by neutralizing the hydrochloric acid produced as a result of indigestion that causes heartburn and irritation in the stomach.

Note: Acidity of acids can be checked by their $pH$, which is between $0-1$(for strong acids), also by the capacity to liberate hydrogen ion in water, as a strong acid has a tendency to liberate more ${{H}^{+}}$ ions. While bases have $pH$ in between $8-14$. This is useful in carrying out a neutralization reaction.