Question

If a more concentrated initial solution of sodium bicarbonate was used in beaker C, would it require more or less bicarbonate to neutralize the acid? Why?

Answer 1

Answer:

It would require less bicarbonate to neutralize the acid.

Explanation:

Sodium bicarbonate NaHCO3 is a, partly soluble sodium salt that decomposes in water to form a weakly basic buffer solution. It dissociates in water resulting in bicarbonate anions HCO− , sodium ions Na+ and H+.

2 NaHCO3(s) → Na2CO3(s) + CO2(g) + H2O(g)

Buffer solutions exist in equilibrium. In a  solution with a strong acid and the conjugate base react, while the other carbonate ions dissociate to form carbonic acid, shifting the equilibrium of the solution back towards a balanced state.

HA ⇄  H+ + A-

Due to its buffering ability i.e. how well it maintains equilibrium, less bicarbonate would need to be added later on to neutralize the acid.