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

Question

cupoosta [38]

3 years ago

6

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?

Biology

1 answer:

saveliy_v [14] · Answer 1 · 2022-11-29T20:44:52+03:00

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.