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

Question

Bingel

2 months 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:

lana [2.4K] · Answer 1 · 2026-03-30T09:02:26+03:00

Response:

It would need a lower amount of bicarbonate to neutralize the acid.

Explanation:

Sodium bicarbonate (NaHCO3) is a partially soluble sodium salt that breaks down in water to create a weakly basic buffer solution. It separates in water releasing bicarbonate ions (HCO−), sodium ions (Na+), and H+.

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

Buffer solutions are maintained in equilibrium. In a solution with a strong acid, the conjugate base reacts, while other carbonate ions release to form carbonic acid, driving the solution back toward balance.

HA ⇄ H+ + A-

Due to its buffering capability, which is how effectively it stabilizes the equilibrium, less bicarbonate will be required later on to neutralize the acid.