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?

Less quantity of bicarbonate is needed for the neutralization of acidic solution.

It require less bicarbonate to neutralize the acid because of its concentrated solution. If a more concentrated solution of sodium bicarbonate is used to neutralize the acid, lower quantity of it will be enough to neutralize it. Sodium Bicarbonate acts as a buffer which is commonly used for maintaining the pH of the solution.

It acts as a base when it is put in the acidic solution so helps in neutralizing the solution so we can conclude that less quantity of bicarbonate is needed for the neutralization of acidic solution.

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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.

This is true.

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