•if a stronger solution of sodium bicarbonate was used in beaker b, would it require more or less acetic acid to neutralize? why?

•if a stronger solution of sodium bicarbonate was used in beaker b, would it require more or less acetic acid to neutralize? why?

Sodium bicarbonate is a salt that formed by reaction of strong base NaOH with weak acid as The overall pH of solution remains basic therefore more acetic acid required to neutralized sodium bicarbonate solution.

More acetic acid is required Explanation: In order to neutrilize a weak acid with a strong base obviously more acid is required to neautrilize. Like in the case given sodium bicarbonate can be formed when a weak acid, acetic acid reacts with a strong base, NaOH. In a titration of a Weak Acid with a Strong Base the titrant is a strong base and the analyte is a weak acid. So more acid is required in order to neutilize NaOH

A stronger acid is needed to neutralize the reaction. Explanation: Neutral pH solutions are because the acid counteracts the effect of the base, and vice versa.
Both chemical products, both acid and base, reach a pH of 7, which indicates the neutrality of the solution in the reaction, that is, the solution is neither acidic nor basic but NEUTRAL.
The higher the alkalinity of the base, the greater the acidity of the acid will be needed to balance and balance the pH to give neutrality as the final product.

Also Read :   Rank these acids according to their expected pka values. clch2cooh clch2ch2cooh ch3ch2cooh cl2chcooh

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