Which buffer would be better able to hold a steady ph on the addition of strong acid, buffer 1 or buffer 2? explain. buffer 1: a solution containing 0.10 m nh4cl and 1 m nh3. buffer 2: a solution containing 1 m nh4cl and 0.10 m nh3

Buffer 1.

Explanation:

Ammonia is a weak base. It acts like a Bronsted-Lowry Base when it reacts with hydrogen ions.

.

gains one hydrogen ion to produce the ammonium ion . In other words, is the conjugate acid of the weak base .

Both buffer 1 and 2 include

The ammonia in the solution will react with hydrogen ions as they are added to the solution:

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There are more in the buffer 1 than in buffer 2. It will take more strong acid to react with the majority of in the solution. Conversely, the pH of buffer 1 will be more steady than that in buffer 2 when the same amount of acid has been added.

what's the

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