In the graph below, we see the buffer zone as small volumes of 0.1 M NaOH are added to 25 mL of 0.1 M acetic acid. The center of the buffer zone is approximately at the point where the number of moles of NaOH added is equal to half of the number of moles of acetic acid present initially.
What would happen to buffer capacity if we use 25 mL of 0.2 M acetic acid rather than 0.1 M? How would its buffer zone compare to the buffer zone in the graph shown above? Explain your answer with a carefully labeled diagram.

Graph is posted in comments below.

Question

In the graph below, we see the buffer zone as small volumes of 0.1 M NaOH are added to 25 mL of 0.1 M acetic acid. The center of the buffer zone is approximately at the point where the number of moles of NaOH added is equal to half of the number of moles of acetic acid present initially.
What would happen to buffer capacity if we use 25 mL of 0.2 M acetic acid rather than 0.1 M? How would its buffer zone compare to the buffer zone in the graph shown above? Explain your answer with a carefully labeled diagram.

Graph is posted in comments below.