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Aspirin is a weak acid with a pKa of 2.5. If a buffered solution of aspirin...

Aspirin is a weak acid with a pKa of 2.5. If a buffered solution of aspirin with a pH of 2.5 is diluted by a factor of 10,what is the new pH?
A) 1.5
B) 2.5
C) 3.5
D) between 2.5 and 3.5
E) 7

I'm not sure what the answer is but I'm guessing it's 2.5 because according to my textbook the pH of a buffered solution doesn't change the acid/base ration, and so according to the Henderson–Hasselbalch equation the pH doesn't change as well. However, when I consulted online sources it says that diluting weak acids increases dissociation and therefore pH.

I'm not sure what's right/wrong so I would like some guidance in this.

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