The resultant pH= 4.95
<h3>Steps</h3>
A weak acid solution and a conjugate base solution can be combined to create a buffer.
Strong acid or strong base addition does not result in a significant pH shift when a weak acid and conjugate base are present in the solution.
A buffer's pH can be determined using the Henderson-Hasselbalch equation:
pH = Pka + log [base] / [acid]
Let 0.05-x represent the amount of acetate in the buffer and x represent the amount of acetic acid in the buffer.
5.2 = 4.75 + log 0.05− x / x
0.05− x = 0.0369 M
HA = 0.0130 M × 800 mL+ 50 mL× 0.1 M = 15.47 mmol
A = 0.0369 M× 800 mL− 50 mL×0.1 M = 24.52 mmol
The new pH is:
pH= 4.75 + log 25.42 / 15.47
pH= 4.95
The resultant pH of the solution= 4.95
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