A 25.0-mL sample of 0.10 M C₂H₃NH₂ (ethylamine) is titrated with 0.15 M HCl. What is the Ph of the solution after 9.00 mL of acid have been added to the amine? K_b = 6.5 × 10^-4 A) 11.08 B) 10.88 C) 10.74 D) 10.55 E) 10.49

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After adding 9.00 mL of 0.15 M HCl to 25.0 mL of 0.10 M ethylamine, the moles of HCl and ethylamine are calculated. The reaction forms the conjugate acid, and the remaining ethylamine and formed conjugate acid are used to find the pH using the Henderson-Hasselbalch equation. The pH is approximately 10.74.

A 250-ML Sample of 0