A 50.00-mL solution of 0.0797 M ammonia (K_b = 1.8 $\times$ 10^-5)is titrated with a 0.0315 M solution of hydrochloric acid as the titrant.What is the pH of the base solution after 23.88 mL of titrant have been added? (K_w = 1.00 $\times$ 10^-14) A) 11.08 B) 9.88 C) 4.12 D) 4.74 E) 12.90

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After adding 23.88 mL of HCl, the solution is a buffer of NH3 and NH4+. Use the Henderson-Hasselbalch equation to find the pH.

A 5000-ML Solution of 0 ×\times× 10-5)is Titrated with a 0 ×\times×

A 5000-ML Solution of 0 $\times$ 10^-5)is Titrated with a 0 $\times$