Calculating the pH of a weak base titrated with a strong acid Izabella An analytical chemist is titrating 235.3 mL of a 0.2600M solution of piperidine (C5H10NH) with a 0.3600M solution of HNO3. The pK of piperidine is 2.89. Calculate the pH of the base solution after the chemist has added 42.7 mL of the HNO3 solution to it. Note for advanced students: you may assume the final volume equals the initial volume of the solution plus the volume of HNO3 solution added. Round your answer to 2 decimal places. pH = -

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Calculating the pH of a weak base titrated with a strong acid
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Izabella
An analytical chemist is titrating 235.3 mL of a 0.2600M solution of piperidine (C5H10 NH) with a 0.3600M solution of HNO3. The pK of piperidine is 2.89.
Calculate the pH of the base solution after the chemist has added 42.7 mL of the HNO 3 solution to it.
Note for advanced students: you may assume the final volume equals the initial volume of the solution plus the volume of HNO3 solution added.
Round your answer to 2 decimal places.
pH
=
☐
☑
?
18
Ar
回
Transcribed Image Text:Calculating the pH of a weak base titrated with a strong acid 1/5 Izabella An analytical chemist is titrating 235.3 mL of a 0.2600M solution of piperidine (C5H10 NH) with a 0.3600M solution of HNO3. The pK of piperidine is 2.89. Calculate the pH of the base solution after the chemist has added 42.7 mL of the HNO 3 solution to it. Note for advanced students: you may assume the final volume equals the initial volume of the solution plus the volume of HNO3 solution added. Round your answer to 2 decimal places. pH = ☐ ☑ ? 18 Ar 回
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