ACIDS BASES AND AQUEOUS EQUILIBRIA Calculating the pH of a weak base titrated wi

Question

ACIDS BASES AND AQUEOUS EQUILIBRIA Calculating the pH of a weak base titrated with a strong.. An analytical chemist is titrating 153.1 mL. of a 0.2400 M solution of piperidine (C,HioNH) with a 0.5200 M solution of HNO, The pK, of piperidine is 2.89. Calculate the pHt of the base solution after the chemist has added 83.2 ml. of the HNO, solution to it Note for advanced students: you may assume the final volume equals the initial volume of the solution plus the volume of HNO, solution added. Round your answer to 2 decimal places

Explanation / Answer

base millimoles = 153.1 x 0.2400 = 36.744

acid millimoles = 0.5200 x 83.2 = 43.264

acid millimoles > base millimoles

[H+] = ( 43.264 -36.744 ) / (153.1 + 83.2)

       = 0.0276 M

pH = -log [H+]

pH   = -log (0.0276)

pH = 1.56

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