An analytical chemist is titrating 221.9 mL of a 0.8100M solution of diethylamine ((C,H3),NH) with a 0.7200M Solution of HNO3. The pK, of diethylamine is 2.89. Calculate the pH of the base solution after the chemist has added 131.7 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. pH = 0

An analytical chemist is titrating 239.3 mL of a 0.8400M solution of methylamine (CH, NH,) with a 0.3300M solution of HNO,. The p K, of methylamine is 3.36. Calculate the pH of the base solution after the chemist has added 257.2 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. pH =

A chemist titrates 230.0 mL of a 0.1072M ethylamine (C,H,NH,) solution with 0.5758M HCI solution at 25 °C. Calculate the pH at equivalence. The p K, of ethylamine is 3.19. Round your answer to 2 decimal places. Note for advanced students: you may assume the total volume of the solution equals the initial volume plus the volume of HCl solution added. pH = Explanation Check 2021 McGraw-Hill Education All Rights sved T Le/Py 18 MacBook Air esc F7 FI F2 F3 F4 *

An analytical chemist is titrating 126.8 mL of a 0.2600M solution of diethylamine ((C₂H), NH) with a 0.1600M solution of HNO3. The pK, of diethylamine is 2.89. Calculate the pH of the base solution after the chemist has added 83.3 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 = 0 x 5 ? do

An analytical chemist is titrating 200.9 mL of a 0.1300M solution of piperidine (C,H, NH) with a 0.6100M solution of HNO₂. The pK, of piperidine is 2.89. Calculate the pH of the base solution after the chemist has added 19.4 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. PH-0 X

An analytical chemist is titrating 208.8mL of a 0.7500M solution of methylamine CH3NH2 with a 0.5600M solution of HNO3 . The pKb of methylamine is 3.36 . Calculate the pH of the base solution after the chemist has added 236.8mL 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.

An analytical chemist is titrating 219.9 mL of a 0.5100 M solution of aniline (CH,NH,) with a 0.1800 M solution of HNO,. The p K, of aniline is 9.37. 3 Calculate the pH of the base solution after the chemist has added 360.5 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.

An analytical chemist is titrating 184.0 mL of a 0.5400M solution of propylamine (C,H,NH,) with a 0.8600M solution of HNO3. The p K, of propylamine is 3.46. Calculate the pH of the base solution after the chemist has added 60.2 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.

An analytical chemist is titrating 135.0 mL of a 0.06400M solution of piperidine (CH,NH) with a 0.4700M solution of HNO3. The pK, of piperidine is 2.89. Calculate the pH of the base solution after the chemist has added 21.3 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 HNO 3 solution added. Round your answer to 2 decimal places. pH = 0 ×

An analytical chemist is titrating 71.3 mL of a 1.000M solution of formic acid (H,CO,) with a 0.6600M solution of KOH. The pK, of formic acid is 3.74. Calculate the pH of the acid solution after the chemist has added 119. mL of the KOH solution to it. Note for advanced students: you may assume the final volume equals the initial volume of the solution plus the volume of KOH Solution added. Round your answer to 2 decimal places. pH =