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.

Calculate the change in pH when 9.00 mL of 0.100 M HCl(aq) is added to 100.0 mL of a buffer solution that is 0.100 M in NH, (aq) and 0.100 M in NH, Cl(aq). Consult the table of ionization constants as needed. ApH = 9.17 Calculate the change in pH when 9.00 mL of 0.100 M NaOH is added to the original buffer solution. ApH 9.32 0

An analytical chemist is titrating 74.8 mL of a 0.7500M solution of propylamine (C,H,NH,) with a 0.2500M solution of HIO,. The p K, of propylamine is 3.46. Calculate the pH of the base solution after the chemist has added 265.9 mL of the HIO, solution to it. Note for advanced students: you may assume the final volume equals the initial volume of the solution plus the volume of HIO, solution added. Round your answer to 2 decimal places. olo pH = I Ar

An analytical chemist is titrating 221.9 mL of a 0.9800M Solution of propionic acid (HC,H,CO,) with a 0.8400OM solution of NaOH. The pK, of propionic acid is 4.89. Calculate the pH of the acid solution after the chemist has added 190.2 mL of the NAOH SOlution to it. Note for advanced students: you may assume the final volume equals the initial volume of the solution plus the volume of NaOH Solution added. Round your answer to 2 decimal places. pH = ?

A chemist titrates 210.0 mL of a 0.4409M hypochlorous acid (HCIO) solution with 0.7835M NaOH solution at 25 °C. Calculate the pH at equivalence. The pK, of hypochlorous acid is 7.50. 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 NAOH solution added. pH = ] ?

An analytical chemist is titrating 149.7 mL of a 0.5500M solution of benzoic acid (HC H CO,) with a 0.8000 M solution of NaOH. The p K of benzoic acid is 4.20. Calculate the pH of the acid solution after the chemist has added 16.29 mL of the NaOH solution to it. Note for advanced students: you may assume the final volume equals the initial volume of the solution plus the volume of NaOH solution added. Round your answer to 2 decimal places. do pH = Check Explanation 2021 McGraw-Hil Education. All Rights Reserved. Terms of Use Privacy Accessibility V I 11:55 acer &

An analytical chemist is titrating 123.0 mL of a 0.5600M solution of diethylamine ((C₂H₂), NH) with a 0.5300M solution of HNO3. The pK, of diethylamine 2 is 2.89. Calculate the pH of the base solution after the chemist has added 111.5 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.

An analytical chemist is titrating 88.2 mL of a 0.2300M solution of nitrous acid (HNO₂) with a 0.5500M solution of NaOH. The pK, of nitrous acid is 3.35. Calculate the pH of the acid solution after the chemist has added 15.8 mL of the NaOH solution to it. Note for advanced students: you may assume the final volume equals the initial volume of the solution plus the volume of NaOH solution added. Round your answer to 2 decimal places. pH = 11 ? 0

A chemist titrates 130.0 mL of a 0.6533 M cyanic acid (HCNO) solution with 0.5467 M KOH solution at 25 °C. Calculate the pH at equivalence. The pK, of cyanic acid is 3.46. 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 KOH solution added. pH = U

10 An analytical chemist is titrating 120.4 mL of a 0.5800M solution of piperidine (C5H₁NH) with a 0.7600M solution of HNO3. The pK, of piperidine is 2.89. Calculate the pH of the base solution after the chemist has added 64.0 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 Ś