An analytical chemist is titrating 199.2 mL of a 0.3400M solution of formic acid (H, Co,) with a 0.4000M solution of NaOH. The p K, of formic acid is 3.74. Calculate the pH of the acid solution after the chemist has added 185.0 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.

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

An analytical chemist is titrating 64.8mL of a 0.3000M solution of ammonia NH3 with a 0.7300M solution of HNO3 . The pKb of ammonia is 4.74 . Calculate the pH of the base solution after the chemist has added 31.6mL 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 77.9 mL of a 1.000M solution of hydrazoic acid (HN₂) with a 0.9800M solution of NaOH. The pK, of hydrazoic acid is 4.72. Calculate the pH of the acid solution after the chemist has added 34.3 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 = 0 X $

An analytical chemist is titrating 111.5 mL of a 0.2600M solution of acetic acid (HCH,CO,) with a 0.5100M solution of NaOH. The p K, of acetic acid is 4.70. Calculate the pH of the acid solution after the chemist has added 10.45 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 An analytical chemist is titrating 69.9 mL of a 0.2200M solution of cyanic acid (HCNO) with a 0.8900M solution of KOH. The pK of cyanic acid is 3.46. Calculate the pH of the acid solution after the chemist has added 5.93 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 0 X Ś

Nitesh

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 146.0 mL of a 1.200 M solution of benzoic acid (HC6H5CO₂) with a 0.6900 M solution of NaOH. The pK of benzoic acid is 4.20. Calculate the pH of the acid solution after the chemist has added 46.25 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 = 0 ×