A chemist titrates 140.0 mL of a 0.7683 M propionic acid (HC₂H₂CO₂) solution with 0.2764 MKOH solution at 25 °C. Calculate the pH at equivalence. The pk of propionic acid is 4.89. 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 = 0 X 5

A chemist titrates 110.0 mL of a 0.3453 M methylamine (CH3NH₂) solution with 0.7011 MHCl solution at 25 °C. Calculate the pH at equivalence. The pK, of methylamine is 3.36. 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 = X S ?

A chemist titrates 100.0 mL of a 0.5181 M carbonic acid (H,CO, solution with 0.7276 M NaOH solution at 25 °C. Calculate the pH at equivalence. The p K, of carbonic acid is 3.60. 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.

A chemist titrates 190.0 mL of a 0.5701 M methylamine (CH3NH₂) solution with 0.4336M HNO3 solution at 25 °C. Calculate the pH at equivalence. The p K of methylamine is 3.36. 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 HNO3 solution added. -0 pH = X` S

A chemist titrates 130.0mL of a 0.6404M acetic acid (HCH3CO2) solution with 0.7306M NaOH solution at 25°C. Calculate the pH at equivalence. The pKa of acetic acid is 4.76.  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.

A chemist titrates 160.0 mL of a 0.6712M benzoic acid (HC6H5CO₂) solution with 0.6137M NaOH solution at 25 °C. Calculate the pH at equivalence. The pk of benzoic acid is 4.20. a 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 = X

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 *

A chemist titrates 50.0 mL of a 0.6961 M ammonia (NH3) solution with 0.1854M HCl solution at 25 °C. Calculate the pH at equivalence. The pk of ammonia is 4.75. 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 = X Ś

A chemist titrates 60.0 mL of a 0.7169M lidocaine (C14H2|NONH) solution with 0.4965 M HNO, solution at 25 °C. Calculate the pH at equivalence. The p Kb of lidocaine is 7.94. 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 HNO, solution added. pH %3D

What is the pH of a buffer solution that is 0.20 M methyl amine, CH3NH2 and 0.18 M methylammonium chloride CH3NH2Cl? The Kb for CH3NH2 is 4.4x10-4. You do not need to solve the quadratic equation for this problem. Express your answer to two decimal places.