A chemist titrates 90.0 mL of a 0.4988 M butanoic acid equivalence. The pK of butanoic acid is 4.82. 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 = X S (HC₂H₂CO₂) solution with 0.0732M KOH solution at 25 °C. Calculate the pH at ?

A chemist titrates 100.0 mL of a 0.3992 M ethylamine (C,H;NH,) solution with 0.6385 M HCl 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 =

A chemist titrates 50.0 mL of a 0.5456M carbonic acid (H₂CO3) solution with 0.1077M KOH solution at 25 °C. Calculate the pH at equivalence. The pKa 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 KOH solution added. pH = X

5. Please solve the following chemistry problem. 

A chemist titrates 90.0 mL of a 0.6900M ethylamine (C,H,NH,) solution with 0.0547M HNO, 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 HNO, solution added. pH = da Explanation Check O 2021 McGraw-H Education All Rights Reserved Terms of Use Pvacy Accessibity 會 APR 23 MacBook Air 20 888 FS esc & delete $ 8 5 2 E R T Y Q W F G

A chemist titrates 90.0 mL of a 0.7050M methylamine (CH3NH₂) solution with 0.5016M HBr 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 HBr solution added. pH = x 5 ?

Calculating the pH at equivalence of a titration solution A chemist titrates 170.0 mL of a 0.0884M pyridine (CHN) solution with 0.1089 M HNO3 solution at 25 °C. Calculate the pH at equivalence. The pK of pyridine is 8.77. b 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 added. pH = A பா

A chemist titrates 140.0 mL of a 0.1432M butanoic acid (HC3H₂CO₂) solution with 0.5600M KOH solution at 25 °C. Calculate the pH at equivalence. The PK of butanoic acid is 4.82. 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 KOH solution added.

A chemist titrates 110.0 mL of a 0.7452M aniline (C,H,NH,) solution with 0.5088M HCl solution at 25 °C. Calculate the pH at equivalence. The p K, of aniline is 4.87. 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 = ||

A chemist titrates 240.0 mL of a 0.3902 M lidocaine (C14H₂, NONH) solution with 0.7622 M HBr solution at 25 °C. Calculate the pH at equivalence. The pK 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 HBr solution added. pH = 0 X