Questions 15-20 refer to the same weak base/strong acid (WB/SA) titration. The Kb of pyridine is 1.7 x 10.⁹. A 40.00 mL solution of 0.700 M pyridine (C5H5N) is being titrated with 1.05 M hydrochloric acid (HCI). What will be the total solution volume (in mL) at the equivalence point? (Two decimal places) Type your answer...

The titration of 25.00 mL of 0.536 M of an unspecified diprotic weak acid (H2A) with 1.00 M potassium hydroxide (KOH).  Ka1 = 1.0 x 10-3 and Ka2 = 4.6 x 10-9. a) What volume of titrant (in mL) will be required to reach the second equivalence point?  (One decimal place) b) What will be the solution pH at the second equivalence point? c)  What will be the solution pH when 30.00 mL of titrant have been added?

When a 17.1 mL sample of a 0.353 M aqueous hypochlorous acid solution is titrated with a 0.401 M aqueous sodium hydroxide solution, (1) What is the pH at the midpoint in the titration? (2) What is the pH at the equivalence point of the titration? (3) What is the pH after 22.6 mL of sodium hydroxide have been added? Only typed solution

O ACIDS AND BASES Calculating the pH of a weak acid titrated with a strong base pH An analytical chemist is titrating 240.9 mL of a 1.000M solution of butanoic acid (HC3H,CO₂) with a 0.2500M solution of NaOH. The pK of butanoic acid is 4.82. Calculate the pH of the acid solution after the chemist has added 630.6 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. = 0 X 1/5 S Sabrina