1.A 25.8 mL aliquot of 0.03 M aqueous hydrochloric acid is titrated with 0.02 M NaOH (ac). What volume (mL) of the base is used when the equivalence point is reached? Place the procedure

15 16 17 Questions 15-20 refer to the same weak base/strong acid (WB/SA) titration. The K, of pyridine is 1.7 x 10. A 40.00 mL solution of 0.700 M pyridine (C5H5N) is being titrated with 1.05 M hydrochloric acid (HCI). What is the solution pH before the titration begins? (Two decimal places) Type your answer... Questions 15-20 refer to the same weak base/strong acid (WB/SA) titration. The K, of pyridine is 1.7 x 10¹⁹. A 40.00 mL solution of 0.700 M pyridine (C5H5N) is being titrated with 1.05 M hydrochloric acid (HCI). What volume (in mL) of titrant will have been added at the half-equivalence point? (Two decimal places) 18 Type your answer... Questions 15-20 refer to the same weak base/strong acid (WB/SA) titration. The K, of pyridine is 1.7 x 10⁹. A 40.00 mL solution of 0.700 M pyridine (C5H5N) is being titrated with 1.05 M hydrochloric acid (HCI). What is the solution when 15.00 mL of titrant have been added? (Two decimal places) Type your answer... DD Questions 15-20 refer to the…

c) A student titrated 50.0 mL of a 0.10 M solution of a certain weak acid with NaOH. The results aregiven in the graph above.I) What is the approximate pKa of the acid? II) What specific value from the graph is needed, in addition to the information in partc above, to calculate the molar concentration of the NaOH? III) Identify a pH value between 2.5 and 7.5 at which the concentration of the weak acid beingtitrated is less than the concentration of the conjugate base.

7. Solution 1 2 Acid CH3CO₂H CF3CO₂H Ka 1.75 × 10-5 1.0 × 10⁰ Acid-dissociation constants of two acids are listed in the table above. A 20. mL sample of a 0.10 M solution of each acid is titrated to the equivalence point with 20. mL of 0.10 M NaOH. Which of the following is a true statement about the pH of the solutions at the equivalence point? (A) Solution 1 has a higher pH at the equivalence point because CH3CO₂H is the stronger acid. (B) Solution 1 has a higher pH at the equivalence point because CH3CO₂H has the stronger conjugate base. (C) Solution 1 has a lower pH at the equivalence point because CH3CO₂H is the stronger acid. (D) Solution 1 has a lower pH at the equivalence point because CH3CO₂H has the stronger conjugate base.