A titration of 16.67 mL of an unknown basic salt, NaA, requires 25.00 mL of 0.240 M HCI to reach the equivalence point. The titration data is shown below: Volume of HCI 5.30 mL 12.50 mL 20.00 mL 25.00 mL pH 10.54 9.97 9.37 What is the value of Ka for the weak acid, HA? 5.41

A titration of 16.67 mL of an unknown basic salt, NaA, requires 25.00 mL of 0.240 M HCI to reach the equivalence point. The titration data is shown below: Volume of HCI 5.30 mL 12.50 mL 20.00 mL 25.00 mL pH 10.54 9.97 9.37 What is the value of Ka for the weak acid, HA? 5.41

Chemistry

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ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter15: Acid-base Equilibria

Section: Chapter Questions

Problem 122CP: A 0.400-M solution of ammonia was titrated with hydrochloric acid to the equivalence point, where...

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Question

Please correct answer and don't use hand rating

A titration of 16.67 mL of an unknown basic salt, NaA, requires 25.00 mL of 0.240 M HCI to reach the equivalence point. The
titration data is shown below:
Volume of HCI 5.30 mL 12.50 mL 20.00 mL 25.00 mL
pH
10.54
9.97
9.37
What is the value of Ka for the weak acid, HA?
5.41

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When 40.00 mL of a weak monoprotic acid solution is titrated with 0.100-M NaOH, the equivalence point is reached when 35.00 mL base has been added. After 20.00 mL NaOH solution has been added, the titration mixture has a pH of 5.75. Calculate the ionization constant of the acid.
Ka for formic acid is 1.7 104 at 25C. A buffer is made by mixing 529 mL of 0.465 M formic acid, HCHO2, and 494 mL of 0.524 M sodium formate, NaCHO2. Calculate the pH of this solution at 25C after 110 mL of 0.152 M HCl has been added to this buffer.
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