10. Acids and Bases
Henderson-Hasselbalch Equation
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Practice this topic
- Multiple Choice
The Kb of C6H5NH2 (aniline) is 3.9 × 10−10. Determine pH of a buffer solution made up of 500 mL of 1.4 M C6H5NH2 and 230 mL of 2.3 M C6H5NH3+.
2642views2rank - Multiple Choice
Determine the buffer component concentration ratio (CB/WA) for a buffer with a pH of 4.7. Ka of boric acid (H3BO3) is 5.4 × 10−10.
2971views - Multiple Choice
Calculate mass of NaN3 that needs be added to 1.8 L of 0.35 M HN3 in order to make a buffer with a pH of 6.5. Ka of hydrazoic acid is 1.9 × 10−5.
2296views - Multiple Choice
Which of the following weak acid-conjugate base combinations would result in an ideal buffer solution with a pH of 9.4?
a) formic acid (HCHO2) and sodium formate (Ka = 1.8 x 10-4)
b) benzoic acid (HC7H5O2) and potassium benzoate (Ka = 6.5 x 10-5)
c) hydrocyanic acid (HCN) and lithium cyanide (Ka = 4.9 x 10-10)
d) iodic acid (HIO3) and sodium iodate (Ka = 1.7 x 10-1)
95views - Textbook QuestionThe pH of a buffer solution containing 0.10 M acetic acid and 0.10 M sodium acetate is 4.74. Write the Henderson–Hasselbalch equation for this buffer.325views
- Textbook QuestionOne of the buffer systems used to control the pH of blood involves the equilibrium between H₂PO₄⁻ and H₂PO₄²⁻. The pKₐ for H₂PO₄²⁻ is 7.21. Write the Henderson–Hasselbalch equation for this buffer system.322views