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+.
2977views2rank - 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.
3405views - 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.
2566views - 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)
227views - Textbook Question
The pH of a buffer solution containing 0.10 M acetic acid and 0.10 M sodium acetate is 4.74.
a. Write the Henderson–Hasselbalch equation for this buffer.
693views - Textbook Question
One 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.
a. Write the Henderson-Hasselbalch equation for this buffer system.
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