Acidity and Basicity of Boric Acid
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Boric acid, H3BO3, is found in some laundry detergents, antimicrobials, and pesticides. With a Ka = 5.8 x 10^-10 it is a weak acid that behaves as a monoprotic acid. Assume you titrate 20.0 mL of 0.11 M boric acid with 0.100 M NaOH. (Show work)
1. Write the equation:
2. What is the pH of the solution before titration begins?
3. Write the equation for the system the equivalence point.
4. What is the pH at the equivalence point?
5. What is the pH at the midpoint of the titration?
6. What is the pH of the solution after adding 5mL of NaOH?
7. What is the pH of the solution after adding 10 mL of NaOH?
8. What is the pH of the solution after adding 11 ml of NaOH?
9. What is the pH of the solution after adding 10 mL of NaOH?
10. What is the pH of the solution after adding 22 mL of NaOH?
11. What is the pH of the solution after adding 25 mL of NaoH?
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Solution Summary
This handwritten solution contains step-by-step calculations which determine the pH of the solution after the addition of a specific amount of NaOH in each case. All formulas and workings are included.
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