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The Chemistry of Acids and Bases

The Chemistry of Acids and Bases. Acids and Bases: Calculate pH/pOH At the conclusion of our time together, you should be able to:. Change any pH reading to pOH Convert pH to concentration of hydronium ion concentrations, hydronium ion concentrations to pH. Review of the pH Scale.

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The Chemistry of Acids and Bases

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  1. The Chemistry of Acids and Bases

  2. Acids and Bases: Calculate pH/pOHAt the conclusion of our time together, you should be able to: Change any pH reading to pOH Convert pH to concentration of hydronium ion concentrations, hydronium ion concentrations to pH

  3. Review of the pH Scale Since 1 mole of OH- in one Liter of water would be a pOH = 0 And the pH and pOH of water is 7 or neutral, Therefore, the pH of a strong base with a pOH of 0 would be pH = 14 Therefore, any pH can be converted to pOH by subtracting from 14.

  4. Examples of Converting pH If an acid has a pH of 3, what would be the pOH? 14 – 3 = 11 If an base has a pOH of 2, what would be the pH? 14 – 2 = 12

  5. A Former Student Trying to Apply His Knowledge of Chemistry!!

  6. Calculating the pH pH = - log [H+] (Remember that the [ ] mean Molarity) Example: If [H+] = 1 X 10-10pH = - log 1 X 10-10 pH = - (- 10) pH = 10 Example: If [H+] = 1.8 X 10-5pH = - log 1.8 X 10-5 pH = - (- 4.74) pH = 4.74

  7. pH Calculations – Solving for H+ on Worksheet#1 If the pH of Coke is 3.55, [H+] = ??? Because pH = - log [H+] then - pH = log [H+] Take antilog/inverse log (10x) of both sides and get 10-pH=[H+] [H+] = 10-3.55 = 2.82 x 10-4 M *** to find antilog/inverse on your calculator, look for “Shift” or “2nd function” and then the log button

  8. Worksheet #2, #3 • If an acid has a pH of 3.55, what would be the pOH? • 14 – 3.55 = • 10.45 • What is the concentration of OH-? [OH-] = 10-10.45 = • 3.55 x 10-11 M

  9. pH Calculations – #4 pOH = - log [OH-] pOH = - log [4.25 x 10-4] pOH = 3.37 pH = 14 – 3.37 = 10.63 A solution has a [OH-] of 4.25 x 10-4.

  10. pH [H+] [OH-] pOH

  11. Calvin’s Approach to Math in Chemistry:

  12. [OH-] 1.0 x 10-14 [OH-] 10-pOH 1.0 x 10-14 [H+] -Log[OH-] [H+] pOH 10-pH 14 - pOH -Log[H+] 14 - pH pH

  13. Acids and Bases: Calculate pH/pOHLet’s see if you can: Change any pH reading to pOH Convert pH to concentration of hydronium ion concentrations, hydronium ion concentrations to pH

  14. Get Your Clicker!!!

  15. If a solution has a pH of 6.5, what is the pOH of that same solution? • 4.5 • 7.5 • 6.5 • 0.0 • 12.5

  16. If a solution has a pH of 8.6, what is the [H+] of that solution? • 8.6 • 2.51 x 10-9 • 1.0 x 108.6 • 1.0 x 105.4 • 5.4

  17. If a solution has a pOH of 9.44, what is the [OH-] of that same solution? • 0.975 • 1.00 x 109.44 • 3.63 x 10-10 • 4.56 • 9.44

  18. If a solution has a [H3O+] of 6.20 x 10-8, what is the pH of that solution? • 6.79 • 8.79 • 5.21 • 4.56 • 7.21

  19. If a solution has a [OH-] of 1.05 x 10-3, what is the pH of that solution? • 11.02 • 2.98 • 1.00 • 3.02 • 10.98

  20. Acid Base Calculation Practice #1 • pH = 12.40, what would be the pOH? • 14 – 12.40 = • 1.60 • What is the concentration of OH-? [OH-] = 10-1.60 = • 0 0251 M

  21. Acid Base Calculation Practice #2 pOH? of 0.00162 M KOH pOH = - log 0.00162 = 2.79 pH = 14 – 2.79 = 11.21

  22. Converting pH to pOH If an acid has a pH of 6, what would be the pOH? 14 – 6 = 8

  23. [H3O+], [OH-] and pH What is the pH of the 0.0010 M NaOH solution? [OH-] = 0.0010 (or 1.0 X 10-3 M) pOH = - log 0.0010 pOH = 3 pH = 14 – 3 = 11

  24. Try These! The OH- ion concentration of a blood sample is 2.5 x 10-7 M. What is the pH of the blood? The pH of rainwater collected in a certain region of the northeastern United States on a particular day was 4.82. What is the H+ ion concentration of the rainwater? 1.51 x 10-5 pOH = 6.6 14.0 – 6.6 = 7.4 pH

  25. Calculating [H3O+], pH, [OH-], and pOH Problem 1: A chemist dilutes concentrated hydrochloric acid to make two solutions: (a) 3.0 M and (b) 0.0024 M. Calculate the [H3O+], pH, [OH-], and pOH of the two solutions at 25°C. [H3O+] = 3.0 M pH = -0.47 [OH-] = 3.388 x 10-15 M pOH = 14.47 [H3O+] = 0.0024 M pH = 2.6 [OH-] = 3.98 x 10-12 M pOH = 11.4

  26. Calculating [H3O+], pH, [OH-], and pOH Problem 2: What is the [H3O+], [OH-], and pOH of a solution with pH = 3.67? Is this an acid, base, or neutral? [H3O+] = 2.14 x 10-4 M pH = 3.67 [OH-] = 4.677 x 10-11 M pOH = 10.33

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