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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. 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

  6. 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

  7. 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

  8. 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.

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

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

  11. [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

  12. 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

  13. The American Medical Association announced today that the Universal Choking Sign has been revised:

  14. Old Sign:

  15. New Sign:

  16. Calvin’s Approach to Math in Chemistry:

  17. Get Your Clicker!!!

  18. 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

  19. 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

  20. 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

  21. 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

  22. 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

  23. 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

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

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

  26. [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

  27. 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

  28. 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

  29. 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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