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Warm-Up

Warm-Up. What is the pH of a 0.00078 M solution of HI ? What is the pOH of a 0.045 M solution of NaOH ? What is the [H+] concentration of a solution of HBr that has a pH of 5.6? What is the pH of a 0.56 M solution of KOH?. Warm-Up. Write formulas for the following acids:

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Warm-Up

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  1. Warm-Up • What is the pH of a 0.00078 M solution of HI? • What is the pOH of a 0.045 M solution of NaOH? • What is the [H+] concentration of a solution of HBr that has a pH of 5.6? • What is the pH of a 0.56 M solution of KOH?

  2. Warm-Up • Write formulas for the following acids: • Hydroiodic Acid • Carbonic Acid • Hydrosulfuric Acid • Nitrous acid

  3. pOH andTitrations Acids and Bases, Day 3 Whitaker 17 December 2013

  4. pOH • Same as pH, but opposite. • Goes from 0 -14 • 0 - 6.99 is basic • 14 – 7.01 is acidic • pOH = -log[OH-] • [OH-]=10-pOH

  5. REMEMBER!! • The molarity of an acid is the Hydrogen (or Hydronium) ion concentration! • The molarity of a base is the Hydroxide ion concentration!

  6. Example • Calculate the pOH for a solution of NaOH with a concentration of 1 x 10-4 M. • pOH = -log[OH-] • pOH = 4

  7. Example • Calculate the pOH for a solution of KOH with a concentration of 0.01 M. • pOH = -log[OH-] • pOH = 2

  8. Example • What is the concentration of a basic solution that has a pOH of 13? • [OH-] = 10-pOH • [OH-] = 1 x 10 -13 M

  9. pH and pOH • As the concentration of [H+] or [OH-] goes up, the other must go down. • pH + pOH = 14

  10. Example • What is the pH of a solution that is found to have a pOH of 10? • pH = 4

  11. Example • What is the pH of a 0.001 M solution of LiOH? • pOH = 3 • pH = 11

  12. Example • What is the pOH of a 0.0001 M solution of HCl? • pH = 4 • pOH = 10

  13. What is the pH of a solution HI with a concentration of .001 M? • What is the concentration of a strong acid with a pH of 3? • What is the pH of a solution of a NaOH with a concentration of 1.0 x 10-6 M?

  14. Objectives • Define aspects of a titration. • Calculate the molarity of a solution using titrations.

  15. Warm-Up • What is the pH of a 0.00078 M solution of HI? • What is the pOH of a 0.045 M solution of NaOH? • What is the [H+] concentration of a solution of HBr that has a pH of 5.6? • What is the pH of a 0.56 M solution of KOH?

  16. Warm-up • What’s the pH of a 0.0001 M solution of NaOH? • What’s the molarity of HCl if the pOH is 13? • If it takes 55 mL of 0.001 M HCl to neutralize 122 mL of a NaOHsolution, what is the concentration of the NaOH solution?

  17. Titrations and Indicators Acids and Bases Whitaker 18 December 2013

  18. Titrations • A titration is a way of determining the molarity of an unknown solution by adding small volumes of a solution with a known molarity. • Involve neutralization reactions.

  19. Neutralization Reaction • Remember that when an acid and base mix, a salt and water are always produced! • Example: • NaOH + HCl -> NaCl + H2O • KOH + HI -> KI + H2O • H2SO4 + 2 LiOH -> Li2SO4 + 2 H2O

  20. Vocabulary of Titrations • The equivalence point - point where exactly enough titrant has been added to react with all of the analyte. • Indicator -a compound that changes color at certain pH’s.

  21. Parts of the Burette Buret containing base or acid Buret clamp Stop-cock Flask Acid or base and indicator

  22. A little more math!!! • In titrations we are looking for the concentration (Molarity) of an unknown solution. • M1V1= M2V2 • Where M1 is the molarity of the acid • V1 is the volume of the acid • M2 is the molarity of the base • V2 is the volume of the base

  23. Example • If it takes 54 mL of 0.1 M NaOH to neutralize 125 mL of an HCl solution, what is the concentration of the HCl? .0432 M

  24. Example • If it takes 25 mL of 0.05 M HCl to neutralize 345 mL of NaOH solution, what is the concentration of the NaOH solution? .0036 M

  25. Indicators!!!

  26. Review • [H30] = [??] • How do acids and bases taste? • What is a strong acid? • What does alkaline mean? • What is the “most basic” pH?? • Under what conditions do gases best dissolve?

  27. Different Types of Acids • Monoprotic • Contains one Hydrogen • HCl • Diprotic • Contains two Hydrogens • H2SO4 • Triprotic • Contains 3 Hydrogens • H3PO4

  28. Changes to Math • When doing titrations, you must account for di- or triprotic acids by adding a 2 or 3 to the acid side.

  29. Example • If it takes 50 mL of 0.5 M KOH solution to completely neutralize 125 mL of sulfuric acid solution (H2SO4), what is the concentration of the H2SO4 solution?

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