Warm-Up

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# Warm-Up - PowerPoint PPT Presentation

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
• 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:
• Hydroiodic Acid
• Carbonic Acid
• Hydrosulfuric Acid
• Nitrous acid

### pOH andTitrations

Acids and Bases, Day 3

Whitaker

17 December 2013

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
REMEMBER!!
• The molarity of an acid is the Hydrogen (or Hydronium) ion concentration!
• The molarity of a base is the Hydroxide ion concentration!
Example
• Calculate the pOH for a solution of NaOH with a concentration of 1 x 10-4 M.
• pOH = -log[OH-]
• pOH = 4
Example
• Calculate the pOH for a solution of KOH with a concentration of 0.01 M.
• pOH = -log[OH-]
• pOH = 2
Example
• What is the concentration of a basic solution that has a pOH of 13?
• [OH-] = 10-pOH
• [OH-] = 1 x 10 -13 M
pH and pOH
• As the concentration of [H+] or [OH-] goes up, the other must go down.
• pH + pOH = 14
Example
• What is the pH of a solution that is found to have a pOH of 10?
• pH = 4
Example
• What is the pH of a 0.001 M solution of LiOH?
• pOH = 3
• pH = 11
Example
• What is the pOH of a 0.0001 M solution of HCl?
• pH = 4
• pOH = 10
• 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?
Objectives
• Define aspects of a titration.
• Calculate the molarity of a solution using titrations.
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
• 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?

### Titrations and Indicators

Acids and Bases

Whitaker

18 December 2013

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.
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
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.
Parts of the Burette

Buret containing base or acid

Buret clamp

Stop-cock

Acid or base and indicator

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
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

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

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?
Different Types of Acids
• Monoprotic
• Contains one Hydrogen
• HCl
• Diprotic
• Contains two Hydrogens
• H2SO4
• Triprotic
• Contains 3 Hydrogens
• H3PO4
Changes to Math
• When doing titrations, you must account for di- or triprotic acids by adding a 2 or 3 to the acid side.
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?