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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:

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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 up1
Warm-Up
  • Write formulas for the following acids:
    • Hydroiodic Acid
    • Carbonic Acid
    • Hydrosulfuric Acid
    • Nitrous acid
poh and titrations

pOH andTitrations

Acids and Bases, Day 3

Whitaker

17 December 2013

slide4
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
REMEMBER!!
  • The molarity of an acid is the Hydrogen (or Hydronium) ion concentration!
  • The molarity of a base is the Hydroxide ion concentration!
example
Example
  • Calculate the pOH for a solution of NaOH with a concentration of 1 x 10-4 M.
  • pOH = -log[OH-]
  • pOH = 4
example1
Example
  • Calculate the pOH for a solution of KOH with a concentration of 0.01 M.
  • pOH = -log[OH-]
  • pOH = 2
example2
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
pH and pOH
  • As the concentration of [H+] or [OH-] goes up, the other must go down.
    • pH + pOH = 14
example3
Example
  • What is the pH of a solution that is found to have a pOH of 10?
  • pH = 4
example4
Example
  • What is the pH of a 0.001 M solution of LiOH?
  • pOH = 3
  • pH = 11
example5
Example
  • What is the pOH of a 0.0001 M solution of HCl?
  • pH = 4
  • pOH = 10
slide13

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?
objectives
Objectives
  • Define aspects of a titration.
  • Calculate the molarity of a solution using titrations.
warm up2
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 up3
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

Titrations and Indicators

Acids and Bases

Whitaker

18 December 2013

titrations
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
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
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
Parts of the Burette

Buret containing base or acid

Buret clamp

Stop-cock

Flask

Acid or base and indicator

a little more math
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
example6
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

example7
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
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
Different Types of Acids
  • Monoprotic
    • Contains one Hydrogen
    • HCl
  • Diprotic
    • Contains two Hydrogens
    • H2SO4
  • Triprotic
    • Contains 3 Hydrogens
    • H3PO4
changes to math
Changes to Math
  • When doing titrations, you must account for di- or triprotic acids by adding a 2 or 3 to the acid side.
example8
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?