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Topic: Titration Do Now: . Acid-Base Titration. A procedure used in order to determine the molarity of an acid or base K nown volume of a solution with a known concentration (standard solution) and k nown volume of unknown concentration and a M A V A = M B V B acid-base indicator needed.

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acid base titration
Acid-Base Titration
  • A procedure used in order to determine the molarity of an acid or base
  • Known volume of a solution with a known concentration (standard solution) and known volume of unknown concentration and a
  • MAVA = MBVB
  • acid-base indicator needed
titration
Titration
  • Standard solution slowly added to unknown solution
  • As solutions mix:
    • neutralization reaction occurs
  • Eventually:
    • enough standard solution is added to neutralize the unknown solution Equivalence point
equivalence point
Equivalence point

total # moles H+1 ions donated by acid equals

total # moles H+1 accepted by base

total moles H+1 = total moles OH-1

titration1
Titration
  • End-point = point at which indicator changes color
    • if indicator chosen correctly:
      • end-point very close to equivalence point
titration of a strong acid with a strong base
14-

Equivalence Pt 

0 ml

20 ml

Titration of a strong acid with a strong base

Phenolphthalein

Color change:

8.2 to 10 

pH

7-

0-

Volume of 0.100 M NaOH added (ml)

40ml

m h 1 v h 1 m oh 1 v oh 1
MH+1 VH+1= MOH-1 VOH-1
  • MH+1= molarity of H+1
  • MOH-1= molarity of OH-1
  • VH+1= volume of H+1
  • VOH-1= volume of OH-1
titration problem 1
Titration Problem #1
  • In a titration of 40.0 mL of a nitric acid solution, the end point is reached when 35.0mL of 0.100M NaOH is added

Calculate the concentration of the nitric acid solution

HNO3 + NaOH H2O + NaNO3

variables
Variables
  • # of H’s = 1
  • Ma= ?
  • Va = 40.0 mL
  • # of OH’s = 1
  • Mb = 0.100 M
  • Vb = 35.0 mL
titration problem 2
Titration Problem #2
  • What is the concentration of a hydrochloric acid solution if 50.0 mL of a 0.250M KOH solution is needed to neutralize 20.0mL of the HCl solution of unknown concentration?

KOH + HCl H2O + KCl

variables1
Variables
  • # of H’s = 1
  • Ma= X
  • Va = 20.0 mL
  • # of OH’s = 1
  • Mb = 0.250 M
  • Vb = 50.0 mL
titration problem 3
Titration Problem #3
  • What is the concentration of a sulfuric acid solution if 50.0mL of a 0.25 M KOH solution is needed to neutralize 20.0mL of the H2SO4 solution of unknown concentration?

H2SO4 + 2 KOH  2 H2O + K2SO4

variables2
Variables
  • # of H’s = 2
  • Ma= X
  • Va = 20.0mL
  • # of OH’s = 1
  • Mb = 0.25M
  • Vb = 50.0mL
slide16
(2)(X)(20.0ml) = (0.25M)(50.0ml)(1)

X = 0.3125 M H2SO4(sulfuric acid)

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