titration introduction
DESCRIPTION
An introduction to titration--why we use it, the advantage of water solution chemistry, and acid-base, conductimetric and redox titrations.TRANSCRIPT
Titration
Using water solutions to make analytical work faster, easier and more
accurate
Mpcfaculty.net
Why Water Solutions?
Why do chemists prefer to conduct reactions in water solution?
Water is a “universal solvent” A true solution is homogeneous
Every mL solution mmoles = any other mL mmoles
Water is a non-conductor No “noise” obscuring conductivity titrations
Water is the product of most acid-base reactions Many interesting salts not soluble in water
Enables precipitation reactions
Types of Titration
Acid-base titration Requires a weak acid indicator for equivalence pt.
Oxidation-reduction titration Usually one or the other has a color change
Precipitation titration Difficult: equivalence point hard to spot (no ppt)
Conductimetric titration Relies on the different size of the ions reacted and
in excess
Acid-Base Titration
Indicator is one color at pH below the equivalence point and changes color close to equivalence point.
Problem: Titrating an unknown molarity of HCl (32.20 mL) with 0.0520 M NaOH reaches a color change at 25.04 mL base. What is molarity of acid?
Strong acid and strong base—what is equiv pH? Ma x Va = Mb x Vb so Ma = Mb x Vb Va Ma = (0.0520 M) x 25.04 mL = 0.0404 M acid 32.20 mL
Why Indicators Work If Chosen Properly
If the indicator's pKa is close to the equivalence pH, then the rapid change in pH around the equiv pt makes the indicator change colors like a stop light Titrations.info
Methyl orange changes colors just short of the equivalence pH of 7 when using strong acid and strong base
So methyl orange would be a decent indicator if you titrate base into acid. Would it work if you titrated acid into base?