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Titrations: A Laboratory Technique for Determining Analyte Concentration, Lecture notes of Chemistry

University of Babylon (UB)Chemistry

Titrations is an analytical method used to determine the concentration of an analyte by adding a precisely measured volume of titrant with known concentration and observing the equivalence point. the basics of titrations, including types of reactions, equivalence point vs end point, blank titration, and methods for determining the end point such as spectrophotometric detection and precipitation titration.

Typology: Lecture notes

2021/2022

Uploaded on 09/07/2022

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Titrations
•Titration is an analytical method in
which the concentration of an analyte
is determined by adding a precisely
measured volume of titrant of known
concentration and observing through
some means when an equivalence point
is reached
At equivalence point:
CunkVunk = CtitrantVtitrant
Titrations
•Titrations are usually used for one of
four types of reactions:
–Acid-base
–Oxidation-reduction
–Complex formation
–Precipitation
pf3
pf4
pf5
pf8

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  •  Titration is an analytical method in which the concentration of an analyte is determined by adding a precisely measured volume of titrant of known concentration and observing through some means when an equivalence point is reached At equivalence point: Cunk Vunk = Ctitrant Vtitrant

Titrations

  •  Titrations are usually used for one of four types of reactions: -  Acid-base -  Oxidation-reduction -  Complex formation -  Precipitation
  •  Equivalence point vs End point
  •  The equivalence point is that point in the titration when stoichiometric amounts of titrant and analyte have been added
  •  The end point is reached when we can observe a change in the solution
  •  The end point will be reached beyond the equivalence point

Titrations

Blank titration

  •  In a blank titration, analyte is not used
  •  The amount of titrant needed to reach the end point is measured
  •  This amount indicates the volume of titrant necessary to observe the physical change at the end point
  •  This volume is subtracted from the volume of titrant used in determination of the unknown
  •  There are other methods to determine the end point of a titration: Spectrophotometric detection Precipitation reactions Potentiometric detection

Titrations

Spectrophotometric detection

  •  Beer’s Law: A = b[X] A = absorbance (signal)  = molar absorptivity b = absorption path length [X] = molar concentration

Spectrophotometric detection

  •  If the analyte absorbs in the UV/vis spectral region, a spectrometer can be used to observe the progress of the titration -  Measure absorbance vs titrant added -  Correct absorbance measurements for change in volume -  Plot corrected absorbance vs titrant added

Titrations

Spectrophotometric detection Corrected absorbance—adjusts for dilution of solution

End point

Precipitation Titrations Before equivalence point: pAg = -log 10 [Ag +^ ]

Titrations

Precipitation Titrations At equivalence point: [Ag +^ ][I - ] = K (^) sp = 8.3 x 10 - [I - ] = [Ag +^ ] = (8.3 x 10 -17) 1/ = 9.1 x 10-9^ M pAg = 8.

Precipitation Titrations After equivalence point:

Titration Curve