EDTA is a chelating agent and chelates metal ions, i.e. attaches metal ions to itself.
For the Cu titration,
taking the average value of the 7 trials for the volume of EDTA consumed, we get:
V EDTA (avg) = 16.90 mL
Assume that the tap water has a Cu2+ conc. of x moles/L
Volume of aliquot = 25 mL = 0.025 L
Moles of Cu2+ in this aliquot = 0.025*x moles
These many moles of EDTA will also be required for titration.
Lets say the standard EDTA solution used in this experiment has EDTA conc. of 'y' moles/L
Volume of EDTA consumed = 16.90 mL = 0.0169 L
Thus, moles of EDTA used = 0.0169*y moles
Equating we get:
0.0169*y = 0.025*x
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For the Pb2+ titration:
Lets assume that tap water has Pb2+ conc of 'x' moles/L,
standard EDTA solution has conc 'y' moles/L and standard
Mg2+ solution has conc. 'z' moles/L.
Moles of EDTA supplied = Volume*conc = 0.025*y
Moles of Pb2+ present = 0.050*x
Moles of EDTA left after the reaction of EDTA with Pb2+ = 0.025*y - 0.050*x
These many moles of Mg2+ are supplied from outside to react with EDTA.
Calculating the average volume of Mg solution used in titration from the 6 trials, we get;
V Mg (average) = 19.26 mL
Thus, moles of Mg2+ = 0.01926*z
Thus, equating we get:
0.01926 = 0.025*y - 0.050*x
Putting 'y' and 'z', we can calculate 'x'
This is for an analytical chemistry. Please show all work and excel sheets. Cu Determination (5...
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