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Complexometric determination of nickel

Complexometric

EDTA

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Complexometric titration » EDTA - titration of nickel

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general remarks

Nickel is titrated with EDTA against murexide. At the beginning of the titration solution should have low ammonia concentration, increased near the end point. This procedure enhances color change at the end point. Reaction between EDTA and Ni2+ ions is relatively slow, so titration should be carried out slightly slower than in other direct EDTA determinations.

EDTA reacts in the same conditions with Cu2+ and Co2+ as well. They should be removed or masked before the titration.

reaction

Reaction taking place during titration is

Ni2+ + EDTA4- → NiEDTA2-

sample size

For 0.01 M titrant and assuming 50 mL burette, aliquot taken for titration should contain about 0.35-0.45 millimoles of nickel (20-26 mg). If preparation of such sample is difficult, we can use different EDTA concentration.

end point detection

End point of nickel titration is easily detected with murexide. Murexide solutions are not stable and should be not stored longer than a week.

solutions used

To perform titration we will need titrant - 0.01 M EDTA solution, 10% ammonium chloride and concentrated ammonium solution. We will also need indicator - either in the form of solution, or ground with NaCl - 100 mg of indicator plus 20 g of analytical grade NaCl.

procedure

result calculation

Calculation of EDTA titration results is always easy, as EDTA reacts with all metal ions in 1:1 ratio:

Ni2+ + EDTA4- → NiEDTA2-

That means number of moles of nickel is exactly that of number of moles of EDTA used.

To calculate nickel solution concentration use EBAS - stoichiometry calculator. Download determination of nickel reaction file, open it with the free trial version of the stoichiometry calculator.

Click n=CV button above EDTA4+ in the input frame, enter volume and concentration of the titrant used. Click Use button. Read mass of nickel in the titrated sample in the output frame.

sources of errors

In general this is a simple titration, with no other problems then those listed as general sources of titration errors.


Page was last modified on September 06 2009, 00:14:15.

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