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EDTA Titration of Ca2+ and Mg2+ in Bottled Water

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  1. EDTA titration of Ca2+ and Mg2+ in bottled water
  2. Objective
  3. Procedure
  4. Apparatus
  5. Data and sample calculations
  6. Results and discussion
  7. Titration with EDTA using Hydroxynaphthol indicator

The objective of this experiment is to determine the total concentration of metal ions required to completely react with EDTA, or ethylene diamine tetra-acetate. The concentration determined will then be taken as the equivalent concentration of Ca2+ and Mg2+. Ca2+ will be analyzed separately in an additional titration after Mg(OH)2 has been precipitated from the solution using a strong base.

[...] The endpoint is indicated by the appearance of a blue tint in the solution. Repeat the titration at least three times more. Prepare a blank using distilled water and perform a blank titration. Record the result and subtract this number from the other volumes obtained in previous titrations. This blank can be used for both parts of the experiment. Calculate the total concentrations of Ca2+ and Mg2+, the individual concentrations of each ion, and the relative standard deviation of the replicate titrations. [...]


[...] Since this is in a 50 mL sample, the molarity of the ions is equal to: 7.36 x 10-5 moles of Ca2+ and Mg2+ = 0.0015 M 0.050 Liters Part II: Titration with EDTA using Hydroxynaphthol Indicator. The concentration of Ca2+ can be calculated from part two of the experiment in which Mg2+ is precipitated using a strong base. The concentration of Ca2+ is related to the number of moles of EDTA needed to reach the endpoint in the titration. [...]

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