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Chemistry Forums for Students => Undergraduate General Chemistry Forum => Topic started by: sun725 on March 15, 2017, 06:38:03 AM

Title: Titration
Post by: sun725 on March 15, 2017, 06:38:03 AM

I have the following question:

50.00 mL of the solution (Fe²⁺ / Fe³⁺) consumes 13.73 mL of 0.01200 M EDTA when titrated at pH = 2.00.

50.00 mL of the solution (Fe²⁺ / Fe³⁺) consumes 29.62 mL of 0.01200 M EDTA when titrated at pH = 6.00.

What is the concentration (in ppm), respectively, Fe²⁺ and Fe³⁺ in the solution? (Remember that we assume that the density of water is equal to 1 g / mL when calculating the concentration in ppm (weight / volume)).

How to approach this question. Can anyone help me where to start in order for me to solve this question ...

Title: Re: Titration
Post by: Borek on March 15, 2017, 07:21:42 AM

What is being complexed at each pH?