I am performing an experiment in order to find the activation energy of EDTA chelation. Consequently, I need to measure the rate of reaction of the process. I am high school student, and so I do not have access to sophisticated equipment, although they might be unnecessary. However, I have been attempting to measure the volume of gas produced, but I am not achieving any result. So, can you suggest any other method to measure the rate of reaction? I would greatly appreciate the help since there is not a sufficient amount of information on the internet to help me get a clear answer, I have been working on the reaction for more than a month and a half.

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    $\begingroup$ It's too fast for you. $\endgroup$ – Mithoron Jun 25 '18 at 18:41
  • $\begingroup$ Thank you but it's quite the opposite. I mean it would be sufficient if I get a few values however I am not getting any. $\endgroup$ – Lina Jun 25 '18 at 19:28
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    $\begingroup$ sigh ZnCO3 is almost insoluble, so you decompose it with acid and expect it would tell you anything about subsequent complexation? Or what? Your query doesn't seem to make much sense. $\endgroup$ – Mithoron Jun 25 '18 at 19:54
  • $\begingroup$ Procedure: (I am using powdered Zn) ZnCO3 + C10H16N2O8 = C10H14N2O8Zn + CO2 + H2O 1. Pipette a 10 mL ( 0.05 mol dm-3) sample of the EDTA solution into a conical flask. 2. Add 5 mL of acidic buffer solution 3. Start the stopwatch when adding 4.49 g of ZnCO3. Given the Zn2+: EDTA ratio of 1:1 4. Stop the stopwatch when a certain volume of CO2 is reached 5.Repeat the experiment at 35 °C using a water bath. 6. Repeat steps 2,3,4,5 for the following temperatures:45 °C ,55 °C, 65 °C 7. Graph ln 1/t vs 1/T. 8. Find the activation energy of the reaction by using the Arrhenius equation. $\endgroup$ – Lina Jun 25 '18 at 20:53
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    $\begingroup$ All of these comments should not be comments, but part of the original question or an answer. $\endgroup$ – pentavalentcarbon Jun 26 '18 at 18:26

I think that the reaction will be too fast for you to measure with the tools in a high school lab. I think that you are not measuring the zinc binding to EDTA but instead making a measurement of the dissolution rate of zinc carbonate in an aqueous solution of EDTA.

If you were to want to measure the rate of the binding rate of zinc by EDTA the best way might be to use a radioactive tracer. I would start with radioactive zinc in an anionic EDTA solution. I would bring this into contact with a non-radioactive solution of zinc. I would then keep on pulling out small samples from the mixture and filtering them through an ion exchange resin which is able to remove either the anionic EDTA complex or the cationic form of zinc.

I would use zinc nitrate or some other form of zinc which does not tend to form anionic complexes when in solution.

I know that this experiment has been done as a teaching lab experiment in a nuclear chemistry unit with radioactive europium, but it has a reputation as a difficult experiment to do.

I suggest you read Williams, K.R.; Choppin, G.R., 1974, J. Inorg. Nucl. Chem., v. 36, no. 8, pp. 1849-1853. This has details of an experiment on the kinetics of metal exchange between EDTA complexes and "free unsolvated metal" for trivalent metals.

An alternative non radioactive method would be to use stopped flow experiments with a metal senstive indicactor present in the mixture. If we assume that the exchange of zinc between the solution and the indicator is very fast then this method could be of use.

Another method could be to take a solution of the zinc complex of EDTA and then treat it with C13 KCN, you could measure the C13 NMR spectrum again and again if it is a relatively slow process. But I think for you that you will be unable to deal with this problem with the chemcials and tools you have in a school lab. Sorry for having to pour some cold water around.

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  • $\begingroup$ Thank you for answering me! Well, I guess I will need to change my research question. Thank you for listing some sources and methods I will try to read them, because I want to understand how this will work. However, my experiment counts as 20% of my grade so I will need to change it. $\endgroup$ – Lina Jun 25 '18 at 21:50

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