I want to use DMG as a reagent for detecting Ni in a solution. in their reaction they form a complex together which color is pink. I attached a picture of the reaction. my problem is I can`t find out about those two H+ at the end of the reaction. The reaction is not stoichiometry balanced. I will appreciate if anyone can help me with this. In addition I need to know what happen exactly between these two.
reference of the picture: Mentele, M. M.; Cunningham, J.; Koehler, K.; Volckens, J.; Henry, C. S. Anal. Chem. 2012, 84, 4474−4480.
The final complex is not pictured correctly. The loss of one proton occurs from one oxime group (NOH) on each of the two molecules of dimethylglyoxime. The reaction is performed in a solution buffered by either an ammonia or citrate buffer to prevent the pH of the solution from falling below 5. If the pH does become too low the equilibrium of the above reaction favours the dissolution of Ni(DMG)
The final complex is not pictured correctly. The loss of one proton occurs from one oxime group (NOH) on each of the two molecules of dimethylglyoxime. The reaction is performed in a solution buffered by either an ammonia or citrate buffer to prevent the pH of the solution from falling below 5. If the pH does become too low the equilibrium of the above reaction favours the dissolution of Ni(DMG)
Ma'am first the Bronsted base like ammonia abstract the proton and then complex formation take
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