Find 3 other methods to increase EDTA selectivity rather :Control of pH,complexation,ppt of infering cations?
551829
EDTA has very little selectivity so I doubt you will find much more.Masking/demasking agents such as cyanide complexes,phosphate anions.. are nothing else than complexation examples.Another method is called kinetic masking; for example determination of Cr and Fe in steel sample solution (under cool condition,the EDTA will react with Fe first and after you heat the solution the EDTA will react with Cr).The choice of indicator might increase selectivity (different indicators have different reaction rate)but I'm not sure about that one...
139895
2 ways come to mind.\n\nYou make a series of solutions of increasing concentration as well as a blank (deionized water) and measure their absorbance in a spectrometer. You find a regression of the data and figure out the methylene blue based on its absorbance.\n\nStandard addition. You take unknown absorbance and add increasing concentrations of methylene blue to it. Graph the data and figure out the concetration corresponding to the y intercetp.
836016
Here is a good guide\n\nhttp://dbhs.wvusd.k12.ca.us/webdocs/Stoichiometry/Limiting-Reagent.html
528995
Hmmm, what exactly do you mean by INSTRUMENTAL techniques? As the guy before me said, you could titrate it against a strong coloured oxidising agent such as acidifies potassium permanganate. But you can't really get the concentration from a spectrophotometer, for example, since peroxide (H2O2) doesn't absorb light.\nI guess you could thry using a NMR spectrometer for the job, or some kind of chromatography, but titration is by far the safest and easyest.
860724
The link below gives a method and chromatogram.  Bear in mind that you will need to prevent the degradation of ascorbic acid during the analysis.  This may be done by adding EDTA and HCl to the solutions, but you will have to work out the concentrations.
382713
The best method is pH meter (other than color indicator). \nTo measur the exact end point, what you have to is:\n\nStart the titration\nInsert a pH probe inside the solution\nNow start adding base to the acid and swirl the solution properly\nKeep track of your pH readings..\nYou will see a sudden jump (some thing like from 5.6 to 9.0 even with one drop addition)\nthats end point.
877634
Any acid, for example:\n\nHCl + H2O  --> Cl- + H3O+
611075
I'm assuming you are extracting from an aqueous solvent?  Preferably, you want to increase the polarity of the aqueous solution, such that the solute has less affinity for water than it would for the organic solvent.  This can be done by "salting" the water (increasing the ionic strength by adding an inert salt, a la NaCl).  You then extract the solute with your organic solvent of choice, usually using smaller aliqouts more frequently vs. larger aliqouts (deals with partition coefficient, or how much will get extracted vs. how much remains in the water).  After extraction, the organic solution is usually dried (more often than not by MgSO4 or Na2SO4) and then the solvent is distilled off to yield hopefully pure product.
636906
Functionallizing the EDTA to make a substituted EDTA
789874
The method may depend upon what type of hydrolysis you performed: acid, base or enzyme.\n\nMost methods would depend upon measuring the increase of reducing sugar in the solution (these are aldehydes).  All of these methods are far more complicated than using the disappearance of the blue-black iodine-starch complex.
886413
Use three test tubes, put equal amout of enzymes in all and put the substance they digest in both (equal amounts of course).\n\ntake a test tube(A) and put 2cm3 of Hydrochloric acid.\nTake test tube (B) and put 2cm3 of Pure water(pH7).\nTake test tube (C) and put 2cm3 of Sodium Hydroxide.\n\nshake them all a little just as you start the test.\n\nLeave them for half an hour at their optimum temperature and other factors.Make sure all factors among them are equal.\n\nAfter that, Test for the substance you put in (e.g test for starch using iodine if you put starch in).\n\nThe one with the most negative result is the optimum pH.
899611
Ba(NO3)2 and sodium phosphate\n\n1.  Ba(NO3)2 + Na3PO4 --> NaNO3 + Ba3(PO4)2\n\n2.  Ba(+2) + NO3(-1) + Na(+1) + PO4(-3) --> Na(+1) + NO3(-1) + Ba(+2) + PO4(-3)\n\n3.  No reaction (All spectator ions cancel out)\n\nBa(NO3)2 and sodium carbonate\n\n1.  Ba(NO3)2 + Na2CO3 --> BaCO3 + NaNO3\n\n2.  Ba(+2) + NO3(-1) + Na(+1) + CO3(-2) --> BaCO3 + Na(+1) + NO3(-1)\n\n3.  Forms BaCO3 (Barium Carbonate)\n\n\nBa(NO3)2 and pottasium iodide\n\n1.  Ba(NO3)2 + KI --> BaI2 + KNO3 \n\n2.  Ba(+2) + NO3(-1) + K(+1) + I(-1) --> Ba(+2) + I(-1) + K(+1) + NO3(-1)\n\n3.  No reaction (All spectator ions cancel out)\n\nBa(NO3)2 and sodium sulfate\n\n1.  Ba(NO3)2 + Na2SO4 --> NaNO3 + BaSO4\n\n2.  Ba(+2) + NO3(-1) + Na(+1) + SO4(-2) --> Na(+1) + NO3(-1) + BaSO4\n\n3.  Forms BaSO4 (Barium Sulfate)\n\nHopes this helps you!
602416
http://www.scienceaid.co.uk/titration.html
1103124
See if these help\n\nhttp://www.rit.edu/~pac8612/webionex/website/\n\nhttp://www.dartmouth.edu/~chemlab/chem3-5/ionx1/overview/procedure.html\n\nhttp://www.culliganmiami.com/pf7.html\n\nhttp://www.wqa.org/sitelogic.cfm?id=1085
97043
The order should be\norganopotassium>organomagnesium>organomercury\n\nPotassium is the most electroposivite among these three metals ie potassium, magnesium, and mercury. Thus it will form K+ ion more easily then the other three. As a matter of fact, organic carbanion will form readily with organopotassium.\nHope this helps..
1102194
Hydrochloric acid is used for pH adjusting swimming pools.\n\nPhosphoric acid is in Coca Cola.
174013
Look up in preferred order: \n(1) Inductively coupled plasma mass spectrometry\n(2) Atomic absorption spectrometry\n(3) Anodic stripping analysis\n(4) Colorimetric methods for heavy metals