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I want to carry out chelation of citric acid and ZnSo4, Can I use boric acid to dissolve the ZnSo4 in it?

the method I need should be easy and costless and the materials should be costless and accessible

Dear All,

Big news flash there,

but it seems to be applicable and a better than TBE and TAE buffers, 10mM Sodium boric acid is used to separate bands up to 5Kbp.

less heat is generated compared to the regular buffers, thus, the voltage and be increased, reducing the time required for separation.

I'm going to imply this in my lab, yet, I'm confused about the ph of the boric acid and the agarose

regarding the latter, a low electroendosmosis agarose should be used, but what is a low EEO agarose anyway, cause the agarose we are using now has an eeo of .09 - .13 compared to an agarose labeled low EEO that its value is 0.1 - 0.15.

So far, I have to get some sodium boric acid, prepare it in a molarity of 10mM (ph ????) and run a gel.

Any more info on the subject is appreciated, I feel this method should be more "out there".

Regards.

I have added 1g of citric to 4 g of zinc sulphate in the 100 ml of boric acid solution.Now, I want to know the actual reaction happening between them?

Is it possible the chelation formation (complexation) reaction between boric acid (H3BO3) and calcium citrate (Ca3(C6H5O7)2).? If so;

- How do I observe

- How do I characterize

- What is the ratio between boric acid and calcium citrate

- What is the effect of the acid (e.g nitric acid) on the chelation

Analytic

the acidity nature of Boric acid is not clearly mentioned in any of the websites.

https://chemistry.stackexchange.com/questions/10614/mechanism-of-acidity-boric-acid

https://en.wikipedia.org/wiki/Boric_acid

what are the ions of boric acid? in Bronsted sense, they would be

H₂BO₃^- ,HBO₃^2- , BO₃^3-

, the ions should be instead

H₃BO₃(OH)^- ,H₃BO₃(OH)₂^2-- , H₃BO₃(OH)₃^3-

Which of the following is true?

even if bronsted ions are formed ,if their water solvation bond appear more coordination-covalent character than hydrogen -bonding character,(which can easily happen since the ionic species is charged) then the ion would appear lewis-like as well.

is this the case here? is then, there exists no sharp boundary between Bronsted and Lewis acidity?

when powdered boric acid (dry) is heated to stove-top temperature, it melts into a viscous bubbling liquid. when the melt is frozen, transparent flakes of solidified boric acid is obtained. But if the flakes are left in room temperature in open air for a day or two, the flakes become opaque. Boric acid has quite low melting point. so, does it become opaque by devitrification, or by absorbing moisture

I am using the 5:4 5 mold borax with Boric acid combination to get higher boron % in water. The solution goes together at room temperature for the Boron % that i am looking for (5.121% boron). I am having an issue with it staying stable over time. After just a few days the storage container has a coat of what looks like salts or crystals. How can i avoid this happening. I have tried MEA and NaOH but neither have worked. Any suggestions?

I'm working on an experiment about ammonia emissions from agricultural soils and I'm supposed to use boric acid to trap the emitted ammonia which I have to titrate with anhydrous sulphuric acid to quantify the ammonia trapped but I don't know the type of indicator I am supposed to use. Does anyone know?