Making Manganese Sulfate

[@CatboyChemicalSociety]

The beige color of the final product suggests iron impurity which can be removed by adding a bit of sodium hydroxide because iron hydroxide will precipitate first and keep adding till a bit of manganese hydroxide forms. Then filter it off and also you can use carbonate as it does the same forming iron carbonate first.

[@integral_chemistry]

Huh iron eh? I wonder where that could have come from.. Worth a shot to try and remove it I suppose.

[@CatboyChemicalSociety]

@@integral_chemistry manganese dioxide sometimes is contaminated with trace iron unless it was analytical grade. I know a few people who even if their manganese dioxide wasn't extracted from batteries was still heavily contaminated with iron because they sometimes just crush and package pyrolusite ore which is 90% MnO2 with some other stuff.

[@RghnutritionAus]

Mind checking out my comment regarding my synthesising... I've tried using sodium hydroxide and hydrogen peroxide to remove any iron impurities... But I still get a light green solution at the end

[@safety_first3579]

You're as impressive as NileRed! I don't understand how you don't have at least a million subscribers already. Keep up the good work.

[@integral_chemistry]

Thank you so much! I do try my best, and while I would be shocked having a million subscribers, I'm also a bit surprised by how few I have on here compared to my other accounts (I have 300k on tik tok as of now). That said, its at least a slow trickle so maybe someday, and I appreciate the support :)

[@safety_first3579]

@@integral_chemistry No problem!

[@experimental_chemistry]

Hm, the beige color of the product looks like there's a little Mn3+ or Mn4+ in there (often found in basic manganese carbonate) - and above all still a lot of moisture. What about drying on a steam bath or in an oven? Manganese sulphate normally is fine white and dusty powder with a slight hue of pink. MnO2 can easily be reduced by sodium bisufite in a solution of dill. sulfuric acid, too (only outdoors because a lot of SO2 is formed!). But then there's a problem with the residual sodium in the product, which maybe forms a Tutton's salt with MnSO4 on crystallization. But I only used this method for cleaning glassware from MnO2 so far, don't know if it works well for a synthesis, which I never considered to carry out, because MnSO4 is a very easy and cheap to optain chemical here.

[@EddieTheH]

Yeah, the H2SO4 is much more valuable to me than the Manganese product!

[@experimental_chemistry]

@@EddieTheH Strange world... And MnO2, too? Or extracted it from a battery?

[@EddieTheH]

@@experimental_chemistry Yeah, all my MnO2 comes from batteries. H2SO4 is insanely difficult to obtain here in the UK (legally, at least!). We're allowed a maximum concentration of 15%, as it's considered a dangerous corrosive liquid, but saturated hydroxide solutions are perfectly legal! It's insane!!!

[@integral_chemistry]

What is the basis for that restriction? Seems arbitrary.. Sulfuric acid sucks because its the most important acid (in my opinion) but by far the toughest to make yourself.

[@experimental_chemistry]

@@integral_chemistry It's restricted a precursor for making xplosives by nitration.

[@cioppicioppi6235]

Hi! great video! Could you explain me the role of H2SO4? The oxalic acid is the reducing agent in this case, but how should we define the acid? Is it used just to keep the Mn in solution as a Sulfate ? Thank you

[@integral_chemistry]

Thank you! Yeah the role of the sulfuric acid is basically to both catalyze the reduction of manganese dioxide, and subsequently dissolve it as it's sulfate salt. I suspect other strong acids could work here too, as well as other reducing agents other than oxalic acid (but I haven't actually tried any yet)

[@RghnutritionAus]

Hey mate, I tried this method before watching your video, I also tried using iron as a reducing agent along side the oxalic acid... However both times after filtering (and removing the iron) both of my solutions were light green instead of pink.... Any ideas what I'm doing wrong.. because I can't work it out for the life of me 😅 I'm using mnO2, sulfuric acid and oxalic acid in the same ratios Even tried filtering with activated carbon 🙄

[@mukonank783]

Well come to the rabbit hole.😂😂. I’ve been getting funny colours as well. I’m starting to think there’s a huge conspiracy out there where everyone is hiding one important step.

[@nikolaiturcan6963]

Nice work!

[@alirezaedalatbin6233]

hey, i wanna do some collaboration with you , how can i connect to you

[@danieljohanides2625]

Can formic acid be used insteed of oxalic acid?

[@integral_chemistry]

Maybe, but my concern would be that it might produce carbon monoxide instead of carbon dioxide