tag:blogger.com,1999:blog-3998325682836029850.post596720717122191993..comments2023-10-20T14:15:04.652+02:00Comments on The Rocket Blog: How to make ammonium perchlorate : electrolysisAnonymoushttp://www.blogger.com/profile/14841069838724705875noreply@blogger.comBlogger25125tag:blogger.com,1999:blog-3998325682836029850.post-85063736709613810052021-08-16T21:15:26.245+02:002021-08-16T21:15:26.245+02:00Try to keep the solution cool or it will eat the p...Try to keep the solution cool or it will eat the platinum coated titanium cathode, if that happens you will still see bubbles but it will stop making chlorates and perchlorates. The best to use for an anode is lead dioxide anode it will stand up the to sodium the best. I might make a video on perchlorates at some point. Here is my Bitchute channel https://www.bitchute.com/channel/JJNI53eMMLUy/ Also you may want to try the membrane style cell. D.B.https://www.blogger.com/profile/11156277678800230283noreply@blogger.comtag:blogger.com,1999:blog-3998325682836029850.post-29754610251923193472021-08-16T19:16:43.407+02:002021-08-16T19:16:43.407+02:00These days i just buy it to avoid making ammonium ...These days i just buy it to avoid making ammonium chlorate because its dangerous stuff and can burn on its own with out any added fuel. Here is a link to a good place to buy ammonium perchlorate and lots of other good stuff. https://www.pyrochemsource.com/Ammonium-Perchlorate-400-micron_p_91.html D.B.https://www.blogger.com/profile/11156277678800230283noreply@blogger.comtag:blogger.com,1999:blog-3998325682836029850.post-33245110908944879292021-08-16T19:09:46.047+02:002021-08-16T19:09:46.047+02:00Did you use iodized salt? You must use pure sodium...Did you use iodized salt? You must use pure sodium chloride. You must use either platinum coated titanium cathode, or MMO cathode. I had luck using platinum coated titanium cathode and stainless steel anode. The only other thing I can think of is something was wrong with the methylene blue, it should have turned purple and you should have seen a small amount of precipitate. D.B.https://www.blogger.com/profile/11156277678800230283noreply@blogger.comtag:blogger.com,1999:blog-3998325682836029850.post-33411053106052468642019-03-14T14:57:05.306+01:002019-03-14T14:57:05.306+01:00You may search for our products through the search...You may search for our products through the search bar on our website. If you would like to receive a copy of our product catalog, please contact us at info@alfa-chemistry.com. <a href="http://www.alfa-chemistry.com/1-hexyl-2-3-dimethylimidazolium-perchlorate-item-296362.htm" rel="nofollow">1-hexyl-2,3-dimethylimidazolium perchlorate</a><br />alfachemistryhttps://www.blogger.com/profile/05704541170361426886noreply@blogger.comtag:blogger.com,1999:blog-3998325682836029850.post-23727185674412982742017-05-29T15:31:24.556+02:002017-05-29T15:31:24.556+02:00I cant find your other post where you cover what t...I cant find your other post where you cover what to use as electrodes, so which one is the anode and which the cathode? Thanks in advanceAnonymoushttps://www.blogger.com/profile/08525980440282286536noreply@blogger.comtag:blogger.com,1999:blog-3998325682836029850.post-40267328356996977402016-07-21T20:50:38.353+02:002016-07-21T20:50:38.353+02:00Those two are the only one I know that works. You ...Those two are the only one I know that works. You could try other materials like steel but it's unlikely to get the job done because it would leach out the iron into the solution (giving you a nice green solution) instead of oxidizing the chloride ion to chlorate and perchlorate ions.Anonymoushttps://www.blogger.com/profile/14841069838724705875noreply@blogger.comtag:blogger.com,1999:blog-3998325682836029850.post-14227557050906240192016-07-21T20:35:52.624+02:002016-07-21T20:35:52.624+02:00This may be dumb to ask but do the electrodes have...This may be dumb to ask but do the electrodes have to be lead dioxide and graphite? Or is there any substitutes for these electrodes?Anonymoushttps://www.blogger.com/profile/14031493030992559996noreply@blogger.comtag:blogger.com,1999:blog-3998325682836029850.post-88648536955458571502016-05-16T20:01:57.400+02:002016-05-16T20:01:57.400+02:00I should have said can not be burned by low concen...I should have said can not be burned by low concentrations of sulfuric acid. When I used 98% it smokes and some not all turns yellow but dose not burn. D.B.https://www.blogger.com/profile/11156277678800230283noreply@blogger.comtag:blogger.com,1999:blog-3998325682836029850.post-39865019096055300992016-04-30T03:04:43.548+02:002016-04-30T03:04:43.548+02:00I made my ammonium chloride so that my be the prob...I made my ammonium chloride so that my be the problem. I used ammonia and hydrochloric acid to form that salt. Like in this video. https://www.youtube.com/watch?v=Nj_J1U4l_Q0D.B.https://www.blogger.com/profile/11156277678800230283noreply@blogger.comtag:blogger.com,1999:blog-3998325682836029850.post-11192180089095991502016-04-30T03:03:03.977+02:002016-04-30T03:03:03.977+02:00This comment has been removed by the author.D.B.https://www.blogger.com/profile/11156277678800230283noreply@blogger.comtag:blogger.com,1999:blog-3998325682836029850.post-86330560958496287972016-04-30T02:55:45.861+02:002016-04-30T02:55:45.861+02:00It is perchlorate that can not be burned by sulfur...It is perchlorate that can not be burned by sulfuric acid. I ran my cell for a week then boiled down the sodium hypochlorite into sodium chlorate then placed it back in the cell for 5 more days then destroyed the remaining chlorate with hydrochloric acid and a boiling process. like on this page > http://www.oocities.org/capecanaveral/campus/5361/chlorate/destroy.html So i know i have perchlorate not chlorate. D.B.https://www.blogger.com/profile/11156277678800230283noreply@blogger.comtag:blogger.com,1999:blog-3998325682836029850.post-65796371559411867972016-04-30T02:41:42.108+02:002016-04-30T02:41:42.108+02:00you must 1st destroy any chlorate remaining b4 yo...you must 1st destroy any chlorate remaining b4 you can start making the (ammonium perchlorate) or you will end up with some (ammonium chlorate) that could set the hole thing off causing injury or death. Here are some ways to do it. http://www.oocities.org/capecanaveral/campus/5361/chlorate/destroy.htmlD.B.https://www.blogger.com/profile/11156277678800230283noreply@blogger.comtag:blogger.com,1999:blog-3998325682836029850.post-10457372339067028212016-04-29T19:19:27.155+02:002016-04-29T19:19:27.155+02:00I think that your product is ammonium chlorate whi...I think that your product is ammonium chlorate which is soluble in water, hence no precipitation.<br />On the other hand, potassium chlorate is insoluble and precipitates, so it should explain why it works with potassium but not ammonium.<br />I suggest that you let your electrolysis run longer to see if it works with ammonium chloride.Anonymoushttps://www.blogger.com/profile/14841069838724705875noreply@blogger.comtag:blogger.com,1999:blog-3998325682836029850.post-36888860399354446682016-04-29T19:13:34.486+02:002016-04-29T19:13:34.486+02:00You could use other salts for the double decomposi...You could use other salts for the double decomposition step such as sulfate.<br />However, you will end up with a different sodium salt in solution after that.<br />For example, if you use ammonium sulfate, then the solution will contain sodium sulfate and thus won't be reusable (chloride is needed for electrolysis).<br />If you don't care about reusing your electrolyte, you could try it but I've never done that, so I can't say if it will be successful.Anonymoushttps://www.blogger.com/profile/14841069838724705875noreply@blogger.comtag:blogger.com,1999:blog-3998325682836029850.post-5201944867048338822016-04-29T18:14:05.418+02:002016-04-29T18:14:05.418+02:00Also what other ammonia salts can be used? Also what other ammonia salts can be used? D.B.https://www.blogger.com/profile/11156277678800230283noreply@blogger.comtag:blogger.com,1999:blog-3998325682836029850.post-82742679523534437992016-04-29T18:11:48.617+02:002016-04-29T18:11:48.617+02:00I mixed the sodium perchlorate with the ammonium c...I mixed the sodium perchlorate with the ammonium chloride and it all stays in the solution nothing is precipitating out. It worked well when i used potassium chloride but not with the ammonium chloride. What do you recommend? D.B.https://www.blogger.com/profile/11156277678800230283noreply@blogger.comtag:blogger.com,1999:blog-3998325682836029850.post-17687850007773706592015-06-14T21:38:27.459+02:002015-06-14T21:38:27.459+02:00I just wanted to clear this process up, as i like ...I just wanted to clear this process up, as i like to double check all of the procedures before hand<br /><br />1. NaCl is dissolved into water<br />2. Lead Dioxide and graphite electrodes are used in electrolysis <br />now i am not sure what is to be done here, as from what i gather i just take the sodium chlorate and use it as electronlite then i add in ammonunium or pottasium chloride and scoop off the resulting preciptate. <br /><br />Is this correct? sorry for this dumb question but i would just like to clear up the process.Anonymoushttps://www.blogger.com/profile/00155399710441762530noreply@blogger.comtag:blogger.com,1999:blog-3998325682836029850.post-66179368370190038952015-04-05T12:34:28.894+02:002015-04-05T12:34:28.894+02:00thank you.
I'm from Korea, Korean amature atte...thank you.<br />I'm from Korea, Korean amature attempt KNSB or KNSU.<br /><br />I learn about it.<br /><br />I hope you to visit my blog.<br /><br />http://blog.naver.com/jetspaceshipAnonymoushttps://www.blogger.com/profile/00812295295118604206noreply@blogger.comtag:blogger.com,1999:blog-3998325682836029850.post-86365005815838070562014-09-06T10:56:18.513+02:002014-09-06T10:56:18.513+02:00Well, for the voltage, there is actually no prescr...Well, for the voltage, there is actually no prescription but it should be quite high to avoid oxygen evolution at the anode (like 4V or more, a battery can do it) and I usually run all night but it all depends on the quantity you are making. The lower the quantity, the lower the time and vice-versa.Anonymoushttps://www.blogger.com/profile/14841069838724705875noreply@blogger.comtag:blogger.com,1999:blog-3998325682836029850.post-79186341796646248552014-09-06T03:30:15.397+02:002014-09-06T03:30:15.397+02:00Thanks for you help. Sorry to keep asking questio...Thanks for you help. Sorry to keep asking question I just have two more I need to ask , would I need to run the cell with the save current as I did to make the electrodes? How long does it need to run.<br />Anonymoushttps://www.blogger.com/profile/08412284550595164639noreply@blogger.comtag:blogger.com,1999:blog-3998325682836029850.post-89106192645869451902014-09-04T15:28:36.565+02:002014-09-04T15:28:36.565+02:00Hello,
Actually, you don't have to do this bec...Hello,<br />Actually, you don't have to do this because one of the useful characteristics it has, besides its powerful oxidizing power, is that it is insoluble in water.<br />So when you add ammonium chloride to your sodium perchlorate solution, AP will precipitate out of solution.<br />You just have to filter out the AP and you can also reuse the solution for another batch.Anonymoushttps://www.blogger.com/profile/14841069838724705875noreply@blogger.comtag:blogger.com,1999:blog-3998325682836029850.post-37492821573982558512014-09-04T03:46:40.156+02:002014-09-04T03:46:40.156+02:00How would I extract the AP from the solution? I wa...How would I extract the AP from the solution? I was thinking boiling could work or would that cause the AP to decompose. Anonymoushttps://www.blogger.com/profile/08412284550595164639noreply@blogger.comtag:blogger.com,1999:blog-3998325682836029850.post-2244710642155739882014-07-10T02:06:20.517+02:002014-07-10T02:06:20.517+02:00This comment has been removed by the author.Anonymoushttps://www.blogger.com/profile/08412284550595164639noreply@blogger.comtag:blogger.com,1999:blog-3998325682836029850.post-37872011175693742892014-06-15T00:24:49.067+02:002014-06-15T00:24:49.067+02:00Thanks for your interest.
To answer you, you would...Thanks for your interest.<br />To answer you, you would need a stoichiometric amount of ammonium, or in non-chemist terms for 1 g of sodium perchlorate, you add 0.5 g of ammonium chloride.Anonymoushttps://www.blogger.com/profile/14841069838724705875noreply@blogger.comtag:blogger.com,1999:blog-3998325682836029850.post-92038610782401316302014-06-14T18:52:52.186+02:002014-06-14T18:52:52.186+02:00How much ammonium would need to be introduced per ...How much ammonium would need to be introduced per oz of sodium perchlorate solution. Anonymoushttps://www.blogger.com/profile/08412284550595164639noreply@blogger.com