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Author: Subject: Everyday Chemistry
JJay
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[*] posted on 28-12-2017 at 21:25


I am going to finally get around to titrating my nitric acid this evening after I put my equipment away. Most of my glassware items have a box that they belong in, but I have a dozen or so that do not... sometime later this week I am going to shop around for polystyrene sheets to make boxes to hold some of those pieces.



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JJay
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[*] posted on 29-12-2017 at 18:06


My nitric acid titrated at 48%.



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ninhydric1
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[*] posted on 29-12-2017 at 18:41


Prepared some zinc carbonate for a higher purity when it comes to preparing zinc compounds. I need some zinc acetate for a nanoparticle project of mine, but zinc chloride would be a useful compound for future organic chemistry reactions I might perform. I'm also going to need some silver nitrate, so I'm preparing for my first nitric acid distillation.



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TheNerdyFarmer
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[*] posted on 29-12-2017 at 19:26


Today, i tried my hand at making magnesium silicide and silane gas. I am making this for a future project which i plan on posting on here soon. Anyway, for the most part it failed. Only the outside of the reaction mixture actually reacted and all of the inside remained unreacted. It did, however, react to form some silane gas. I think that one reason that it didn't work well was that my magnesium was more like very fine small shavings rather than powder. (any ideas on how to make the powder? I was thinking perhaps ball milling in mineral oil, then washing the remaining mixture with acetone or toluene to get rid of the mineral oil. Secondly, I used a small butane torch to heat up the mixture. Butane is certainly capable of getting hot enough but the problem was in the size of the flame. Since I was using a small torch, the flame was only able to cover a small portion of the test tube at a time. Anyway, next time i think i am going to try propane because i have a propane torch that has a larger flame. I believe my next project will be to dry some methanol that i have with magnesium shavings/ribbon. (If anyone has a good source of reasonably affordable, quality 3A molecular sieves, or owns some that they want to sell, please U2U me). Molecular sieves would be ideal.. but sometimes you just gotta make do :P.

[Edited on 30-12-2017 by TheNerdyFarmer]
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mayko
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[*] posted on 1-1-2018 at 18:13


Took my first shot at pulling lithium out of batteries today; 1 of the two was a success :)
the other.... well.........




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j_sum1
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[*] posted on 5-1-2018 at 19:31


Attempted making nitric acid via the Tdep method using bisulfate. The process is a foaming nightmare and painfully slow. I don't think I'll be doing it again.



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[*] posted on 5-1-2018 at 23:03


Did you get any nitric to come over?
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j_sum1
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[*] posted on 5-1-2018 at 23:33


Well I haven't tested it yet but something came over woth a whole lot of NO2. I think it is RFNA but there may be some water in it.

The reaction ate my favourite stir bar. I guess it wasn't PTFE like I thought.




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JJay
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[*] posted on 9-1-2018 at 13:37


I checked three different stores and couldn't find any distilled water, so I'm distilling some water....



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JJay
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[*] posted on 9-1-2018 at 15:09


I figured that since I'm boiling some water I might as well calibrate my wildly inaccurate alcohol thermometer. I used a couple of data points in a boiling point calculator with the barometric pressure at the nearby airport and found that it is off by 4.8 degrees at 100 C!

I guess that's what you get for $1.75 with free shipping from China....




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JJay
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[*] posted on 11-1-2018 at 13:33


I'm distilling some muriatic acid to obtain pure azeotropic HCl for use in synthesis and as an acidimetric primary standard. I'll be monitoring barometric pressure carefully.

...

Now I have two 500 mL bottles of HCl, one labeled "20.2% (lab)" and one labeled "20.244% (lab best)."

[Edited on 12-1-2018 by JJay]




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j_sum1
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[*] posted on 13-1-2018 at 22:07


Distilled some hardware store toluene and then removed remaining water using a Dean Stark trap and Dimroth condenser.

There is something oddly satisfying about watching vapour fronts and condensation in a nice bit of glassware.




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[*] posted on 14-1-2018 at 01:52


Quote: Originally posted by JJay  

Now I have two 500 mL bottles of HCl, one labeled "20.2% (lab)" and one labeled "20.244% (lab best)."
[Edited on 12-1-2018 by JJay]


20.244% is an incredibly precise number




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[*] posted on 14-1-2018 at 06:21


Quote: Originally posted by JJay  
I'm distilling some muriatic acid to obtain pure azeotropic HCl for use in synthesis and as an acidimetric primary standard. I'll be monitoring barometric pressure carefully.

...

Now I have two 500 mL bottles of HCl, one labeled "20.2% (lab)" and one labeled "20.244% (lab best)."

[Edited on 12-1-2018 by JJay]


How did you measure the pressure that accurately?
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JJay
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[*] posted on 14-1-2018 at 10:21


The last digit is estimated using basic measurement theory (i.e. linear regression).



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ninhydric1
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[*] posted on 14-1-2018 at 12:12


Made some chloroform via haloform reaction, but might've made a chloroform-acetone azeotrope instead. Might need to do some washings or maybe a distillation.



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[*] posted on 14-1-2018 at 19:12


I made some solid iodine for the first time with potassium iodide, sodium bisulfate, and hydrogen peroxide. When I replenish my sodium bisulfate and potassium iodide, I will do this on a larger scale.
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