DCHAS-L Discussion List Archive
From: Tammy M. Lutz-Rechtin <tlutzrec**At_Symbol_Here**UARK.EDU>
Subject: Re: [DCHAS-L] nitric acid distillation
Date: Wed, 14 Oct 2020 16:46:31 +0000
Reply-To: ACS Division of Chemical Health and Safety <DCHAS-L**At_Symbol_Here**Princeton.EDU>
Message-ID: DM6PR04MB3849E2BBCA0ED9EC639179C1BA050**At_Symbol_Here**DM6PR04MB3849.namprd04.prod.outlook.com
In-Reply-To
First of all, I wouldn't let them do this without a step-wise plan or SOP. What the student proposed is not a plan but a general description. How many ml, conc., time, what glassware and set-up, analysis, PPE, storage, waste, emergency response plan etc...
I suggest you require a JSA as well with two advising chemist approval required. Additionally, this should be done on a very small scale to start. Not to mention other regulations that may apply to production of this grade of fuel. Finally-Is this a risk
the university is willing to take? What is the value in a student doing this? For research on fuels? For fun?
Tammy Rechtin
From: ACS Division of Chemical Health and Safety <DCHAS-L**At_Symbol_Here**Princeton.EDU> on behalf of Laurie Yoder <laurie.yoder**At_Symbol_Here**EMU.EDU>
Sent: Wednesday, October 14, 2020 9:11 AM
To: DCHAS-L**At_Symbol_Here**Princeton.EDU <DCHAS-L**At_Symbol_Here**Princeton.EDU>
Subject: [DCHAS-L] nitric acid distillation
We have a senior chem student who has proposed making fuming nitric acid by reaction of fertilizer and concentrated sulfuric acid. (wants to make rocket fuel because this is what they do on youtube...) After my first "no way on earth are you
going to do this!" they looked up some safety information and sent me the "proposal", copied below. This is a highly motivated student who loves chemistry and legitimately wants to learn and try new things so I hate to shut them down without taking the opportunity
for education. My problem is that everything about this looks high-risk, and I need some help to sort it out to best communicate what the concerns are, other than "you're going to injure yourself and damage the property.."
My question for the group is what do you see as the top risks here and what would someone (in theory) need to do to mitigate them? I'm thinking (hoping!) it should become obvious to the student why we can't manage it here.
Thanks for your help!
Laurie
This is from the student:
"The reaction vessel will be a round bottom flask with a heater from there the gaseous nitric acid will run through a still cooled with ice water and covered with aluminum foil to minimize the breakdown of nitric acid into NO2 due to UV light. The product will
be collected in another round bottom flask and the excess NO2 and uncondensed Nitric acid will be bubbled through a water trap (we shouldn't use rubber tubing here).
"Products- Sodium Sulphate is a common fertilizer just like sodium nitrate the last of the acid in the reaction chamber can be neutralized and the waste can be easily disposed of as solid waste or mixed into the compost pile.
"Fuming Nitric Acid- This is the product we are interested in collecting. It will be used by XXX as the oxidizing agent in a model rocket. Fuming Nitric acid quickly destroys Nitrile gloves, setting them alight and melting them. For this reason an alternative
is necessary. Vinyl gloves deform a bit but do not melt or burn on contact with Fuming Nitric acid. Therefore obtaining Vinyl gloves and a Vinyl smock could also be a productive option. That said, direct skin contact with fuming Nitric acid is not as damaging
to the skin as solutions containing more water. As long as it is promptly removed working without gloves would potentially be a viable option. All work will take place in the hood because gaseous nitric acid and NO2 are continuously released. Once the Fuming
Nitric Acid is isolated it can be stored indefinitely in an amber glass container with a teflon sealed lid.
"Nitric acid from water trap- This product's density can be measured to determine its concentration. Then it can be stored in glass for use in other experiments.
"NO2 gas- We will do our best to minimize the production of this side product. Nitric acid breaks down into NO2 faster at high temperature and with more light. We will minimize the necessary temperature in the reaction pot, and ice the condensing regions and
product. All the glassware connections will be greased using the same sulfuric acid in the reaction pot which would be a good reason to wear vinyl gloves. This will seal the reaction with the overpressure continuously bubbling into the trap where more of
the gas can condense and the extra NO2 will be pumped out of the hood where the entire synthesis will occur.
"Additional considerations
Limiting personnel access- Because the Chemical prep room is the only hood which is off limits to most students during the day it would be the ideal location for this synthesis. 2 people will monitor the reaction at all times and eyewashes and a shower are
readily available. There is a designated fire extinguisher on hand and the labspace is not used too much so it can be cleaned up and sorted to meet our needs.
Eye protection- Eye protection will be worn at all times
"YouTube Sources
https://www.youtube.com/watch?v=QmCdrDLyNXQ&t=502s
https://www..youtube.com/watch?v=aUzMms62hKw
"Duke OESO Guidelines for Safe Use of
NITRIC ACID...[lots more copied and pasted stuff from internet...]
--
Laurie M. Yoder, PhD
Assistant Professor of Chemistry and Chemical Hygiene OfficerEastern
Mennonite University
540.432.4420
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