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Techniques for CollectorsNew "acid" to remove calcite from specimens
14th May 2009 19:50 UTCRory Howell
Looking for other ways to remove calcite and save the minerals, I have found a new "synthetic acid" that works great! The material is called EMS Barracuda Concrete Stripper, and is manufactured by Environmental Manufacturing Solutions. The material is very safe to handle, and the MSDS sheet lists it as 000 (non reactive, non corrosive, non flammable).
The material is an amber liquid, and has a slight "soapy" smell, but no fumes of any kind. It is safe on all metal I have tried it on, all clothes I have tried it on, and on counters, floors, etc. (tile grout would be affected though as it is basically calcite with sand). It is safe to handle - the only thing I noticed was a scratch I had from a rose bush stung slightly when my arm was in the liquid. As with all liquids and chemicals, I wear goggles, and if you were inclined to drink the stuff for some reason, the MSDS says that it may cause "loose bowels".
The barracuda dissolves more calcite per gallon than hydrochloric (but slower), and is much safer than any other way I have found to remove calcite chemically. When dissolving the calcite, it causes a very fine "foam" on the calcite as it dissolves. Like dish detergent, it causes a "foam cap", so you have to be careful to leave enough room in the bucket above the liquid level (it did clean all the dirt off my floor in the laundry room real good!). No fumes, no worrys about burns, etc. It did still affect the apatite and scapolite, but mostly just the luster - it did not turn them to "sand" like other acids have.
Unfortunately, the material did not do squat on removal of iron staining on any of the specimens I tried it on, so I am stuck with more aggresive chemicals for that.
I found the barracuda at a local concrete supply store - he had it in 250 gallon totes, but allowed me to buy 5 gallons at a time - cost was only slightly higher than hydrochloric adic would have been.
24th May 2009 00:30 UTCAlan Ions
i've personally found that a good automotive rust remover will get rid iron staining, but don't use it on soft minerals like malachite or azurite.
24th May 2009 12:43 UTCAnonymous User
Thanks for the information!!
Philippe.
24th May 2009 13:38 UTCJamison K Turnbull
24th May 2009 13:52 UTCAnonymous User
Also another example is http://www.mindat.org/photo-227271.html and http://www.mindat.org/photo-227272.html
These were on the same specimen, a large ~40 cm piece of host rock with much calcite. After HCl, I got about 5 specimens and the rest had nothing good. Before HCl, simply a big piece of calcite+rock with a bit of schorl, pyrite.
So I don't have before-after photos, but you can imagine how much calcite is removed - anywhere from 2 cm thick to 20 cm + Just depends on the vein size and how much calcite was kept on the specimen when it was removed.
Philippe.
24th May 2009 14:48 UTCGord Howe
Gord
24th May 2009 15:07 UTCMark D. Sherwood
Avoid skin contact.
Use in a well ventilated area.
Try a small sample or hidden corner for possible unintended effects before treating a valuable specimen.
Mark
25th May 2009 01:36 UTCRobert Simonoff
25th May 2009 17:53 UTCHenry Barwood
Henry Barwood
9th Jul 2009 20:21 UTCHenry Barwood
9th Jul 2009 20:53 UTCDavid Von Bargen Manager
They sell this stuff by 5 gallons:
http://orders.jpsupply.com/webapp/catalog/product/list.asp?line=B0012&C=CTW
Also http://www.enviromfg.com/howto.html has dealer lists for this.
10th Jul 2009 16:22 UTCHenry Barwood
Thanks for the information. I may have to accumulate a few specimens to warrant even a 5 Gal. pail.
10th Jul 2009 16:31 UTCDavid Von Bargen Manager
14th Jul 2009 00:41 UTCNeed to Know
14th Jul 2009 00:46 UTCDavid Von Bargen Manager
19th Jul 2009 08:37 UTCCostas Constantinides
8th Aug 2009 11:40 UTCPeter Haas
8th Aug 2009 16:51 UTCGeorg Graf
to remove Calcite I use Essigessenz = pure acetic acid, which you can buy in Germany in each supermarket in the "Spice" department (besides vine gear, olive oil, salt e.c.t.)
It is easy to handle, not very dangerous - don´t bring it in Your eyes! It is an acid!
And the generated Calcium-Acetate is soluble in water. You wash after cleaning Your spezimen in pure water and the acid and the Ca-Acetate is away.. Minerals like Apatite or Fluorite are not attacked, if You don´t let Your spezimen stay a long time in the acid.
I let normaly a small rest of the calcite on the spezimen, so You can see: Calcite was removed by acid.
Other carbonate minerals like Malachite, Dolomite and others are attacked or not, so You have no clear result. Normaly the are not totaly removed, but damaged.
Aragonite reacts with acetic acid like Calcite.
My Pyrochlore of the Kaiserstuhl (...photo-39996.html) was liberated from Calcite by acetic acid. Below the Pyrochlore You can see, unfortunately not sharp - an Apatite prism.
Greetings from Goslar
Georg
9th Aug 2009 10:57 UTCGeorg Graf
little bit more precise: Essigessenz is pur, 25%, acetig acid.
Greetings from Goslar
Georg
10th Aug 2009 21:24 UTCEd Drown
It seems that the "synthetic acid" is urea hydrochloride, as disclosed in a patent-infringement lawsuit filed by Peach State Labs against Environmental Manufacturing Systems.
(US District Court for the Northern District of Georgia, Rome Division; Filed Nov 26, 2008)
The disputed US patent is 5,672,279; "Method for Using Urea Hydrochloride".
The patent is fairly straightforward (for patents, that is) in describing how to prepare and use urea hydrochloride for the removal of calcium carbonate.
Ed
31st Aug 2009 04:09 UTChorsecore
Does the Barracuda product indicate what it is, specifically what type of acid, i.e. sulfamic acid or muriatic acid?
In my limited experience with cleaning copper with acids, it seems if you leave the specimen in the acid to long it can discolor the piece. Also, once the piece is removed from the acid, rinse it thoroughly with water and once rinsed towel dry followed by a hair dryer - be sure to remove all water as any remaining water seems to tarnish the piece.
Also, one trick is to soak the specimen in water after the acid bath - it helps take away the "new penny" shine that comes with acid cleaned copper. The length of soak time is strictly based on your taste.
I must compliment you on that Central piece you found in the stream - gorgeous! Any chance that piece is available?
Hope this helps a bit!
Ben
31st Aug 2009 04:19 UTCBen Vone
Feel free to drop me an e-mail Patrick - I always enjoy making contact with fellow Copper Country enthusiasts!
Ben
horsecore Wrote:
-------------------------------------------------------
> Hi Phillip,
>
> Does the Barracuda product indicate what it is,
> specifically what type of acid, i.e. sulfamic acid
> or muriatic acid?
>
> In my limited experience with cleaning copper with
> acids, it seems if you leave the specimen in the
> acid to long it can discolor the piece. Also,
> once the piece is removed from the acid, rinse it
> thoroughly with water and once rinsed towel dry
> followed by a hair dryer - be sure to remove all
> water as any remaining water seems to tarnish the
> piece.
>
> Also, one trick is to soak the specimen in water
> after the acid bath - it helps take away the "new
> penny" shine that comes with acid cleaned copper.
> The length of soak time is strictly based on your
> taste.
>
> I must compliment you on that Central piece you
> found in the stream - gorgeous! Any chance that
> piece is available?
>
> Hope this helps a bit!
>
> Ben
31st Aug 2009 13:17 UTCJolyon Ralph Founder
This makes no sense. If it is patented then the information must be available publically in the patent application documentation, and will probably be online. The whole point of patents is that you can't keep your invention secret.
If it's just a "trade secret" rather than a patent then there's no reason someone can't test it to find out what it is.
In any case I wouldn't suggest anyone put good mineral specimens into an unknown mixture of chemicals.
Jolyon
31st Aug 2009 14:20 UTCDavid Von Bargen Manager
http://patft.uspto.gov/netacgi/nph-Parser?Sect1=PTO1&Sect2=HITOFF&d=PALL&p=1&u=%2Fnetahtml%2FPTO%2Fsrchnum.htm&r=1&f=G&l=50&s1=5672279.PN.&OS=PN/5672279&RS=PN/5672279
1st Sep 2009 20:24 UTCPeter Haas
This is replacing a trade name with a trivial name that doesn't make any sense either ....
1st Sep 2009 21:51 UTCKnut Eldjarn 🌟 Manager
Knut
2nd Sep 2009 14:09 UTCPeter Haas
Urea will not survive being brought in contact with mineral acids in any conditions. It even hydrolyses in demineralized water; reaction will be complete within a couple of minutes at less than 60 °C. Acids considerably accelerate decomposition (H+ catalysis).
2nd Sep 2009 14:20 UTCAlfredo Petrov Manager
10th Sep 2009 04:15 UTCHoward Heitner
10th Sep 2009 07:18 UTCAlfredo Petrov Manager
11th Sep 2009 01:39 UTCHoward Heitner
12th Sep 2009 07:25 UTCAlfredo Petrov Manager
Nitric acid however should never be used for cleaning sulphides. Dilute HCl works fine on most sulphides. Almost all the abundant pyrite and sphalerite specimens from Peru on the market have been cleaned with HCl and, contrary to many peoples' expectations, the pyrite remains stable; the HCl does not cause it to decompose.
28th Sep 2009 17:15 UTCBill Browne
EMS does make a product that is very effective on rust stains.
It is called Players Choice. The link is:
http://www.enviromfg.com/pdf/Groundskeeper%20Literature.pdf
I suggest you try it.
EMS has over 100 products and can make custom formulations to meet a wide array of needs. We have used a number of them with great success. And they are totally GREEN.
21st Oct 2009 20:27 UTCjmac
Please see attached. One must know how to read a civil filing prior to passing judgment.
PSL "accused" EMS of this and never tested Barracuda nor did they ever make Barracuda or any of the other accuse products for EMS. This case was dismissed after investigation, depositions and a strong 40+ page order from the judge in Rome Georgia.
Our formula for Barracuda and many other products have been tested by NSF, certified as DfE worthy, have been evaluated by FDA experts and such. I can go one and one with valid governmental documentation such as a 96 page test from the US Department of Navy.
EMS has since file against PSL for patent invalidity. EMS sells in BULK thus I realize none of you would be paying customers however, if anyone wants a FREE sample of our Barracuda; please email me direct at jmac@enviromfg.com.
Thanks
26th Oct 2009 17:12 UTCEd Drown
Apologies for not responding sooner, it is good when a representative (I presume) for a company can answer questions about the use of their products. With regards to the documents referenced herein, they were located via a Google(TM) search and are believed to be but not necessarily represented as true copies.
coby.nixon.googlepages.com/PeachStateComplaint.pdf
shumakerindustries.com/pdf/Barracuda Literature.pdf
The filing by Peach State Labs, "PeachStateComplaint", dated November 26, 2008 is fairly clear. Bully for you in getting a dismissal. I do not recall, however, any assertions made in this forum as to the validity of PSL's claims. In their filing PSL did disclose their patent and therefore their active ingredient(s); which was germane to the topic under discussion, i.e. what type of "acid" is in "Barracuda". That question was not definitively answered in the PSL filing. It does appear, however, that they believed it to be urea hydrochloride.
It is all well and good for you to have NSF and FDA approvals for "Barracuda", do you have any documents from the US patent office (or WPO) that you can cite? The above referenced version of your product literature does have on its first page the claim that you have patented this "acid," quoting:
"Independent tests confirm that Barracuda, formed with EMS’ patented SynTech®, the world’s only synthetic acid, dissolves nearly 15% more concrete than Hydrochloric acid."
Which patent(s) covers "SynTech®"?
It seems to me that in this forum, marketing terms will not get one very far in having your product accepted by all as suitable for mineral cleaning and preparation. The statement in your brochure "It is safe on paint, chrome, aluminum, wiring, plastic and even glass." does not begin to cover the diverse chemistry that is encountered in this field. If your "synthetic acid" contains chloride ions, those that wish to use it to clean native copper for example, would want to take that into consideration when determining its suitability for use.
That is why the composition of "Barracuda" was and still is it seems, an open question and a concern to those who may wish to try it.
Any clarification that you can provide would be greatly appreciated.
Cheers,
Ed
Reference herein to any specific commercial products, process, or service by trade name, trademark, manufacturer, or otherwise, does not necessarily constitute or imply its endorsement or recommendation. Product names are for identification purposes only. All trademarks and registered trademarks are the property of their respective owners.
26th Oct 2009 17:36 UTCStephen Moreton Expert
1st Dec 2009 18:56 UTCPeter Haas
Apart from the solubility of apatite, the conversion grade of phosphate into hydrogen phosphates only depends on proton concentration (i.e. pH value) and acid strength (i.e. pK value), because the reaction is a proton transfer. The chemical nature of the anion has no effect. The risk of apatite decomposition, therefore, is lowest with phosphoric acid (pK1 around 2) and much higher with all other mineral acids (pK < 0).
The most annoying side effects of phosphoric acid are the low solubilities of many phosphates, giving rise to the formation of unwanted precipitates. A good alternative is citric acid, which has a similar strength, but superior complexing ability. Dissolution of calcite by mineral acids acts only on the anion (carbonate decomposition). In citric acid, this is assisted by complexation of the cation.
30th Jun 2011 21:49 UTCMarc Maseman
From the article:
4/19/11 - EMS Willfully Infringes Peach State Labs Patent ROME, GEORGIA (April 19) – A US District Court for Middle District of Florida jury has found that Environmental Manufacturing Solutions (EMS) willfully infringed on Peach State Labs, Inc’s. method for using urea hydrochloride (patent 5,672,279). The jury reached a verdict on Monday, April 18 in the matter which was filed in 2009 -- Environmental Manufacturing Solutions, LLC v. Peach State Labs, Inc., Case No. 6:09-CV-395.
Urea Hydrochloride is a commonly used product for removing mineral scales and for pH control as buffered HCl is safer than HCl. But, please don't confuse "safer" with "safe". Many of the companies blending Urea HCl in violation of Peach State's patent do not blend at the recommended level of at least one part urea to one part HCl to make a complete buffer. Typically, with concrete removers, a 1:1 buffer doesn't work very well, so most companies use .5 part Urea to 1 Part HCl, leaving half the acid content as free HCl. This will knock down the fuming action, but by no means makes it safe.
I have personally witnessed many chemical burns and lots of damaged equipment from the use of Urea HCl and the many products in the market that claim 0-0-0 using Urea Hydrochloride.
For a good test of your 0-0-0 "synthetic" or "safe" product, take a pop top from a soda can and drop it in to a sample. Urea HCl will completely dissolve the aluminum top within a half a day. And by completely, I mean it will be gone. One comment was correct that "synthetic" etc is a bunch of marketing hype. All the "patented" language from EMS is based on Peach State's patent in which they are in which they now have been judged to have infringed upon. To my knowledge, EMS owns no patents of its own.
No one will tell you what is in their safe product, so it is up to you to either demand empirical evidence from a third party laboratory (and that you trust the results to be valid) and that you do some homework on your own. As you may be able to tell, I am in the industry and compete against EMS. We battle with marketing half-truths and deceptions daily.
This was written to help shed a bit of light on the subject and not for the sake of mentioning my product, but since I am here, I can also say that we offer lines of products that are truly safe..
30th Jun 2011 23:07 UTCPeter Haas
1st Jul 2011 00:30 UTCTom Trebisky
The only "natural" way to get hydrochloric acid that I can think of would be to pump somebody's stomach.
The usual marketing hype I suppose, insofar as calling something a synthetic acid would add to the products
appeal. I would still be careful with it, as has been said. For that matter I would be careful with acetic acid,
which is quite "natural"
1st Jul 2011 03:10 UTCAnonymous User
Interesting this thread is running. I am about to post a new thread regarding acid etching.
Many in the Copper Country of Michigan use sulfamic acid, sold in hardware and home improvement stores as a solid that can be dissolved in water. It is faster than vinegar. That said I like vinegar. It is gentle and slow and if followed by generous and repeated soakings in water crystals of many minerals come out clean and not frosted. Sulfamic seems to clean copper and silver well but accessory minerals may not survive as well.
George
25th Jul 2011 02:05 UTCEd Godsey
-------------------------------------------------------
>
> little bit more precise: Essigessenz is pur, 25%,
> acetig acid.
>
I too used to use Essigessenz for calcite removal. But I found a much cheaper 25% acetic acid source at the local Korean market. It's in a liter size bottle and called simply 'concentrated vinegar' in English. It's less than $4.00 and and will dissolve a lot of calcite.
I first came across it searching for a safe weed killer, which it is when diluted 2:1. Blackberries are a noxious weed here and I use it so I don't incur the wrath of the park district which has the adjoining property.
31st Jul 2011 15:37 UTCBart Cannon
My haphazard experiments with acids and minerals over the years have produced many curious results which lead me to believe that a crucial factor is the composition of the solution as the reaction occurs.
For example, when dissolving calcite away from pyrrhotite, things work well for a while, and then suddenly, the acid bath starts generating hydrogen sulfide and the the pyrrhotite starts dissolving. I think that this is because the HCl solution has become a CaCl2 solution which must be corrosive toward pyrrhotite.
Here in King County, Washington we have wonderful locality for shiny dodecahedral magnetite enclosed in calcite. The darned things are always etched when I use HCl to remove the calcite. Maybe magnetite is soluble in a CaCl2 solution resulting from the interaction of calcite with HCl.
I'm going to try some other acids, including this now infamous "synthetic" acid.
Since we have all these chemists on this thread, I will impose upon them to explain why ammonium bifluoride is a more pleasant, yet effective substance to use for opaline crust removal on other silicates than even dilute HF. Doesn't it dissociate into the same thing?
I've heard some talk that I don't understand about ammonium bifluoride being "self buffering". Maybe that means that it's always just the right concentration. Magic?
10th Aug 2011 12:32 UTCRoberto Sbalchiero
Thanks.
24th Aug 2011 15:08 UTCAngryAngler17
Does your company sell urea hydrochoride? I think a lot of people on here were just looking to purchase it and try it out. In light of what you've posted some of us may be swayed away from ordering barracuda.Thanks
15th May 2012 18:57 UTCWallace Mitchell
I would like to reestablish contact with you.
Wallace
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Copyright © mindat.org and the Hudson Institute of Mineralogy 1993-2024, except where stated. Most political location boundaries are © OpenStreetMap contributors. Mindat.org relies on the contributions of thousands of members and supporters. Founded in 2000 by Jolyon Ralph.
Privacy Policy - Terms & Conditions - Contact Us / DMCA issues - Report a bug/vulnerability Current server date and time: May 2, 2024 22:07:08