Anyone had experience of this product
|278 forum posts|
Quoting the great Edmund Blackadders' physician
"I've had time to consider the matter and I can strongly recommend a course of leeches"
I'm sure molasses has its place, but the ants in my garden would love it so it's not coming in my shop.
|Martin W||26/06/2019 11:14:42|
|789 forum posts|
Just been rummaging around on the web and found a list of sequestering/chelating agents, see below.
"The main types of commercial sequestering agents are:
The last entry might explain why molasses works as a de-rusting agent. I have looked but as yet have not located a complete list of compounds found in molasses. It could be that it does contain 'Sugar Acrylates' but there again I may be barking up the wrong tree, again .
edit. another quote from the web.
"Molasses owes its properties to cyclic hydroxamic acids which are powerful chelators of iron. More of these compounds are found if the molasses is derived from sugar beet rather than cane sugar. The plants from which molasses is made presumably use these chelating agents to help them extract minerals from the soil."
So maybe the sugar acrylates aren't the main agent. Must check the trees before barking .
Edited By Martin W on 26/06/2019 11:43:36
Edited By Martin W on 26/06/2019 11:48:10
|Kiwi Bloke||26/06/2019 12:03:17|
|187 forum posts|
Thanks Martin. Well, we're getting somewhere... But questions remain: why do chelators prefer to bind the Fe from the oxide rather than from the lump of metal? Is it because the oxide is far more soluble in the chelator solution than is the elemental iron? Will chelators attack the base metal significantly / at all? Are there more important things I should be doing at this time?
|Michael Gilligan||26/06/2019 14:32:59|
13253 forum posts
NO ... Nothing is more important than for you to give us a definitive answer
|Mark Rand||26/06/2019 22:33:24|
|711 forum posts||
Possibly because rust is a porous powder loosely mechanically bonded to the surface where as iron is a (poly)crystalline solid.
|Anthony Knights||27/06/2019 08:21:51|
|235 forum posts|
I have a tin of black treacle in my kitchen cupboard. Perhaps i should relocate it to the workshop.
|pgk pgk||28/06/2019 07:47:27|
|1360 forum posts|
My chemistry is too outdated and limited to really break down an answer but it occurred to me to dig about as to what is in molasses.
If you 'chemical composition of molasses' and view the images then there is a legion of charts some of which show a significant difference between cane and beet molasses. This link for instance shows a signiicant difference with pH with their sample of cane molasses at ph5 and signiicantly that sample also has a substantial level of reducing sugars. The old school biology test for glucose will precipitate copper salts from benedicts solution for instance.
This link which happens to be beet molassses also gives an indication of the variety of minerals within the complex (not really a suprise since we're looking at organic life).
So....(and this is a simpliied 'stretch'.. it's seems reasonable to assume that cane molasses would have enough acidity to break down some of the iron oxides into a soluble form as well as perhaps some indirect reduction. (perhaps the complex of chemical composition having an effect analagous to a catalyst?). It may/my not be that the effect is more pronounced on the oxide than crystalline iron (and anyway the reaction is slow enough that users stop when the rust has gone. A test with leavng a piece of clean iron for months?).
I other words everyone is correct (or the soup of molasses is too complex to unravel)
|Kiwi Bloke||28/06/2019 11:13:49|
|187 forum posts|
My experience is that months of immersion in molasses doesn't cause the base metal to be etched - but the rust goes.
It does rather seem that 'chelation' is a term that gets used without being strictly defined. Oxalic and citric acids get called chelators. Both remove rust. Both are acids and, as far as I know, form iron citrate and iron oxalate. Is this chelation? Are these relatively simple metal salts of organic acids chelates? I'm not getting much further in this particular quest for knowledge...
|pgk pgk||28/06/2019 13:23:56|
|1360 forum posts|
Just shows how rusty my chem is...
I still think using that term here, however technically correct, imbues the use of such de-rusters as having a magical property to the average shopper.
|Martin W||28/06/2019 14:49:08|
|789 forum posts|
A further bit of digital digging has shown that chelation is a very specific process where a large molecule will form at least two bonds to a metal ion. One definition found is :
Also an entry can be found in Wikipedia here . There are many other descriptions of chelation but they all describe the same process
Hope this helps.
|Tim Stevens||28/06/2019 15:12:51|
1040 forum posts
The term chelation is used in gardening - it is a good way of supplying chemicals (such as iron) to ericaceous plants (eg heathers and rhododendrons) when they are planted in soils which are not acid enough.
It is also the case that many organic acids serve as reducing agents (ie they reduce ferric iron Fe+++ to Ferrous iron Fe++), and this is much easier to dissolve. Thus ferric oxide (rust) becomes ferrous, and is dissolved by the acid. Ferric compounds tend to be yellow or brown, ferrous tends to be green. A plastic bottle of citric acid which has been used for rust removal will start off green-ish, and after a week or more, will become yellow and pull in the sides of the bottle. This is because the dissolved ferrous iron absorbs oxygen from the air in the bottle, producing ferric iron and lowering the air pressure (as the oxygen is no longer there).
I hope this does not add to the confusion (if any).
Edited By Tim Stevens on 28/06/2019 15:15:57
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