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"It can also be prepared by electrolysis of magnesium sulfate [Epsom salts] solution at moderate voltage with a copper anode: this reaction produces hydrogen, copper sulfate solution, and copper hydroxide precipitate."
what happens to the magnesium? MgSO4(aq) + Cu(S) --dc--> h2(g) + Mg(OH)2(s) + CuSO4(aq) would make more sense.
The article states: "In an illustration of a "single metal replacement reaction," iron is submerged in a solution of copper sulfate. Upon standing, iron dissolves and copper precipitates. Fe + CuSO4 → FeSO4 + Cu"
Can anyone tell me if any similar reactions occur with stainless steel or other metals (brass, copper, chrome, etc...), pure or otherwise, in a natural state (i.e. not through electrolysis or other method)? Many thanks - Yes, it is a process called transmetalation (I think). It is essentially a battery, where initially there is no Iron salt, and no copper electrode. In a typical battery, as it looses energy, one electrode is degraded with the metal going into solution, and the other one is built up, with metal coming out of solution. This is essentially a short circuited version of that. Electrolysis would push this the other way, so you could get iron out and put copper in. With any 2 metals, one will go into the solution and precipitate the other out (assuming there is some of the metal to go into solution and some metal to precipitate out). Electrolysis will reverse this. — Preceding unsigned comment added by Black.jeff (talk • contribs) 01:08, 26 October 2011 (UTC)
does copper(II) sulphate conduct electric current?why?
How can you turn Copper(II) sulfate into copper?
Does someone have the balanced equation for that decomposition of Copper(II) sulfate into the oxides? RJFJR 00:41, Feb 12, 2005 (UTC)
Not homework. I've been out of school too long to remember some of this. First equation easy. Second I got with some work. Didn't think of the third one. The article says the the products of decomposition are CuO and Cu2O. I read that the first time thought: shouldn't that be CuO and SO2 (and O2)? Thank you for clearing that up for me. RJFJR 14:22, Feb 12, 2005 (UTC)
I checked Handbook of Physics and Chemistry 34th edition, Chemical Rubber Company, 1952 (was my dad's) RJFJR 14:38, Feb 12, 2005 (UTC)
The above description is right. You get CuSO4 -> CuO + SO3 as it decomposes. First of all, I've done this one before and can attest that you can't get copper. Second, the current equation has O2 and Cu metal as products. This is two reductions and nothing being oxidized. It violates the rules of redox chemistry and can't possibly be correct. If, for example, carbon was added to the reactants, it could feasibly steal an oxygen from the CuO and SO3 to make CO2, and the reduction of the CuO to copper metal would balance with the oxidation of carbon to CO2. I will change the equation. Dormroomchemist 05:20, 10 April 2007 (UTC)
Does anyone mind if I move this page to Copper(II) sulfate (i.e., the IUPAC name)? Currently this is a redirect. Thought I'd better ask since this has been a busy page, although all of the text in this page conforms to the IUPAC name. Walkerma 20:36, 21 Feb 2005 (UTC)
Yes I do- it may seem a minor thing, but I'm trying to get all pages standardised on the IUPAC system- nearly all of them are now (see List of inorganic compounds. That way if you type in the correct name, you find the compound. I have added a move request to the page since I was unable to do the move myself. Walkerma 23:01, 28 Mar 2005 (UTC)
Can someone please change Sulfate to Sulphate, im not being anti-american but its internationally rcognised as sulphur/sulphate/sulphate etc., my credential to prove my knowledge is that im studying chemistry to AS-Level (hopefully beyond that too) at college
I'm also studying AS Chemistry, and I know about sulfate being the IUPAC name, but am confused as to why ethanoic acid is incorrect, as it is ethane with a carboxylic acid group on the end, 'ethan' + 'oic acid', no? (I know this isn't relevant to the page, but just confused).
Also if you are really british, the title would have no z! changing.
i am currently studying chemistry at A2 level, my teacher mentioned that the name Sulphate is officially being changed to sulfate at some point soon here in britain, also Acetic acid is the 'given' name for the chemical, Ethandioic acid is the name if you break it down for naming so to speak, both can be interchangeable. —Preceding unsigned comment added by 220.127.116.11 (talk) 23:58, 9 December 2007 (UTC)
What's up with the [Copper(I) sulfate] under "Related compounds"? It's just a redirect to [Copper(II) sulfate] anyways... Jamie 09:13, 3 December 2005 (UTC)
What does the (II) stand for? I imagine it's some kind of secret chemistry handshake, but I found no explanation or link in this article. Pergelator. — Preceding unsigned comment added by 18.104.22.168 (talk) 03:53, 8 August 2013 (UTC)
My Biology teacher once told me that copper(II) sulfate displaces iron in the haemoglobin of the blood, causing anaemia. Is this true, or just a misinterpretation of what's already up on the Wiki about copper(II) sulfate being used in tests for anaemia? Is this behind its 'harmful' rating?
On a similar note, why is it harmful to the environment? What regulations are there for its disposal? Firefly99 10:27, 2 April 2006 (UTC)
What is the reason behind the change of colours when it has full water content (blue) and when it has been dehydrated, without water (white)?
This chemical is toxic, when taken internally, right? Shouldn't the article say so?
I don't know if this contradicts the supposed toxic effects of this compound, but they feed this stuff to pigs http://www.cda.org.uk/megab2/general/cuFarm/sec12.htm . I remember when i was a boy my friends dad had a pig farm, and he had a big bag of blue copper sulphate to feed the pigs with. Surely this needs to be mentioned in the article? I used to get jars of it to take home and grow crystals with.
It could be used as a supplement mixed into the food, in trace quantities to prevent copper deficiency, much like ferrous sulfate is used to prevent iron deficiency. Dormroomchemist 07:13, 25 September 2007 (UTC)
The article says that copper sulphate is poisonous. However, I am told that it is used against algues in a pond where people are supposed to swim in and where they actually do. Of course it is not completely contradictory to being poisonous, but it should be put in perspective: it seems not to be that poisonous that you cannot swim in water with copper sulphate (a hand full in 50 m3), taking into account that most people swallow quite some water during swimming.
Am I correct?
I am trying to ensure that it says that is to poisonous, but someone else keeps undoing it and I have no idea why. I am sure that there are plenty of children thinking of having a nice copper sulphate lick.
why does this substance change color from blue to green when water is added?
I read that during the 1906 earthquake in San Francisco, soldiers who guarded the Federal Mint building, tore the tar roofing off the wooden rafters and dipped the rafters with "blue vitriol". What for? Is it fire resistant? Kraxler 17:00, 9 January 2007 (UTC)
Thanks, i was trying to find it.
The article uses both frequently. Isn't one form or the other standardized by IUPAC? toll_booth 01:22, 21 February 2007 (UTC)
Sulfate is the correct IUPAC spelling.Lostandcold 01:43, 13 May 2007 (UTC)
I deleted this sentence from the paragraph on the use of CuSO4 in aquaria: "The algae cell dries out due to copper(II) sulphate being a desiccant." This must be a prank, right? --Jorge Stolfi 22.214.171.124 13:29, 1 April 2007 (UTC)
In one of my edits, I removed this image. It is left here is others think that it should be moved back. I just did not see the relevance of the image.--Smokefoot 22:45, 5 June 2007 (UTC)
Can we have a bit about Copper Sulfate in solution please, there isn't much about it on the page and i think there probably should be more, as it can be used as a micronutrient in low molarity, also my coursework is based on the effect of copper sulfate solution on the germination of mung beans, so it obviously has other applications than those listed.
Can someone provide some information on whether Copper Sulphate is a (non)competitive and (non)permanent inhibitor to Catalase. Some websites say it is comptitive, but some say otherwise. Can someone give some clarification to this, and also add it to the article? Matwilko (talk) 12:06, 14 December 2007 (UTC)
Does anybody know the structural formula of copper sulfate? I've seen:
But it doesn't seem to work: it fails in terms of fulfilling the Lewis structure
NOTE: in that diagram above, the two floating Oxygens should be beneath and above the Sulfur atom
I have another stupid question - is copper sulfate a polar molecule?
For real, or is this vandalism? It seems unlikely they'd put poisonous copper compounds in that is all. 126.96.36.199 (talk) 21:26, 2 March 2008 (UTC)
a pirahna solution of H2SO4 and H2O2 (super acid be careful) will oxidise copper into CuO and react with the H2SO4 to make CuSO4. —Preceding unsigned comment added by 188.8.131.52 (talk) 18:54, 14 May 2008 (UTC)
Why is there nothing on this page about use of CuSO4 as an antidote, considering that it is listed on the antidote template that also appears at the bottom? Mr0t1633 (talk) 16:53, 10 August 2008 (UTC)
This sentence seems a bit odd.
"Since it is available commercially, copper sulfate is usually purchased, not prepared in the laboratory."
Surely many compounds are available commercially. ??
I find that important. That something may be commercially available does not imply that the synthetic chemist will prefer to buy it. Examples include lithium diisopropylamide, tetrakis(triphenylphosphine)palladium. These compounds are either used on a small scale, are easily prepared, or do not keep well, among other things. On the other hand, some compounds are not available widely, or at all. While we use different headers, "preparation" usually refers to a semi-large scale - gram-<1 kg scale. "Synthesis" refers to small quantities, perhaps less than 1 gram. "Production" refers to industrial scale - tons, perhaps. --Rifleman 82 (talk) 18:34, 8 October 2008 (UTC)
"Archaic names for copper(II) sulfate are "blue vitriol" and "bluestone"." Except the source given only describes these other names as "Synonyms". "Bluestone" is still very much in use - Google gives 127,000 hits for bluestone copper. SmithBlue (talk) 07:43, 18 November 2008 (UTC)
In Some Properties of Copper Sulfate they say that copper sulfate is pretty soluble and if the pH is kept less than 7, the pH would have a small unpredictable effect. If a lot of sulfuric acid is used the solubility will be decreased by the addition of a common ion "(SO4)^-2" but this would require a very low pH. On the other hand if the pH is significantly greater than 7 copper hydroxide Cu(OH)2 would precipitate but under more or less neutral conditions, i.e. pH ~7, pH has little effect on the solubility of copper sulfate.
As per TOXICOLOGICAL PROFILE FOR COPPER, copper sulfate is soluble in methanol and slightly soluble in ethanol. If anyone finds this information worth for inclusion into the main article, please include it. J.D. (talk) 20:39, 4 February 2010 (UTC)
Has anyone information on the use of the compound in agriculture in the past? I found the history of the Bordeaux mixture and there is copper sulphate indicated already in use in 19th century. I think it would an interesting addition to the article.--Dia^ (talk) 12:13, 9 April 2011 (UTC)
I added a Citation Needed tag in the Chromated Copper Arsenate paragraph of the "herbicide, fungicide and pesticide" section. No citation was listed, and most MSDS that I could find for CCA treated wood list Copper Oxide as the copper source, and most Copper Quaternary and Copper Azole (used now instead of CCA as CCA is being phased out) MSDS list Copper Carbonate as the copper ingredient. All other MSDS that I could find simply listed "proprietary copper compound" or simply "copper". I couldn't find any MSDS listing Copper Sulfate Pentahydrate as an ingredient in Chromated Copper Arsenate, Copper Quaternary, or Copper Azole treated lumber. Harperska (talk) 04:50, 3 March 2013 (UTC)
in the side bar it says "< 650 °C decomp"
this should be be written with "> 650 °C decomp"
On this Wikipedia page pentahydrate solubilities in water are 316 g/L (0 °C), 2033 g/L (100 °C) and anhydrate solubilities in water are 243 g/L (0 °C), 320 g/L (20 °C), 618 g/L (60 °C) and 1140 g/L (100 °C). I think these data should be changed and the reasons are as follows. First of all, the data are expressed in g/L but we are not sure if it is the weight of solute present in a given volume of solution or solvent and we also need to know the density. Besides, volume measures depend on temperature. Secondly, at 0 °C and 100 °C copper sulfate may not exist as pentahydrate. According to Mullin’s book, the transition CuSO4•5H2O⇌ CuSO4∙3H2O occurs at 95.9 °C and above that temperature the solid phase consists of mixture of pentahydrate and trihydrate or only trihydrate.  Finally, according to the solubility data from Detherm, the anhydrate solubilities on Wikipedia page are not correct.
I downloaded all the solubility data of copper sulfate from Detherm and converted all the units to molal. To avoid confusion in the case of hydrated salts dissolved in water the solute concentration always refers to the anhydrous salt. The Figure 1 is the comparison of data from DETHERM and the data from Wikipedia and the average solubility at each temperature based on Detherm data were calculated to give the solubility curve in Figure 2. Finally the solubility data I obtained based on data from DETHERM are 1.09 molal (10°C), 1.31 molal (20°C), 1.56 molal (30°C), 1.80 molal (40°C), 2.12 molal (50 °C), 2.48 molal (60°C ), 2.95 molal (70°C ), 3.42 molal (80 °C).
--Baihuiqian (talk) 17:22, 18 February 2014 (UTC)