Talk:Hydrogen iodide

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The sentance "Once again, although chemically related, hydriodic acid is not pure HI but a mixture containing it." is not really necessary. all acids are of this nature, the very definition of acid is 'a substance in an aqeous solution'. Now, i can see the point of listing that HI is normally 98-99% or whatever was listed, but i think the sentance above should be removed and just say, "according to the definition of acid(and then we will put a link there), HI contains little water in solution." —Preceding unsigned comment added by (talk) 21:01, 2 May 2009 (UTC)

HI solubility in water[edit]

Under 'Properties of hydrogen iodide' it says: "One liter of water will dissolve 425 liters of HI [...]" Isn't it a bit unclear what is meant here (bear in mind I'm no chemist)? Is it 425 liters of (gaseous) HI at 20 degrees celsius? Gaseous HI has, I presume, a fairly low density which would mean 425 liters of HI isn't very much.

425 is quite a lot, assuming normal pressure and temperature. It is almost 20 moles, or more than 2 kilograms. --Itub (talk) 14:07, 9 July 2008 (UTC)

It's HI gas - I've checked the source, and it makes sense to me as a BS.c. in chemistry. I added "gas" after "... 425 liters of HI ..." (talk) 10:27, 23 August 2010 (UTC)

425 litres of any gas is not meaningful without further qualification. You should include ideally density (e.g. molar density per litre) or temperature and pressure (e.g. SLC: 25deg C @ 1 atm). — Preceding unsigned comment added by (talk) 09:30, 13 August 2011 (UTC)

Comment from article[edit]

I leave it to others to outline the chemical formula for this reaction.

Unsigned comment left in the article, moved here by Ziggurat 01:29, 13 February 2006 (UTC)
It seems to me this article falls into a 1st year chemistry trap: at one point it seems to overlook the fact that when an acid is dissolved into ions, it does not protonate. The proton simply does not exist freely in solution. Instead, we observe the hydronium ion (H3O+) and the equation must include water for it to be a balanced equation as a result. I'll alter it and leave you all to pick at it :) Mattabat 22:06, 3 February 2007 (UTC)
Those equations, as fixed up, look a little mangled in Internet Explorer! - I'm going to leave them however as they are correct (and look good in Firefox). Guess Internet Explorer needs work.. Mattabat

Dissociation energy of HI[edit]

Silberberg's Chemistry, 4th edition, lists the bond energy of HI as 295 kJ/mol, which means a photon of wavelength ~406nm will cause a molecule to break. Where was 578nm obtained from in this article? Also - why does wikipedia distinguish betwen dissociation energy and bond energy? No text I can find distinguishes them, and several specifically state they are the same. 18:55, 14 July 2006 (UTC)

Article status[edit]

I have made a few additions to the article, mainly adding a few organic reactions of HI with ethers and alcohols, and also a section on use of HI in making methamphetamine. I am wondering what parts of the page you guys think still need much work, I would like to see this in the B class sometime. Dffasd (talk) 02:33, 7 July 2008 (UTC)

This is way beyond "start" in my opinion, so I've rated it B. --Itub (talk) 14:04, 9 July 2008 (UTC)


The density given in the infobox (2.85g/ml at -47 degrees(why this temperature??)) seems to be much too high for a gas; the German article has 5.8g/l at 0 degrees Celsius, which seems much more reasonable. --Roentgenium111 (talk) 19:44, 3 November 2009 (UTC)

I just noticed that HI is a liquid at -47 degrees, so the value given might be right. Still, the density at 0°C (or maybe 20°C) would be more valuable for the infobox, IMO.--Roentgenium111 (talk) 19:47, 3 November 2009 (UTC)

Formation via phosphorus[edit]

Why does the equation have water on the reactants side and water in the same form on the reactants side? --Cheminterest (talk) 20:36, 24 March 2010 (UTC)

HX (g) vs HX (aq)[edit]

Why are our articles on HF, HCl, and HBr split along these lines, but not that on HI? Double sharp (talk) 01:47, 26 August 2016 (UTC)

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