Talk:Lead(II) nitrate

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[edit] older entries

Let's see how this'll come up in the logs. Wim van Dorst (Talk) 19:37, 8 May 2006 (UTC).

It is too short for A-Class yet, but for such a normal compound, there's surprisingly little info. Wim van Dorst (Talk) 23:57, 11 May 2006 (UTC).

W. C. HamiltonA neutron crystallographic study of lead nitrate Acta Cryst. (1957). 10, 103-107 10.1107/S0365110X57000304

H. Nowotny and G. Heger Structure refinement of lead nitrate Acta Cryst. (1986). C42, 133-135 doi:10.1107/S0108270186097032

--134.76.234.75 07:42, 12 May 2006 (UTC)

  • thanks for the references, I agree that other than that there is not much to be found on this topic, turned the library upside down. V8rik 20:58, 9 October 2006 (UTC)

[edit] Lead Nitrate, history

Production 1st in USA 1943? My ancestors producing & selling this in Lancashire 1870's.--Bostan 13:31, 23 July 2006 (UTC)

  • Hi Bostan, it is phrased oddly, that is true. It says that the first commercial production in the USA was in 1943. It should not say that the first commercial production was in 1943 in the USA. So it needs rephrasing. More importantly, would you have information about the period before 1943 (anywhere in the world, but notably in Lancashire of course), that could contribute to the value of this article? Wim van Dorst (Talk) 14:20, 23 July 2006 (UTC).

[edit] Lead Nitrate

Wim, I have replied on your talk page, not used to this yet--Bostan 15:20, 23 July 2006 (UTC)

[edit] Peerreviewer output

The following suggestions were generated by a semi-automatic javascript program, and might not be applicable for the article in question.

You may wish to browse through User:AndyZ/Suggestions for further ideas. Thanks, Wim van Dorst (Talk) 23:16, 16 October 2006 (UTC)

[edit] Aqueous chemistry

In my opinion, most of what is said under "Aqueous chemistry" should belong to the Pb(II) cation and not to lead nitrate specifically (even though in practice you could have only lead nitrate or lead acetate in aqueous solution). The precipitation of lead iodide or lead hydroxide oxides is not a property of lead nitrate but of the divalent lead cation. What's specific for lead nitrate is then e.g. that it is used in the demonstration of precipitation reactions (where of course lead iodide also may be mentioned) but for closer description of which reactions occur between the lead cation and various anions I think a reference to an article about the cation should be more appropriate.

This is a valid issue to discuss, but at present we don't have a set of pages on cations (I even proposed this last year, but we agreed we did'nt have the resources of people to write those pages, and people dind't see it as a priority). However, the precipitation of lead hydroxide IS a property of lead nitrate, in the same way that a property of hydrochloric acid is to react with aq. NaOH to make aq. NaCl. An article on HCl that doesn't give examples of acid-base reactions would be flawed - in the same way, an article on lead nitrate needs examples of pptn reactions. This would be less valuable but for the fact that the nitrate and acetate are the only soluble lead salts commonly found. Actually the Pb(OH)2 point is an interesting one, because I added the section in the article that states in fact it usually does NOT form Pb(OH)2 but rather a basic lead(II) nitrate - in other words, the compound is NOT behaving like a simple Pb2+(aq) ion.
If you would like to write an article on the Pb(II) cation (and other cations!), I'd encourage you to do that, I think it would be a valuable addition to Wikipedia. It would provide a good place to discuss these issues in a more general context. Thanks, Walkerma 05:48, 6 November 2006 (UTC)

[edit] Plumb dulcis

Plumb dulcis (Sweet lead) is the term from the alchemist. The German word for lead acetate is Bleizucker (Lead suggar).

Some quaestions to this:

Is there a possible mix up between the words, chemicals or between the languages? Is it possible to mention that Plumb dulcis is called that way because it tastes sweet? --Stone 12:27, 10 November 2006 (UTC)

[edit] taste

The article fails to mention the taste of this compound.

It does say "dulcis" under the name, and we don't want to be giving people ideas, now do we?--Ron E 00:49, 8 March 2007 (UTC)
The sweet taste of many Beryllium salts (which are also poisonous) is mentioned in that article. Taste-based nomenclature is an interesting topic if considered from a history of chemistry perspective. --Noren 14:57, 8 March 2007 (UTC)

[edit] No space before the parentheses

It seems like there should be a space before the parentheses, no? --Liface 00:38, 8 March 2007 (UTC)

No space is standard IUPAC notation. æ² ✆ 2007‑03‑08t01:36z
That's right, there is no space in IUPAC. This is also explained here. Walkerma 02:39, 8 March 2007 (UTC)

[edit] Anon comment

The following was left on the page-rating thingie, so I'm moving it here:

I feel I must query the description of lead(II) nitrate as a "strong, stable oxidizer".

Whilst lead (II) compounds could be reduced to lead metal by strong reducing agents (thus categorizing them as weak oxidizers), they are more commonly thought of as weak reducing agents, that can be oxidized to lead (IV) by strong oxidizers. In any case no examples are brought in the article to demonstrate any oxidizing or reducing properties. (The example given where lead nitrate forms oxygen and dinitrogen tetroxide is not a demonstration of lead ion as an oxidizer, but rather a disproportionation of the nitrate ion.)

Perhaps a better description might be "a stable compound, with weak oxidation and reduction properties". 194.90.190.116 08:31, 8 March 2007 (UTC)

Its hazards are listed under NFPA 704 as an oxidizer. Under fire hazards, Aldrich's MSDS site warns it's a [strong oxidizer]. Considering the conveniently web-accessible safety information I think the existing description is correct. --Noren 15:10, 8 March 2007 (UTC)

[edit] Help!

This page got vandalized, I tried to revert it to the previous version and haven't quite managed it, can someone fix it please? Sorry. Jules 15:12, 8 March 2007 (UTC)

Why is the chemical formula reading Pd instead of Pb? It is beyond my expertise (which is not much) to correct this. Dormroomchemist 08:43, 12 March 2007 (UTC)

I think this was a type in one of the templates, where I found Pd marked down as lead (Note - these templates are really complicated!). I fixed the typo, and, Hey Presto! nothing changed. (Maybe a server cache problem?) It was also calculating the wrong molar mass. So I used the slightly lower tech version and forced the formula * molar mass in, and that has worked. I also noticed an embarrassing problem with the solubility, also fixed. Walkerma 22:40, 12 March 2007 (UTC)
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