Talk:Ionic strength

message: : I believe this should be split off into a seperate article, as it is not really about ionic strength. While the resulting article will refer to this page certainly, it is more of an experimental technique that deserves its own page, much in the way of Standard_addition Pckilgore (talk) 17:19, 15 December 2007 (UTC)
replies: text:  You are absolutely right. This section is irrelevant and I have deleted it. Petergans (talk) 09:47, 14 July 2008 (UTC)
thread_title:  Ionic Replacement 

message: Is there a direct way to measure ionic strength, whether with an instrument, some kind of titration, a fluorimetric probe, etc?
-- Tom Anderson 2008-01-16 2055 +0000  —Preceding unsigned comment added by 128.40.81.141 (talk) 20:55, 16 January 2008 (UTC)
thread_title:  Measuring ionic strength 

message: The above definitions involve two assumptions:
(not mentioning it)
1) water solutions
2) complete (total) dissociation.
Organic compounds might dissolve in water, and might have more carboxylic groups.
In principle the concentration should be different from the dissociated ions and more ionization steps are possible. E.g. ortho dibenzoic acid dissociates C6H4(COO-)2 + 2H+.
I have never seen ionic strength defined for organic compounds, but it would be logical:
the sum of molal concentration of ions multiplied by their Z number and multiplied by the dissociation degree.  —Preceding unsigned comment added by Karesz, Charlie (talk • contribs) 08:35, 10 September 2008 (UTC)
thread_title:  organic substances 

message: The presence of the square of the charge number in the expression of ionic strength can be equivalently expressed by considering the absolute value of the charge number or the root square from the square of the charge number.--MagnInd (talk) 08:17, 5 October 2013 (UTC)
thread_title:  Equivalent expressions 

message: There seems to be a derived concept from ionic strength, namely ionic strength fraction which describes binary mixed electrolytes. Some details are useful to be included.--5.15.59.0 (talk) 10:55, 20 January 2016 (UTC)
thread_title:  Ionic strength fraction 

message: Substituted at 19:04, 29 April 2016 (UTC)
thread_title: Assessment comment

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thread_title:  External links modified 

message: about your recent modification of Molal (mol/kg): 
https://en.wikipedia.org/w/index.php?title=Ionic_strength&type=revision&diff=960168316&oldid=933081419
15:35, 1 June 2020 Christian75 talk contribs  7,422 bytes -6  Remove "water" in molal (mol/kg water). It doesn't have to be water 
Just a request for clarification concerning your recent edit. What do you exactly mean? 
Is it water or another solvent (e.g., DMF, DMSO, liquid ammonia, (an ionic liquid or a molten salt, but then, I strongly doubt in such a case because of the very high electrolytic background ???), a mixture water/alcohol to modify the water dielectric constant and to decrease the solubility of some salts, or any organic solvent capable of dissociating an ionic substance...).
Or, is it the mass of the whole solution and not the mass of water considered here as the solvent of reference: 
:solution mass = solvent mass + solutes mass
:solution mass = water mass + solutes mass
I was also puzzled by the term water considered as the solvent. 
I am inclined to consider that it is the mass of the solution. 
Then, why not to clearly mention: mass of the solution, the aim being to get rid of volume changes due to the contraction or the expansion of the solution after mixing or dilution. 
Remember also that the concept of ionic strength was initially defined for aqueous solutions where it is used in most of the cases. Maybe does it exist some relatively exotic research fields, where it is not water but another solvent. Then, we need to take care not to give an excessive place to something relatively rare.
Indeed, we need to avoid to puzzle the reader with a non-necessary big theoretical generalization which in fact is very rarely applicable and only deals with a very narrow research field poorly known. 
I would suggest to stick to the simple case of ordinary aqueous solutions. However, if you are familiar with a rare application of the ionic strength concept to non-aqueous solvents, I propose that you create a new section dedicated to this special application with some relevant references to illustrate the ideas that you have in mind. Such as specialized section should have an appropriate size proportionate to the rest of the content of the page to avoid to cannibalize it, because the concept of ionic strength mainly deals with aqueous solutions. 
What is your opinion and thanks to adapt the main page accordingly if considered relevant. Best regards, Shinkolobwe (talk) 15:58, 1 June 2020 (UTC)
replies: text: I removed water because the lead talks about solutions (and not water). IUPACs definition (and out article) of molal i "Amount of entities of a solute divided by the mass of the solvent."(IUPAC. Compendium of Chemical Terminology, 2nd ed. (the "Gold Book")). Therefore, I added "solvent" in my last edit to clarify what molal means. The reference from "Journal of Chemical Education" talks about (a little) about solvents and polarity. Christian75 (talk) 16:50, 1 June 2020 (UTC)
replies: text:  Thank you for your quick answer and for this well sourced explanation. For more clarity, I also just added the term "L solution" to the definition of molarity: molar (mol/L solution). So, it is also clearer from this side. Shinkolobwe (talk) 17:41, 1 June 2020 (UTC)
thread_title:  Recent change in Molal (mol/kg): It doesn't have to be water ?