Talk:PH indicator/Archive 1

Archive 1

pH indicators graphic view

I have created a graphic view of the pH indicators giving their operation range and the associated colour change. The image can be found here: https://commons.wikimedia.org/wiki/File:A_graphic_view_of_Acid-Base_Indicators.svg I would like to know where the image can be placed, for a good view. (Damitr (talk) 11:56, 2 September 2014 (UTC))

Methyl violet

Could someone please clarify the behaviour of this pH indicator? According to methyl violet it is the opposite to what is shown in the table. Either pH Indicator or methyl violet needs to be corrected.--Paiconos 22:14, 29 Apr 2005 (UTC)

Fixed. Good catch. --TenOfAllTrades (talk/contrib) 15:22, 30 Apr 2005 (UTC)

is there a reson the listed indicators arent linked? --Herzog 04:11, 6 October 2005 (UTC)

20100730: Gentian violet (aka methyl violet 10B) has 2 extra Me groups compared to methyl violet. CAS numbers are different as well. I wonder, if it is time for Wikipedia t osplit into chempedia or Wikichempedia and everyday stuff. —Preceding unsigned comment added by 74.247.199.50 (talk) 15:57, 30 July 2010 (UTC)

3',3,5',5,-tetrachloro-3,4,5,6-tetrabromosulfonphthalein

Can someone elucidate on this (obsolete?) indicator? Alternative spellings: 3',3,5',5,-tetrachloro-3,4,5,6-tetrabromosulphonephthalein. Was produced some time ago by Boehringer Mannheim. It is good to have all the information collected, because some older publications use them. I could not find it from manufacturers. It is amaizing, it was wide used and popular, and today you can not find anything available. Thanks —Preceding unsigned comment added by 74.247.199.50 (talk) 15:48, 30 July 2010 (UTC)

H+ is incorrect

There are no such species in solution as H+, the correct species representing an acidic proton in the hydronium ion (H3O+).

-H+ is shorthand for the hydronium ion, showing theres one proton available. It is correct either way. 199.111.85.50 01:20, 22 March 2007 (UTC)

Anthocyanin pH indicators

why in any of the articles has no-one metioned garlic? this turns green/blue when exposed to warm acid, eg; vinegar at approx 40 degrees celcius.

Range of an indicator

Can someone please explain to me how one might determine the pH at which an indicator changes color?

That is simple. You simply have to find the pKa (that is, the -log(Ka)) of the indicator. The pKa is when the two colours are at equal concentration, concentrations over that shift the indicator to the colour listed in the table. This can be proven using the equilibrium formula and allowing [HIn]=[In-]*, meaning that the two forms are in equal amounts. The two should then cancel leaving you with Ka=[H3O+], meaning that two forms are equal when the pH is equal to the pKa(definition stated above).However, usually when one colour is within 10X in concentration to the other, both forms of the colour will exist. Over that, one colour is definitely more visible than the other. Therefore, a transition pH (usually between +/-1, -- 10X or 1/10th concentration --, of the pKa) is given in tables.

That said, we should add a table of pKa values to this article.

• HIn stands for H+ ions binded to the indicator, where In = indicator. In- stands for the form missing the hydrogen ion. Therefore, the equilbrium of the two forms, the same as an acid/base equilbrium is: HIn<--->In- + H30+. The equilibrium formula can be used to find the pH at which the indicator changes colour, as seen above.

Value not matching

The pH range given in this article (4.4-6.3) does not match with the value given in Methyl red (4.4-6.2). Could somebody check the real figure and make the corresponding correction? Thanks. - LR4087 13:37, 24 October 2006 (UTC)

Specified pH ranges are usually approximate; they rely on the appearance of a colour change, and there's definitely some uncertaintly at the edges of the range. A discrepancy of a tenth of a pH unit in these values probably means that the numbers were drawn from different reference texts; it's most likely that neither figure is more 'real' than the other. TenOfAllTrades(talk) 15:19, 24 October 2006 (UTC)

I agree with TenOfAllTrades, but think that (if not already done so), a standard unit for use on the site should be agreed between proper chemists (ie, not me :-))

82.40.75.55 22:57, 27 November 2006 (UTC)

Box about pH

ie. {{pH_indicator_template}}

I have updated/added these to the relevant pages based on the information give on this main page. Any discrepancies are mere typing/ommison errors. I do not know much about any of these solutions, so please don't rant at me if any data is wrong - as I have said i was copied from the main page here.

82.40.75.55 22:55, 27 November 2006 (UTC)

Natural pH indicators?

I just feel like these could be elaborated on since some are not immediately clear with their corresponding pages. 199.111.85.50 01:20, 22 March 2007 (UTC)

Indicator Table

The way the table is arranged now, it doesn't have any logical arrangement. It should either be alphabetical, or by pH transition. If the latter, the second transition of the 2 indicators needs to be separated. LDCorey (talk) 19:50, 6 March 2008 (UTC)

Litmus

Is there any reason that litmus is omitted from the table of indicators? Andrewa (talk) 04:59, 23 March 2008 (UTC)

pH indicators are frequently weak acids or bases

Frequently? If they cannot gain or lose protons how can they respond to pH changes? I believe this should read

pH indicators are themselves weak acids or bases

but I am not a chemist. Can a chemist comment? Moletrouser (talk) 07:28, 13 October 2010 (UTC)