Bromothymol blue

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Bromothymol blue
Bromothymol-blue-2D-skeletal.png
Bromothymol-blue-3D-balls.png
Names
Preferred IUPAC name
3,3-Bis[3-bromo-4-hydroxy-2-methyl-5-(propan-2-yl)phenyl]-2,1λ6-benzoxathiole-1,1(3H)-dione
Identifiers
3D model (JSmol)
ChEBI
ChEMBL
ChemSpider
ECHA InfoCard 100.000.884 Edit this at Wikidata
EC Number
  • 200-971-2
UNII
Properties
C27H28Br2O5S
Molar mass 624.38 g·mol−1
Density 1.25 g/cm3
Melting point 202 °C (396 °F; 475 K)
Sparingly soluble in water[1]
Acidity (pKa) 7.0
Hazards
Safety data sheet See: data page
http://www.sciencelab.com/msds.php?msdsId=9927468
GHS pictograms GHS07: Harmful
GHS Signal word Warning
GHS hazard statements
 H302, H315, H319
P264, P270, P280, P301+312, P302+352, P305+351+338, P321, P330, P332+313, P337+313, P362, P501
NFPA 704 (fire diamond)
2
1
0
Supplementary data page
Structure and
properties
 Refractive index (n),
Dielectric constant (εr), etc.
Thermodynamic
data
 Phase behaviour
solid–liquid–gas
Spectral data
 UV, IR, NMR, MS
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
☒N  (what is checkY☒N ?)
Infobox references

Bromothymol blue (also known as bromothymol sulfone phthalein and BTB) is a pH indicator. It is mostly used in applications that require measuring substances that would have a relatively neutral pH (near 7). A common use is for measuring the presence of carbonic acid in a liquid. It is typically sold in solid form as the sodium salt of the acid indicator.

Structure and properties[]

Bromothymol blue (pH indicator)
below pH 6.0 above pH 7.6
6.0 ⇌ 7.6

Bromothymol blue (pH indicator)
below pH <0 above pH 6.0
<0 ⇌ 6.0

[citation needed]

Bromothymol blue acts as a weak acid in a solution. It can thus be in protonated or deprotonated form, appearing yellow or blue, respectively. It is bright aquamarine by itself, and greenish-blue in a neutral solution. The deprotonation of the neutral form results in a highly conjugated structure, accounting for the difference in color. An intermediate of the deprotonation mechanism is responsible for the greenish color in neutral solution.[2]

The protonated form of bromothymol blue has its peak absorption at 427 nm thus transmitting yellow light in acidic solutions, and the deprotonated form has its peak absorption at 602 nm thus transmitting blue light in more basic solutions.[3] Highly acidic Bromothymol blue is magenta in color.

The general carbon skeleton of bromothymol blue is common to many indicators including chlorophenol red, thymol blue, and bromocresol green.[2]

The presence of one moderate electron-withdrawing group (bromine atom) and two moderate donating groups (alkyl substituents) are responsible for bromothymol blue's active indication range from a pH of 6.0 to 7.6. While the conjugation is responsible for the length and nature of the color change range, these substituent groups are ultimately responsible for the indicator's active range.[2]

Structure at different pH ranges

Bromothymol blue is sparingly soluble in oil, but soluble in water, ether, and aqueous solutions of alkalis. It is less soluble in nonpolar solvents such as benzene, toluene, and xylene, and practically insoluble in petroleum ether.[4]

Synthesis and preparation[]

Bromothymol blue is synthesized by addition of elemental bromine to thymol blue in a solution in glacial acetic acid.[5]

To prepare a solution for use as pH indicator, dissolve 0.10 g in 8.0 cm3 N/50 NaOH and dilute with water to 250 cm3. To prepare a solution for use as indicator in volumetric work, dissolve 0.1 g in 100 cm3 of 50% (v/v) ethanol.[4]

Uses[]

Different colors of bromothymol blue at marked pH conditions.
A less diverse but wider range of the different colors shown by bromothymol blue. The magenta color on the left-hand side is bromothymol blue with concentrated hydrochloric acid.

Bromothymol blue may be used for observing photosynthetic activities, or as a respiratory indicator (turns yellow as CO2 is added).[6][7] A common demonstration of BTB's pH indicator properties involves exhaling through a tube into a neutral solution of BTB. As carbon dioxide is absorbed from the breath into the solution, forming carbonic acid, the solution changes color from green to yellow. Thus, BTB is commonly used in science classes to demonstrate that the more that muscles are used, the greater the CO2 output.

Bromothymol blue has been used in conjunction with phenol red to monitor the fungal asparaginase enzyme activity with phenol red turning pink and bromothymol blue turning blue indicating an increase in pH and therefore enzyme activity.[citation needed] However, a recent study suggests that methyl red is more useful in determining activity due to the bright yellow ring form in the zone of enzyme activity.[8]

It may also be used in the laboratory as a biological slide stain. At this point, it is already blue, and a few drops are used on a water slide. The cover slip is placed on top of the water droplet and the specimen in it, with the blue coloring mixed in.[clarification needed] It is sometimes used to define cell walls or nuclei under the microscope.

Bromothymol is used in obstetrics for detecting premature rupture of membranes. Amniotic fluid typically has a pH > 7.2, bromothymol will therefore turn blue when brought in contact with fluid leaking from the amnion. As vaginal pH normally is acidic, the blue color indicates the presence of amniotic fluid. The test may be false-positive in the presence of other alkaline substances such as blood or semen, or in the presence of bacterial vaginosis.

See also[]

References[]

  1. ^ "Archived copy". Archived from the original on 2015-11-26. Retrieved 2015-12-11.CS1 maint: archived copy as title (link)
  2. ^ Jump up to: a b c De Meyer, Thierry (March 2014). "Substituent effects on absorption spectra of pH indicators: An experimental and computational study of sulfonphthaleine dyes". Dyes and Pigments. 102: 241–250. doi:10.1016/j.dyepig.2013.10.048. hdl:1854/LU-4353650. Archived from the original on 2020-07-29. Retrieved 2020-03-16.
  3. ^ Nahhal; et al. (18 July 2012). "Thin film optical BTB pH sensors using sol–gel method in presence of surfactants" (PDF). International Nano Letters. 2 (16): 3. Bibcode:2012INL.....2...16E. doi:10.1186/2228-5326-2-16. Archived (PDF) from the original on 2014-11-29. Retrieved 18 November 2014.
  4. ^ Jump up to: a b O'Neil, Maryadele J (2006). The Merck Index. Merck Research Laboratory. p. 1445. ISBN 978-0-911910-00-1.
  5. ^ "Bromothymol blue" (PDF). Archived (PDF) from the original on 27 November 2020. Retrieved 4 April 2020.
  6. ^ Sabnis R. W. (2007). Handbook of Acid-Base Indicators. CRC Press. ISBN 978-0-8493-8218-5.
  7. ^ Sabnis R. W. (2010). Handbook of Biological Dyes and Stains: Synthesis and Industrial Applications (1st ed.). Wiley. ISBN 978-0-470-40753-0.
  8. ^ Dhale, Mohan (July 2014). "A comparative rapid and sensitive method to screen l-asparaginase producing fungi". Journal of Microbiological Methods. 102: 66–68. doi:10.1016/j.mimet.2014.04.010. PMID 24794733.

External links[]

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