Phenolphthalein

Phenolphthalein is a chemical compound with the formula C20H14O4 and is often written as "HIn" or "phph" in shorthand notation. Phenolphthalein is often used as an indicator in acid–base titrations. For this application, it turns colorless in acidic solutions and pink in basic solutions. It belongs to the class of dyes known as phthalein dyes.

Phenolphthalein
Names
Preferred IUPAC name
3,3-Bis(4-hydroxyphenyl)-2-benzofuran-1(3H)-one
Other names
3,3-Bis(4-hydroxyphenyl)isobenzofuran-1(3H)-one
Identifiers
3D model (JSmol)
ChEMBL
ChemSpider
DrugBank
ECHA InfoCard 100.000.914
KEGG
UNII
Properties
C20H14O4
Molar mass 318.328 g·mol−1
Appearance White powder
Density 1.277 g/cm3 (32 °C (90 °F))
Melting point 258–263 °C (496–505 °F; 531–536 K) [1]
400 mg/L
Solubility in other solvents Insoluble in benzene and hexane; very soluble in ethanol and ether; slightly soluble in DMSO
UV-vis (λmax) 552 nm (1st)
374 nm (2nd)[1]
Pharmacology
A06AB04 (WHO)
Hazards
GHS pictograms [1]
GHS Signal word Danger
GHS hazard statements
 H341, H350, H361[1]
P201, P281, P308+313[1]
NFPA 704 (fire diamond)
Flammability code 3: Liquids and solids that can be ignited under almost all ambient temperature conditions. Flash point between 23 and 38 °C (73 and 100 °F). E.g. gasolineHealth code 2: Intense or continued but not chronic exposure could cause temporary incapacitation or possible residual injury. E.g. chloroformReactivity code 0: Normally stable, even under fire exposure conditions, and is not reactive with water. E.g. liquid nitrogenSpecial hazards (white): no code
3
2
0
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
N verify (what is YN ?)
Infobox references

Phenolphthalein is slightly soluble in water and usually is dissolved in alcohols for use in experiments. It is a weak acid, which can lose H+ ions in solution. The phenolphthalein molecule is colorless, and the phenolphthalein ion is pink. When a base is added to the phenolphthalein, the equilibrium shifts, leading to more ionization as H+ ions are removed. This is predicted by Le Chatelier's principle.

Uses

pH indicator

Phenolphthalein's common use is as an indicator in acid-base titrations. It also serves as a component of universal indicator, together with methyl red, bromothymol blue, and thymol blue.[2]

Phenolphthalein adopts at least four different states in aqueous solution as a result of pH changes.[3] Under strongly acidic conditions, it exists in protonated form (HIn+), providing an orange coloration. Between strongly acidic and slightly basic conditions, the lactone form (HIn) is colorless. The doubly deprotonated (In2-) phenolate form (the anion form of phenol) gives the familiar pink color. In strongly basic solutions, phenolphthalein is converted to its In(OH)3− form, and its pink color undergoes a rather slow fading reaction and becomes completely colorless above 13.0 pH.

Species H3In+H2InIn2−In(OH)3−
Structure
Model
pH <-1[3]0−8.28.2−10.0[4]>10.0
Conditions strongly acidicacidic or near-neutralbasicstrongly basic
Color orangecolorlesspink to fuchsiacolorless
Image
An animation of the pH dependent reaction mechanism: H3In+ → H2In → In2− → In(OH)3−

Concrete carbonation

Phenolphthalein's pH sensitivity is exploited in other applications: concrete has naturally high pH due to the calcium hydroxide formed when Portland cement reacts with water. As the concrete reacts with carbon dioxide in the atmosphere, pH decreases to 8.5-9. When a 1% phenolphthalein solution is applied to normal concrete, it turns bright pink. However, if it remains colorless, it shows that the concrete has undergone carbonation. In a similar application, some spackling used to repair holes in drywall contains phenolphthalein. When applied, the basic spackling material retains a pink color; when the spackling has cured by reaction with atmospheric carbon dioxide, the pink color fades.[5]

Education

In a highly basic solution, phenolphthalein's slow change from pink to colorless as it is converted to its In(OH)3− form is used in chemistry classes for the study of reaction kinetics.

Entertainment

Phenolphthalein is used in toys, for example as a component of disappearing inks, or disappearing dye on the Hollywood Hair Barbie hair. In the ink, it is mixed with sodium hydroxide, which reacts with carbon dioxide in the air. This reaction leads to the pH falling below the color change threshold as hydrogen ions are released by the reaction:

OH−(aq) + CO2(g) → CO2−
3(aq) + H+(aq).

To develop the hair and "magic" graphical patterns, the ink is sprayed with a solution of hydroxide, which leads to the appearance of the hidden graphics by the same mechanism described above for color change in alkaline solution. The pattern will eventually disappear again because of the reaction with carbon dioxide. Thymolphthalein is used for the same purpose and in the same way, when a blue color is desired.[6]

Medical uses
See also: Phenol red

Phenolphthalein has been used for over a century as a laxative, but is now being removed from over-the-counter laxatives[7] because of concerns over carcinogenicity.[8][9] Laxative products formerly containing phenolphalein have often been reformulated to have alternate active ingredients: Feen-a-Mint[10] switched to bisacodyl and Ex-Lax[11] was switched to a senna extract.

Thymolphthalein is a related laxative made from thymol.

Despite concerns regarding its carcinogenicity, the use of phenolphthalein as a laxative is unlikely to cause ovarian cancer.[12] Phenolphthalein has been found to inhibit human cellular calcium influx via store-operated calcium entry (SOCE, see Calcium release activated channel § Structure). This is effected by its inhibiting thrombin and thapsigargin, two activators of SOCE that increase intracellular free calcium.[13]

Phenolphthalein has been added to the European Chemicals Agency's candidate list for Substances of Very High Concern (SVHC).[14]

A reduced form of phenolphthalein, phenolphthalin, which is colorless, is used in a test to identify substances thought to contain blood, commonly known as the Kastle–Meyer test. A dry sample is collected with a swab or filter paper. A few drops of alcohol, then a few drops of phenolphthalin, and finally a few drops of hydrogen peroxide are dripped onto the sample. If the sample contains hemoglobin, it will turn pink immediately upon addition of the peroxide, because of the generation of phenolphthalein. A positive test indicates the sample contains hemoglobin and, therefore, is likely blood. A false positive can result from the presence of substances with catalytic activity similar to hemoglobin. This test is not destructive to the sample; it can be kept and used in further tests. This test has the same reaction with blood from any animal whose blood contains hemoglobin, including almost all vertebrates; further testing would be required to determine whether it originated from a human.

Synthesis

Phenolphthalein can be synthesized by condensation of phthalic anhydride with two equivalents of phenol under acidic conditions (hence the name). It was discovered in 1871 by Adolf von Baeyer.[15][16][17]

Synthesis of phenolphthalein:[18]

The reaction can also be catalyzed by a mixture of zinc chloride and thionyl chloride.[19]

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gollark: Hmm. That was my second guess.
gollark: I'm trying to figure out who you are implying are "skids".
gollark: Hmm.
gollark: Or, well, monetizing it for large-ish-scale sale.

See also

References
  1. "Phenolphthalein". Retrieved 7 October 2014.
  2. "Universal Indicator". ISCID Encyclopedia of Science and Philosophy. Archived from the original on September 25, 2006.
  3. Wittke, Georg (1 March 1983). "Reactions of phenolphthalein at various pH values". Journal of Chemical Education. 60 (3): 239. doi:10.1021/ed060p239. ISSN 0021-9584.
  4. Rathod, Balraj B.; Murthy, Sahana; Bandyopadhyay, Subhajit (20 February 2019). "Is this Solution Pink Enough? A Smartphone Tutor to Resolve the Eternal Question in Phenolphthalein-Based Titration". Journal of Chemical Education. 96 (3): 486–494. doi:10.1021/acs.jchemed.8b00708.
  5. US 6531528, Ronald D. Kurp, "Ready to use spackle/repair product containing dryness indicator", assigned to Dap Products Inc.
  6. Toystore
  7. Spiller, H. A.; Winter, M. L.; Weber, J. A.; Krenzelok, E. P.; Anderson, D. L.; Ryan, M. L. (May 2003). "Skin Breakdown and Blisters from Senna-Containing Laxatives in Young Children". The Annals of Pharmacotherapy. 37 (5): 636–639. doi:10.1345/aph.1C439. PMID 12708936.
  8. Dunnick, J. K.; Hailey, J. R. (1996). "Phenolphthalein Exposure Causes Multiple Carcinogenic Effects in Experimental Model Systems" (PDF). Cancer Research. 56 (21): 4922–4926. PMID 8895745.
  9. Tice, R. R.; Furedi-Machacek, M.; Satterfield, D.; Udumudi, A.; Vasquez, M.; Dunnick, J. K. (1998). "Measurement of Micronucleated Erythrocytes and DNA Damage during Chronic Ingestion of Phenolphthalein in Transgenic Female Mice Heterozygous for the p53 Gene". Environmental and Molecular Mutagenesis. 31 (2): 113–124. doi:10.1002/(SICI)1098-2280(1998)31:2<113::AID-EM3>3.0.CO;2-N. PMID 9544189.
  10. https://www.drugbank.ca/drugs/DB04824
  11. Stolberg, Sheryl Gay (August 30, 1997). "3 Versions of Ex-Lax Are Recalled After F.D.A. Proposes Ban on Ingredient".
  12. Cooper, G. S.; Longnecker, M. P.; Peters, R. K. (2004). "Ovarian Cancer Risk and Use of Phenolphthalein-Containing Laxatives". Pharmacoepidemiology and Drug Safety. 13 (1): 35–39. doi:10.1002/pds.824. PMID 14971121.
  13. Dobrydneva, Y.; Wilson, E.; Abelt, C. J.; Blackmore, P. F. (2009). "Phenolphthalein as a Prototype Drug for a Group of Structurally Related Calcium Channel Blockers in Human Platelets". Journal of Cardiovascular Pharmacology. 53 (3): 231–240. doi:10.1097/FJC.0b013e31819b5494. PMID 19247192.
  14. "Phenolphthalein - Substance Information - ECHA". echa.europa.eu. Retrieved 2017-11-06.
  15. Baeyer, A. (1871). "Ueber eine neue Klasse von Farbstoffen". Berichte der Deutschen Chemischen Gesellschaft. 4 (2): 555–558. doi:10.1002/cber.18710040209.
  16. Baeyer, A. (1871). "Ueber die Phenolfarbstoffe". Berichte der Deutschen Chemischen Gesellschaft. 4 (2): 658–665. doi:10.1002/cber.18710040247.
  17. Baeyer, A. (1871). "Ueber die Phenolfarbstoffe". Polytechnisches Journal. 201 (89): 358–362.
  18. Max Hubacher, U.S. Patent 2,192,485 (1940 to Ex Lax Inc)
  19. U.S. Patent 2,522,939
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