Litmus is a water-soluble mixture of different dyes extracted from lichens. It is often absorbed onto filter paper to produce one of the oldest forms of pH indicator, used to test materials for acidity.

Litmus powder
Chemical structure of 7-hydroxyphenoxazone, the chromophore of litmus components


The word "litmus" comes from an Old Norse word for "pulp".[1] About 1300 the Spanish physician Arnaldus de Villa Nova began using litmus to study acids and bases.[2][3] From the 16th century onwards, the blue dye was extracted from some lichens, especially in the Netherlands.

Natural sourcesEdit

Litmus can be found in different species of lichens. The dyes are extracted from such species as Roccella tinctoria (South American), Roccella fuciformis (Angola and Madagascar), Roccella pygmaea (Algeria), Roccella phycopsis, Lecanora tartarea (Norway, Sweden), Variolaria dealbata, Ochrolechia parella, Parmotrema tinctorum, and Parmelia. Currently, the main sources are Roccella montagnei (Mozambique) and Dendrographa leucophoea (California).[2]


Litmus paper after being used

The main use of litmus is to test whether a solution is acidic or basic, as blue litmus paper turns red under acidic conditions, and red litmus paper turns blue under basic or alkaline conditions, with the color change occurring over the pH range 4.5–8.3 at 25 °C (77 °F). Neutral litmus paper is purple.[2] Wet litmus paper can also be used to test for water-soluble gases that affect acidity or basicity; the gas dissolves in the water and the resulting solution colors the litmus paper. For instance, ammonia gas, which is alkaline, turns red litmus paper blue. While all litmus paper acts as pH paper, the opposite is not true.

Litmus can also be prepared as an aqueous solution that functions similarly. Under acidic conditions, the solution is red, and under alkaline conditions, the solution is blue.

Litmus (pH indicator)
below pH 4.5 above pH 8.3
4.5 8.3

Chemical reactions other than acid–base can also cause a color change to litmus paper. For instance, chlorine gas turns blue litmus paper white; the litmus dye is bleached[4] because hypochlorite ions are present. This reaction is irreversible, so the litmus is not acting as an indicator in this situation.


The litmus mixture has the CAS number 1393-92-6 and contains 10 to around 15 different dyes. All of the chemical components of litmus are likely to be the same as those of the related mixture known as orcein, but in different proportions. In contrast with orcein, the principal constituent of litmus has an average molecular mass of 3300.[5] Acid-base indicators on litmus owe their properties to a 7-hydroxyphenoxazone chromophore.[6] Some fractions of litmus were given specific names including erythrolitmin (or erythrolein), azolitmin, spaniolitmin, leucoorcein, and leucazolitmin. Azolitmin shows nearly the same effect as litmus.[7]

A recipe to make litmus out of the lichens, as outlined on a UC Santa Barbara website says:[8]

Details are difficult to find because the processes were kept secret. This summary of a modern manufacturing procedure is from The vanishing lichens, D H S Richardson, London, 1975. The lichens (preferably Lecanora tartarea and Roccella tinctoria) are ground in a solution of sodium carbonate and ammonia. Stir the lichens from time to time and the color changes from red to purple and finally blue after about four weeks. The lichens are then dried and powdered. At this stage the lichens contain partly litmus and partly orcein pigments. The orcein is removed by extraction with alcohol, leaving the pure blue litmus. It is marketed as blue lumps, masses, or tablets, after mixing with colorless compounds such as chalk and gypsum. Litmus paper is paper impregnated with this substance.


Red litmus contains a weak diprotic acid. When it is exposed to a basic compound, the hydrogen ions react with the added base. The conjugate base formed from the litmus acid has a blue color, so the wet red litmus paper turns blue in alkaline solution.


  1. ^ "Litmus". 7 October 2021.
  2. ^ a b c Neupert, Manfred (January 31, 2013). "Lackmus". Römpp Lexikon Chemie (in German).
  3. ^ Surber, Christian; Humbert, Philippe; Abels, Christoph; Maibach, Howard (2018). "The Acid Mantle: A Myth or an Essential Part of Skin Health?". In Surber, Christian; Abels, Christoph; Maibach, Howard (eds.). pH of the Skin: Issues and Challenges. Current Problems in Dermatology, ISSN 1421-5721, Volume 54. Basel: Karger Medical and Scientific Publishers. p. 3. ISBN 9783318063851. Retrieved 30 August 2022. In the early 14th century, the Spanish scholar, Arnaldus de Villa Nova (1235–1311), began to use litmus for studying acids and bases. This compound, extracted from a lichen, had been used as a dye since at least the time of the Vikings, but he was the first person known to use it as a test of acidity.
  4. ^ O'Leary, Donal (2000). "Chlorine". The Chemical Elements. Archived from the original on 2008-12-21.
  5. ^ Beecken, H.; E-M. Gottschalk; U. v Gizycki; H. Krämer; D. Maassen; H-G. Matthies; H. Musso; C. Rathjen; Ul. Zdhorszky (2003). "Orcein and Litmus". Biotechnic & Histochemistry. 78 (6): 289–302. doi:10.1080/10520290410001671362. PMID 15473576. S2CID 41944320.
  6. ^ H. Musso, C. Rathjen (1959). "Orcein dyes. X. Light absorption and chromophore of litmus". Chem. Ber. 92 (3): 751–3. doi:10.1002/cber.19590920331.
  7. ^ E.T. Wolf: Vollständige Übersicht der Elementar-analytischen Untersuchungen organischer Substanzen, S.450-453, veröffentlicht 1846, Verlag E. Anton (Germany)
  8. ^ "Students ask questions, UCSB scientists answer them". UCSB ScienceLine. 2002.