Abstract
There have been attempts at the secondary and tertiary levels of education to teach chemistry and physics without the use of mathematical equations and their derivations, supposedly simplifying the subject and making it more acceptable to students. But if our concern is with the nature of chemistry, one must realize that many of its laws are mathematical in nature.
This is a preview of subscription content, log in via an institution to check access.
Access this chapter
Tax calculation will be finalised at checkout
Purchases are for personal use only
References
Frank HS, Oswalt RL (1947) The stability and light absorption of the complex ion FeSCN++. J Am Chem Soc 69:1321–1325
Lister MW, Rivington DE (1955) Some measurements on the iron(III)-thiocyanate system in aqueous solution. Can J Chem 33(10):1572–1590
Lister MW, Rivington DE (1955) Some measurements on the iron(III)-thiocyanate system in aqueous solution. Can J Chem 33(10):1579
Maeder M, Neuhold YM (2007) Practical data analysis in chemistry. Elsevier, Amsterdam
de Berg K, Maeder M, Clifford S (2016) A new approach to the equilibrium study of iron(III) thiocyanates which accounts for the kinetic instability of the complexes particularly observable under high thiocyanate concentrations. Inorg Chim Acta 445:155–159
de Berg K, Maeder M, Clifford S (2017) The thermodynamic formation constants for iron(III) thiocyanate complexes at zero ionic strength. Inorg Chim Acta 446:249–253
Blackman A, Gahan L (2014) SI chemical data, 7th edn. Wiley, Milton
Laurence GS (1956) A potentiometric study of the ferric thiocyanate complexes. Trans Faraday Soc 52:236–242
Perrin DD (1958) The ion Fe(CNS)+2. Its association constant and absorption spectrum. J Am Chem Soc 80(15):3852–3856
Ramette RW (1963) Formation of monothiocyanatoiron(III). J Chem Educ 40(2):71–72
Cobb CL, Love GA (1998) Iron(III) thiocyanate revisited. A physical chemistry equilibrium lab incorporating ionic strength effects. J Chem Educ 75(1):90–92
Betts RH, Dainton FS (1953) Electron transfer and other processes involved in the spontaneous bleaching of acidified aqueous solutions of ferric thiocyanate. J Am Chem Soc 75:5721–5727
Hoffmann R (2012) Nearly circular reasoning. In: Kovac J, Weisberg M (eds) Roald Hoffmann on the philosophy, art, and science of chemistry. Oxford University Press, New York, pp 45–52
Gladstone JH (1855) On circumstances modifying the action of chemical affinity. Phil Trans R Soc Lond 145:179–223
Bray WC, Hershey AV (1934) The hydrolysis of ferric ion. The standard potential of the ferric-ferrous electrode at 25 °C. The equilibrium Fe+++ + Cl− = FeCl++. J Am Chem Soc 56:1889–1893
Gingras Y (2001) What did mathematics do to physics? Hist Sci xxxix:383–416
Knight D (1992) Ideas in chemistry. The Athlone Press, London
Author information
Authors and Affiliations
Corresponding author
Rights and permissions
Copyright information
© 2019 The Author(s), under exclusive license to Springer Nature Switzerland AG
About this chapter
Cite this chapter
de Berg, K.C. (2019). The Reaction and Its Equilibrium Constants: The Role of Mathematics and Data Analysis. In: The Iron(III) Thiocyanate Reaction. SpringerBriefs in Molecular Science(). Springer, Cham. https://doi.org/10.1007/978-3-030-27316-3_6
Download citation
DOI: https://doi.org/10.1007/978-3-030-27316-3_6
Published:
Publisher Name: Springer, Cham
Print ISBN: 978-3-030-27315-6
Online ISBN: 978-3-030-27316-3
eBook Packages: Chemistry and Materials ScienceChemistry and Material Science (R0)