Calconcarboxlic acid is soluble in water and a variety of other solvents, including sodium hydroxide, ethanol and methanol.[3] It has a violet colour in dissolved form in ethanol. The melting point of calconcarboxylic acid is at approximately 300 °C, where it undergoes thermal decomposition.
Background
Though the determination of calcium and magnesium by complexometric titration with standard solutions of disodium dihydrogen tetraacetate, utilising Eriochrome Black T as indicator is widely accepted and quite adequately understood, it, like other complexometric titration methods, suffers from the limitations of having an indistinct endpoint (where a photometric titrator is needed to provide acceptable accuracy) and/or having to separate the metals before titration can occur.[2] Calconcarboxylic acid was thus adopted as a superior alternative due to its ability to give a good and visual endpoint and its rapid performance even with the presence of magnesium.
Synthesis
As described by James Patton and Wendell Reeder in 1956, calconcarboxylic acid can be synthesised by coupling diazotized 1-amino-2-naphthol-4-sulfonic acid with 2-hydroxy-3-napthoic acid.[2]
Applications
Calconcarboxylic acid is used for the determination of calcium ion concentration by complexometric titration. Free calconcarboxylic acid is blue colour, but changes to pink/red when it forms a complex with calcium ions. EDTA forms a more stable complex with calcium than calconcarboxylic acid does, so addition of EDTA to the Ca–calconcarboxylic acid complex causes formation of Ca-EDTA instead, leading to reversion to the blue colour of free calconcarboxylic acid.[4]
For the complexometric titration, the indicator is first added to the titrant containing the calcium ions to form the calcium ion-indicator complex (Ca-PR) with a pink/red colour. This is then titrated against a standard solution of EDTA. The endpoint can be observed when the indicator produces a sharp, stable colour change from wine red to pure blue, which occurs at pH values between 12 and 14,[2] this indicates the endpoint of the titration, as the Ca-PR complexes have been completely replaced by the Ca-EDTA complexes and hence the PR indicator reverts to its blue colour.[4]
The reaction can be given by:
Ca-PR + EDTA4- → PR + [Ca-EDTA]2-
The Patton-Reeder Indicator is often used here in the form of a triturate.
This method of complexometric titration is dependent on the pH of the solution being sufficiently high to ensure that magnesium ions precipitate as magnesium hydroxide before the PR indicator is added to prevent interference with the results, as if magnesium were present, the EDTA would also form complexes with it. Concentrated sodium hydroxide or potassium hydroxide is usually added to the solution to this end.
The accuracy of this method may also be affected by the presence of metal ions such as copper, iron, cobalt, zinc or manganese in sufficiently high concentrations.[4]
