Whenever you write "H + (aq)" what you really mean is a hydroxonium ion, H 3O +.
It is being pulled off by a water molecule in the solution.
However, if you write it like this, remember that the hydrogen ion isn't just falling off the complex ion. The water is, of course, acting as a base by accepting the hydrogen ion.īecause of the confusing presence of water from two different sources (the ligands and the solution), it is easier to simplify this: The complex ion is acting as an acid by donating a hydrogen ion to water molecules in the solution. A hydrogen ion is lost from one of the ligand water molecules: The ion reacts with water molecules in the solution. In common with the other 3+ ions, the hexaaquachromium(III) ion is fairly acidic - with a pH for typical solutions in the 2 - 3 range. Use the BACK button on your browser to return to this page. Note: If you aren't happy about complex ions (including the way they are bonded and named), it would pay you to follow this link and explore the first couple of pages in the complex ions menu before you go on. The simplest ion that chromium forms in solution is the hexaaquachromium(III) ion - 3+. Reactions of chromium(III) ions in solution Check your syllabus and past papers to find out exactly what you need to know. You are very unlikely to need everything on this page.
You will find links to other pages where these reactions are discussed in more detail. The first part of this page is a summary of the reactions of chromium(III) ions in solution. It includes: reactions of chromium(III) ions in solution (summarised from elsewhere on the site) the interconversion of the various oxidation states of chromium the chromate(VI)-dichromate(VI) equilibrium and the use of dichromate(VI) ions as an oxidising agent (including titrations). This page looks at some aspects of chromium chemistry required for UK A level (and its equivalents).
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