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Dec 8, 2017 at 23:16 vote accept Charly
Dec 8, 2017 at 4:12 comment added Martin - マーチン Please note that the iron(III) thiocyanate complex is better described as the following: $\ce{[Fe(SCN)_{$x$}(H2O)_{$6-x$}]^{3-x}}; x \in \{1,2,3\}$. It is also with itself in equilibrium. || Most of the time there is no need for bracketing subscripts within mhchem constructs, i.e. \ce{Fe^3+} is actually preferred over \ce{Fe^{3+}}. There is also a wide variety of arrows available, that better typeset than \to, e.g. ->, <=>, <-->, etc. Just for further reference.
Dec 7, 2017 at 22:03 history edited Gert CC BY-SA 3.0
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Dec 7, 2017 at 22:01 comment added Gert @Charly: sorry but your lab question was wrong. Wouldn't be the first time or the last.
Dec 7, 2017 at 21:57 comment added MaxW @Charly = You can clearly see that something, the precipitate, is scattering light in the "yellow" test tube. A complex would have a "clear" (not colorless) solution as the red solution does. I'll point out that the lab almost certainly had a centrifuge. Centrifuging the yellow test tube would have separated the ppt nicely from the solution.
Dec 7, 2017 at 21:53 comment added Charly Gert this might very well be the right answer (and thank you a ton for the quick reply), but quick clarification: I didn't suspect that the reaction between Na2HPO4 with Fe+3 forms a complex, my lab question informed me so "the HPO4-2 ion forms a complex with the Fe+3 ion." So maybe both reactions happened?.... (the insoluble salt you spoke of aswell as the ironIII complex the lab spoke of)
Dec 7, 2017 at 21:48 history edited Gert CC BY-SA 3.0
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Dec 7, 2017 at 21:16 history edited Gert CC BY-SA 3.0
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Dec 7, 2017 at 21:03 history edited Gert CC BY-SA 3.0
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Dec 7, 2017 at 20:56 history answered Gert CC BY-SA 3.0