Nickel (II) Chloride (NiCl2) and Lithium Chloride (LiCl) under the microscope 🔬. NiCl2.6H2O is a green hydrate. Owing to its strong hydropholicity, LiCl readily abstracts this water [ Ссылка ], and we can transiently see a yellow nickel salt. This color is characteristic of the NiCl4-- complex. More generally, anhydrous NiCl2 is bright yellow. Gradually, more atmospheric moisture is incorporated. As this happens, the bright yellow color shifts to darker and greener tones, and dissolution sets in, with LiCl dissolving first, and NiCl2 dissolution starting after LiCl has disappeared.
Some solubilities, deliquescent relative humidities:
LiCl: 84.25 g/100 mL (25 °C) (DRH 10%) [ Ссылка ]
NiCl2: 67.5 g/100 mL (25 °C) (DRH 53 %) [ Ссылка ]
Salt hydrate pair equilibria:
LiCl·H2O = LiCl + H2O(g) (RH 1.3%)
NiCl2·2H2O = NiCl2 + 2H2O(g) (RH 1.3%)
NiCl2·4H2O = NiCl2·2H2O + 2H2O(g) (RH 24 +/- 1 %)
NiCl2·6H2O = NiCl2·2H2O + 2H2O(g) (RH 54 %)
What else do we see? 👀🔬
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If you want to see some of my theoretical work in chemistry, see for example:
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To attend our research seminar on autocatalysis, visit:
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