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Co (H 2 O) 62+aq + 4 Cl -aq (+ heat) → CoCl 42-aq + 3 H 2 O l. The blue form is anhydrous and tetrahedral coordinated, the pink form is hydrated and is octahedral coordinated. ΔH = ~42-54kJ/mol. Conc. HCl is not only a source of Cl - but also has a dehydrating effect.
- Experiment 4: Equilibrium and Temperature - Complexes of Cobalt (II)
This process relies heavily on solubility and precipitation...
- Experiment 4: Equilibrium and Temperature - Complexes of Cobalt (II)
The distinctive colours of the two cobalt(II) species in solution produce an attractive visual demonstration of a reversible reaction and the effect of concentration and temperature on the position of equilibrium.
1. The equilibrium is heat + [Co(H2O)6]2+(aq) + 4 Cl−(aq) ⇌ [CoCl4]2−(aq) + 6 H2O(l) pink blue. Equilibrium 3. 2. Temperature effects. a. Heat causes shift in equilibrium to products . b. Cooling shifts equilibrium to reactants. 3. Concentration effects. Excess Cl− causes formation of a more blue complex (tetrachlorocobalt (II))
The blue colour is the result of cobalt chloride complex ions (CoCl 42–) in less dense acetone. This classic Le Châtelier’s Principle lab explores the reversible chemical reaction: Co (H 2 O) 62+ + 4Cl – + heat --> CoCl 42– + 6H 2 O. pink blue.
Exposure to idea of equilibrium. Exposure to concept of hydrous form. Solid knowledge of factors affecting rate of reaction. Knowledge of stoichiometry and limiting reagents. (Optional) Exposure to equilibrium constants. Before the demonstration, students should be able to:
1 de ene. de 2012 · Cobalt complexes in aqueous solutions as dioxygen carriers. Maria RosariaTiné. Show more. Add to Mendeley. https://doi.org/10.1016/j.ccr.2011.10.009Get rights and content. Abstract. This article provides a short survey on the thermodynamic and kinetic behaviour of cobalt complexes, which are able to bind molecular oxygen in aqueous solutions.
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