Resultado de búsqueda
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))
We begin by dissolving the Cobalt Chloride in water, forming the pink hydrous form. The system’s equilibrium is then stressed by adding substances that affect concentrations or other parameters. 2- 2 [CoCl 4] (aq) 6H 2O (l)[Co(H 2O) 6] (aq) 4Cl (aq) + ++! (blue) (pink)
1 de ene. de 2023 · Equilibria in the cobalt (II)–Schiff base system were evaluated. •. The speciation model was confirmed by potentiometric and spectroscopic methods. •. Kinetic analysis showed a structural change of complexes from octahedral to tetrahedral. •. Antimicrobial activity of Schiff bases and their Co (II) complexes was evaluated. •.
22 de dic. de 2017 · The first two complexes are cationic and are formed by Co 2+ cations coordinated by two TEA ligands plus nitrate or succinate anions, respectively. The equilibrium geometries of the [Co(TEA) 2] 2+ cations have been optimized at the B3LYP/cc-pVDZ level.
