What is cobalt equilibrium?
An equilibrium exists between a hydrated cobalt species and anhydrous cobalt chloride, both Co ions have an oxidation state of 2+. The equilibrium equation representing the system is. [Co(H2O)6]2+(aq) + 4 Cl- <–> [CoCl4]2-(aq) + 6H2O Keq = 1.7×10-3.
How would the addition of water affect the hydrated cobalt ion equilibrium?
Thus, when reactants predominate, the solution looks pink and when products predominate, the solution looks blue. Adding water would shift equilibrium to favor the formation of the hydrous form. When most of the negative species around the cobalt ion are water molecules, the ion absorbs light so that it appears pink.
In which direction is the cobalt equilibrium shifted by increasing the temperature of this reaction?
forward direction
Increasing the temperature of an endothermic reaction shifts the equilibrium in the forward direction, to consume some of the excess energy and make more products.
Is the cobalt equilibrium exothermic or endothermic?
– heating cobalt(II) chloride hydrate The formation of is endothermic. On heating, the equilibrium shifts to the left and the solution turns blue.
What happens to cobalt chloride when heated?
Heating pink hydrated cobalt(II) chloride makes it turn blue.
Is the reaction exothermic why co h2o 6 2 +( aq )+ 4cl − AQ ⇌ cocl4 2 − aq )+ 6h2o L?
The Co(H2O)62+ complex is pink, and the CoCl42- complex is blue. This reaction is endothermic as written, so adding heat causes the equilibrium constant to shift to the right.
How will the cobalt equilibrium be affected?
Watch as the equilibrium between two different coloured cobalt species is disturbed, accompanied by a colour change predicted by Le Chatelier’s principle. This equilibrium can be disturbed by changing the chloride ion concentration or by changing the temperature.
What happens when water is added to cobalt?
If the chloride or cobalt concentrations increase, the equilibrium will also shift towards the blue anhydrous cobalt chloride. Add water, however, and the equilibrium will shift back towards the pink hydrated species.
Is the reaction exothermic why co H2O 6 2 +( aq )+ 4cl − AQ ⇌ CoCl4 2 − aq )+ 6h2o L?
What happens when AgNO3 is added to cobalt chloride?
Addition of AgNO3 to the blue solution of CoCl4 2– results in the formation of a white precipitate of AgCl, via the reaction Ag+(aq) + Cl–(aq) → AgCl(s), and a pink solution of Co(H2O)6 2+.
What happens when you add HCl to cobalt chloride?
If you add concentrated hydrochloric acid to a solution containing hexaaquacobalt(II) ions (for example, cobalt(II) chloride solution), the solution turns from its original pink colour to a dark rich blue. The six water molecules are replaced by four chloride ions. The reaction taking place is reversible.
What gas turns cobalt chloride pink?
Water vapour gas turns blue cobalt chloride paper light pink.
How are cobalt ions in equilibrium in solution?
Watch as the equilibrium between two different coloured cobalt species is disturbed, accompanied by a colour change predicted by Le Chatelier’s principle. The two different coloured Co (II) complex ions, [Co (H2O)6]2+ and [CoCl4]2-, exist together in equilibrium in solution in the presence of chloride ions:
What happens in the equilibrium between pink and blue cobalt?
The reaction [Co (H 2 O) 6] 2+ (aq) + 4Cl – (aq) → [CoCl 4] 2– (aq) + 6H 2 O (l) is endothermic. Therefore, in accordance with Le Chatelier’s principle, when the temperature is raised, the position of the equilibrium will move to the right, forming more of the blue complex ion at the expense of the pink species.
How does Le Chatelier’s principle affect cobalt equilibrium?
The colour changes accompanying the changes in equilibrium position are as predicted by Le Chatelier’s principle. 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.
What happens when cobalt chloride increases in concentration?
Initially, a beaker contains a red-pink solution of cobalt (II) chloride, present as [Co (H 2 O) 6] 2+ ions and chloride ions. If the chloride or cobalt concentrations increase, the equilibrium will also shift towards the blue anhydrous cobalt chloride.