- #1
corinnab
- 9
- 1
I am totally confused with this question and have trying to figure it out for hours!
Co(H2O)62+ (aq) + 4 Cl- (aq) ----> CoCl42- (aq) + 6 H2O (l)
The equilibrium constant K = 4.82x 10-4
We begin by putting enough [Co(H2O)6]Cl2 (assume the salt dissociate completely into
ions) into 100.0 mL of water to make the formal concentration 0.182 mol/L
(a) Demonstrate that this system is not at equilibrium, initially.
(b) When the system comes to equilibrium, what are the final concentrations of each
of the species?
Co(H2O)62+ (aq) + 4 Cl- (aq) ----> CoCl42- (aq) + 6 H2O (l)
The equilibrium constant K = 4.82x 10-4
We begin by putting enough [Co(H2O)6]Cl2 (assume the salt dissociate completely into
ions) into 100.0 mL of water to make the formal concentration 0.182 mol/L
(a) Demonstrate that this system is not at equilibrium, initially.
(b) When the system comes to equilibrium, what are the final concentrations of each
of the species?