Question

Calculate the equilibrium concentration of Ni²+ in a 1.0-M solution Ni(NH₃)₆₂.

a) 0.5 M
b) 0.8 M
c) 1.0 M
d) 1.2 M

Answer 1

Without the dissociation constant or additional data it's impossible to accurately determine the equilibrium concentration of Ni2+ from a c. 1.0-M solution of [Ni(NH3)6](NO3)2. A full dissociation would imply a 1.0 M concentration of Ni2+, but partial dissociation would result in a lower concentration.

Step-by-step explanation:

To calculate the equilibrium concentration of Ni2+ in a c. 1.0-M solution of [Ni(NH3)6](NO3)2, we must consider the dissociation of [Ni(NH3)6]2+ in solution. To do this, we would need to know the dissociation constant (Ka or Ksp) for the complex ion in the solution. Without this information or any additional data on the equilibrium state or degree of dissociation, it is not possible to calculate the precise concentration of Ni2+.

Generally, if the complex ion [Ni(NH3)6]2+ is fully dissociative, the Ni2+ concentration would remain the same as the initial concentration of the complex ion, which is 1.0 M. However, if the complex ion partially dissociates, the concentration of Ni2+ will be less than the initial concentration, but without the specific Ka, we cannot determine the extent of this change.