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#NiCl_3# is a strong electrolyte. How do you determine the concentration of each of the individual ions in a 0.400 M #NiCl_3# solution?

Answer 1

I think you mean #NiCl_2#.

In aqueous solution, nickel chloride gives a beautiful green solution, which we would represent as #[Ni(OH_2)_6]^(2+)# or simply as #Ni^(2+)(aq)#. Two (aquated) chloride counterions, #Cl^(-)(aq)#, are along for the ride.

The concentration of the hexaqua complex is (clearly) #0.400*mol*L^-1#. The concentration of the chloride counterions is #0.800*mol*L^-1#.

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Answer 2

Cooper Anderson

To determine the concentration of each individual ion in a 0.400 M NiCl₃ solution, you can use the concept of stoichiometry. Since NiCl₃ dissociates completely into Ni²⁺ and 3 Cl⁻ ions, the concentration of Ni²⁺ ions would be equal to the initial concentration of NiCl₃, which is 0.400 M. The concentration of Cl⁻ ions would be three times the concentration of NiCl₃, so it would be 3 * 0.400 M = 1.20 M.

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Answer from HIX Tutor

When evaluating a one-sided limit, you need to be careful when a quantity is approaching zero since its sign is different depending on which way it is approaching zero from. Let us look at some examples.