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This is an incomplete question, here is a complete question.
A 0.130 mole quantity of NiCl₂ is added to a liter of 1.20 M NH₃ solution. What is the concentration of Ni²⁺ ions at equilibrium? Assume the formation constant of Ni(NH₃)₆²⁺ is 5.5 × 10⁸
Answer : The concentration of ions at equilibrium is,
Explanation : Given,
Moles of = 0.130 mol
Volume of solution = 1 L
Concentration of = Concentration of
= 0.130 M
Concentration of = 1.20 M
The equilibrium reaction will be:
Initial conc. 0.130 1.20 0
At eqm. x [1.20-6(0.130)] 0.130
= 0.42
The expression for equilibrium constant is:
Now put all the given values in this expression, we get:
Thus, the concentration of ions at equilibrium is,
