Calculate the equilibrium concentration of Ni^2+ in a 1.0-M solution [Ni(NH3)6](NO3)2

Name: Problem 85, Chapter 15: Chemistry
Uploaded: 2019-10-08T08:22:31-08:00
Duration: 3 min 8 s
Channel: Rikhil Makwana
Description: Calculate the equilibrium concentration of Ni^2+ in a 1.0-M solution [Ni(NH3)6](NO3)2

step 1 Hello everyone, this is Ricky and today we're working on problem 85. We're going to be calculati

Calculate the equilibrium concentration of Ni^2+ in a 1.0-M...

Key Concepts

Formation Constant (Stability Constant)

The formation constant, also known as the stability constant, quantifies the strength of the complex ion formation, indicating the extent to which the metal ion prefers to exist in its complexed form over its free ionic form. A high formation constant means that very little free Ni²? remains in solution, which is a critical concept when calculating equilibrium concentrations.

Complex Ion Formation

Complex ion formation involves the binding of a central metal ion with one or more ligands to form a coordination complex. In the given problem, the formation of the nickel-ammonia complex [Ni(NH3)6]²? is key, and understanding the equilibrium between the free metal ion and the complex is crucial for determining the concentration of Ni²?.

Mass Action Law

The mass action law provides the framework for writing the equilibrium constant expression for a reaction, where the concentrations of the reactants and products are raised to the power of their stoichiometric coefficients. This law is essential for calculating the equilibrium concentration of Ni²? based on the reaction's established equilibrium constant.

Chemical Equilibrium

Chemical equilibrium is the state in which the rates of the forward and reverse reactions are equal, resulting in constant concentrations of reactants and products. In this context, it involves understanding how the complex ion [Ni(NH3)6]²? maintains a balance with its dissociation into Ni²? and ammonia molecules.

Transcript

Please give Ace some feedback