The formation of a complex ion can be represented by the following general equation:M^n+ + xL MLx^n-x +where M^n+ is the metal ion, L is the ligand, and MLx^n-x + is the complex ion formed. The equilibrium constant for this reaction is given by:Kf = [MLx^n-x +] / [M^n+] * [L]^x where Kf is the formation constant, and the concentrations are represented in square brackets.Now, let's consider the three scenarios:1. Increasing the concentration of the ligand L :When the concentration of L is increased, according to Le Chatelier's principle, the equilibrium will shift to the right to counteract the change. This means that more complex ion MLx^n-x + will be formed, and the equilibrium position will shift to the right.Mathematically, as [L] increases, the denominator in the Kf expression becomes larger, and to maintain the constant value of Kf, the concentration of the complex ion [MLx^n-x +] must also increase.2. Decreasing the concentration of the ligand L :When the concentration of L is decreased, the equilibrium will shift to the left to counteract the change, according to Le Chatelier's principle. This means that less complex ion MLx^n-x + will be formed, and the equilibrium position will shift to the left.Mathematically, as [L] decreases, the denominator in the Kf expression becomes smaller, and to maintain the constant value of Kf, the concentration of the complex ion [MLx^n-x +] must also decrease.3. Keeping the concentration of the ligand L constant:If the concentration of L is kept constant, there will be no change in the equilibrium position. The concentrations of the metal ion, ligand, and complex ion will remain the same, and the equilibrium will not shift.Mathematically, since [L] remains constant, the Kf expression will not change, and the concentrations of the complex ion [MLx^n-x +] and the metal ion [M^n+] will also remain constant.In summary, increasing the concentration of the ligand will shift the equilibrium position to the right, forming more complex ion, while decreasing the concentration of the ligand will shift the equilibrium position to the left, forming less complex ion. Keeping the concentration of the ligand constant will not affect the equilibrium position.