The silver ion concentration in a 0.2 M solution of Ag(NH3)2 NO3 is (Kdiss=6.8. .×10^-8, 1.5^3=3

step 1 Hello students, for this question, we know that 0 .03 moles of AGN -03 will react with 0 .06 mol

The silver ion concentration in a 0.2 M solution of Ag(NH3)2...

The silver ion concentration in a $0.2 \mathrm{M}$ solution of $\mathrm{Ag}\left(\mathrm{NH}_{3}\right)_{2} \mathrm{NO}_{3}$ is $\left(K_{\mathrm{diss}}=6.8\right.$ $\left.\times 10^{-8}, 1.5^{3}=3.4\right)$ (a) $0.2 \mathrm{M}$ (b) $1.5 \times 10^{-3} \mathrm{M}$ (c) $1.16 \times 10^{-4} \mathrm{M}$ (d) $6.8 \times 10^{-8} \mathrm{M}$

The silver ion concentration in a $0.2 \mathrm{M}$ solution of $\mathrm{Ag}\left(\mathrm{NH}_{3}\right)_{2} \mathrm{NO}_{3}$ is $\left(K_{\mathrm{diss}}=6.8\right.$
$\left.\times 10^{-8}, 1.5^{3}=3.4\right)$
(a) $0.2 \mathrm{M}$
(b) $1.5 \times 10^{-3} \mathrm{M}$
(c) $1.16 \times 10^{-4} \mathrm{M}$
(d) $6.8 \times 10^{-8} \mathrm{M}$

Key Concepts

Complex Ion Equilibrium

This concept involves the formation and dissociation of complex ions when a metal ion binds with ligands. In solution, the distribution of a metal between its free ionic form and its complexed form is governed by an equilibrium process, which is influenced by the concentrations of the metal, the ligands, and the stability of the complex.

Equilibrium Constant Expression

The equilibrium constant (whether it be a formation constant or dissociation constant) is a quantitative measure of the position of an equilibrium. It is expressed as the ratio of the concentrations of the products to those of the reactants at equilibrium, each raised to the power of their coefficients, and it allows for the calculation of unknown concentrations in a chemical system.

Dissociation Constant

For complex ions, the dissociation constant specifically quantifies the extent to which a complex ion dissociates back into the metal ion and its ligands. A small dissociation constant indicates that the complex is very stable, meaning that very little free metal ion is present in the solution.

Approximation Methods in Equilibrium Calculations

When equilibria are strongly shifted toward the formation of one species, approximation techniques can be used to simplify calculations. These methods involve assuming that changes in concentration are negligible relative to the initial concentrations, allowing for an easier determination of species present in very low concentrations.

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