For the reaction [Ag(CN)2] ⇌Ag^+ +2 CN^-, the equilibrium constant, at 25^∘ C, is 4.0 ×10^-19. C

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

For the reaction [Ag(CN)2] ⇌Ag^+ +2 CN^-, the equilibrium...

For the reaction $\left[\mathrm{Ag}(\mathrm{CN})_{2}\right] \rightleftharpoons \mathrm{Ag}^{+}$ $+2 \mathrm{CN}^{-}$, the equilibrium constant, at $25^{\circ} \mathrm{C}$, is $4.0 \times 10^{-19}$. Calculate the silver ion concentration in a solution which was originally $0.10$ molar in $\mathrm{KCN}$ and $0.03$ molar in $\mathrm{AgNO}_{3}$. (a) 0 (b) $0.03 \mathrm{M}$ (c) $3 \times 10^{-19} \mathrm{M}$ (d) $1.71 \times 10^{-19} \mathrm{M}$

For the reaction $\left[\mathrm{Ag}(\mathrm{CN})_{2}\right] \rightleftharpoons \mathrm{Ag}^{+}$
$+2 \mathrm{CN}^{-}$, the equilibrium constant, at $25^{\circ} \mathrm{C}$, is $4.0 \times 10^{-19}$. Calculate the silver ion concentration in a solution which was originally $0.10$ molar in $\mathrm{KCN}$ and $0.03$ molar in $\mathrm{AgNO}_{3}$.
(a) 0
(b) $0.03 \mathrm{M}$
(c) $3 \times 10^{-19} \mathrm{M}$
(d) $1.71 \times 10^{-19} \mathrm{M}$

Key Concepts

Chemical Equilibrium

This concept refers to the state in a reversible reaction where the rate of the forward reaction equals the rate of the reverse reaction. At this point, the concentrations of reactants and products become constant over time. Evaluating chemical equilibria is crucial for determining how a system responds to changes in conditions and allows for quantitative predictions using the equilibrium constant.

Equilibrium Constant (K)

The equilibrium constant is a numerical value that characterizes the ratio of the concentrations of products to reactants at equilibrium, raised to the power corresponding to their stoichiometric coefficients. For reactions with very small or very large equilibrium constants, it indicates that the equilibrium lies far to one side, meaning one set of species is present in minute concentration compared to the other.

Complex Ion Formation

Complex ion formation involves a metal ion binding to one or more ligands to form a complex species. This process can significantly alter the effective concentration of the free metal ion in solution, and is central to understanding how metal ions behave in the presence of ligands such as cyanide. The formation constant for a complex ion quantifies the stability of the complex in solution.

Stoichiometry of Reactions

Stoichiometry in chemical reactions focuses on the quantitative relationships between reactants and products. It is essential for determining the limits and ratios in which substances react. When applied to equilibrium problems, stoichiometry helps in setting up relationships between changes in concentration of different species as the system reaches equilibrium.

Approximation Methods in Equilibrium Calculations

Approximation methods are useful in simplifying the mathematical treatment of equilibrium systems, especially when there are extremely small or large equilibrium constants. By recognizing that some concentrations can be negligibly small, one can make reasonable assumptions to simplify the algebra and obtain approximate solutions that are accurate enough for practical purposes.

Transcript

Please give Ace some feedback