The solubility of AgCN in a buffer solution of pH=3.0 is (Ksp. of AgCN =1.2 ×10^-16 ; Ka of .HCN

step 1 The solubility product constant, KSP is the product of molar concentration of individual ion of

The solubility of AgCN in a buffer solution of pH=3.0 is...

The solubility of $\mathrm{AgCN}$ in a buffer solution of $\mathrm{pH}=3.0$ is $\left(K_{\mathrm{sp}}\right.$ of $\mathrm{AgCN}$ $=1.2 \times 10^{-16} ; K_{\mathrm{a}}$ of $\left.\mathrm{HCN}=4.8 \times 10^{-10}\right)$ (a) $1.58 \times 10^{-5} \mathrm{M}$ (b) $2.0 \times 10^{-5} \mathrm{M}$ (c) $1.58 \times 10^{-4} \mathrm{M}$ (d) $2.5 \times 10^{-9} \mathrm{M}$

The solubility of $\mathrm{AgCN}$ in a buffer solution of $\mathrm{pH}=3.0$ is $\left(K_{\mathrm{sp}}\right.$ of $\mathrm{AgCN}$ $=1.2 \times 10^{-16} ; K_{\mathrm{a}}$ of $\left.\mathrm{HCN}=4.8 \times 10^{-10}\right)$
(a) $1.58 \times 10^{-5} \mathrm{M}$
(b) $2.0 \times 10^{-5} \mathrm{M}$
(c) $1.58 \times 10^{-4} \mathrm{M}$
(d) $2.5 \times 10^{-9} \mathrm{M}$

Key Concepts

Equilibrium Shifts (Le Chatelier's Principle)

Le Chatelier's Principle explains how an equilibrium system responds to changes in concentration, pressure, or temperature by shifting to counteract the change. In the context of solubility and acid-base reactions, this principle helps predict the direction in which an equilibrium will shift when conditions such as pH are altered.

Buffer Solution Concepts

Buffer solutions maintain a nearly constant pH when small amounts of acid or base are added to the system. They are essential in chemical equilibria, as they stabilize the pH, which can significantly influence solubility equilibria, especially when the solubility is dependent on pH-sensitive species.

Solubility Product (Ksp)

The solubility product is an equilibrium constant that represents the product of the molar concentrations of the ions produced when a sparingly soluble salt dissolves. It quantifies how much of the salt can dissolve in solution at equilibrium and is crucial for predicting precipitation and dissolution behavior in chemical systems.

Acid Dissociation Constant (Ka)

The acid dissociation constant measures the extent to which a weak acid donates protons in an aqueous solution. This constant helps in understanding the equilibrium between the acid and its conjugate base, which is important for predicting how pH changes can affect the solubility and speciation of compounds in solution.

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