Determine the percent ionization of a 0.125 M HCN solution.

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Identify the relevant chemical equation for the ionization of HCN: \( \text{HCN} \rightleftharpoons \text{H}^+ + \text{CN}^- \).

Write the expression for the acid dissociation constant \( K_a \) for HCN: \( K_a = \frac{[\text{H}^+][\text{CN}^-]}{[\text{HCN}]} \).

Look up the \( K_a \) value for HCN, which is typically around \( 6.2 \times 10^{-10} \).

Set up an ICE (Initial, Change, Equilibrium) table to determine the concentrations of \( \text{H}^+ \), \( \text{CN}^- \), and \( \text{HCN} \) at equilibrium.

Calculate the percent ionization using the formula: \( \text{Percent Ionization} = \left( \frac{[\text{H}^+]}{[\text{HCN}]_0} \right) \times 100\% \), where \([\text{HCN}]_0\) is the initial concentration of HCN.

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주요 개념

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Ionization of Weak Acids

Weak acids, like hydrocyanic acid (HCN), do not completely dissociate in solution. Instead, they establish an equilibrium between the undissociated acid and its ions. The degree to which a weak acid ionizes is crucial for calculating properties such as pH and percent ionization.

Equilibrium Constant (Ka)

The acid dissociation constant (Ka) quantifies the strength of a weak acid by measuring the extent of ionization at equilibrium. For HCN, the expression for Ka is derived from the concentrations of the products (H+ and CN-) and the reactant (HCN) at equilibrium, which is essential for calculating percent ionization.

Percent Ionization Calculation

Percent ionization is calculated by taking the concentration of ionized acid at equilibrium, dividing it by the initial concentration of the acid, and multiplying by 100. This metric provides insight into the strength of the acid and its behavior in solution, which is vital for understanding the properties of HCN in this context.