What is the value of K_b for the cyanide anion, CN⁻? K_a(HCN) = 6.2 × 10⁻¹⁰

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Quizplus · Accepted Answer

The value of $K_{a}$ for HCN is given as $6.2 \times 10^{-10}$. The cyanide anion, $CN^-$, is the conjugate base of HCN. The relationship between the acid dissociation constant ($K_a$) of a weak acid and the base dissociation constant ($K_b$) of its conjugate base in water is given by the equation $K_w = K_a \times K_b$, where $K_w$ is the ionization constant of water at 25°C, equal to $1.0 \times 10^{-14}$. Therefore, to find $K_b$ for $CN^-$, we rearrange the equation to $K_b = \frac{K_w}{K_a}$ and substitute the given values: $K_b = \frac{1.0 \times 10^{-14}}{6.2 \times 10^{-10}} = 1.6 \times 10^{-5}$.

What Is the Value of Kb for the Cyanide Anion

What Is the Value of K_b for the Cyanide Anion