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Which of the following compounds or ions has the strongest conjugate acid? K.(HCN) = 4.0 × 10-10 , K. (NH,+) = 5.6 × 10-10, K.(HSO,¯) = 1.2 x 10-2 O CN Ο ΝΗ, O so,

Which of the following compounds or ions has the strongest conjugate acid? K.(HCN) = 4.0 × 10-10 , K. (NH,+) = 5.6 × 10-10, K.(HSO,¯) = 1.2 x 10-2 O CN Ο ΝΗ, O so,

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ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Chapter1: Chemical Foundations
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**Question:** Which of the following compounds or ions has the strongest conjugate acid? \( K_a(\text{HCN}) = 4.0 \times 10^{-10} \), \( K_a(\text{NH}_4^+) = 5.6 \times 10^{-10} \), \( K_a(\text{HSO}_4^-) = 1.2 \times 10^{-2} \). - ○ \(\text{CN}^-\) - ○ \(\text{NH}_3\) - ○ \(\text{SO}_4^{2-}\) **Explanation:** The dissociation constant \( K_a \) indicates the strength of an acid. The higher the \( K_a \) value, the stronger the acid. In this case, we compare the conjugate acids: HCN, NH4+, and HSO4-. - \( K_a(\text{HCN}) = 4.0 \times 10^{-10} \) - \( K_a(\text{NH}_4^+) = 5.6 \times 10^{-10} \) - \( K_a(\text{HSO}_4^-) = 1.2 \times 10^{-2} \) Therefore, HSO4- has the strongest conjugate acid because its \( K_a \) value is the highest.
Transcribed Image Text:**Question:** Which of the following compounds or ions has the strongest conjugate acid? \( K_a(\text{HCN}) = 4.0 \times 10^{-10} \), \( K_a(\text{NH}_4^+) = 5.6 \times 10^{-10} \), \( K_a(\text{HSO}_4^-) = 1.2 \times 10^{-2} \). - ○ \(\text{CN}^-\) - ○ \(\text{NH}_3\) - ○ \(\text{SO}_4^{2-}\) **Explanation:** The dissociation constant \( K_a \) indicates the strength of an acid. The higher the \( K_a \) value, the stronger the acid. In this case, we compare the conjugate acids: HCN, NH4+, and HSO4-. - \( K_a(\text{HCN}) = 4.0 \times 10^{-10} \) - \( K_a(\text{NH}_4^+) = 5.6 \times 10^{-10} \) - \( K_a(\text{HSO}_4^-) = 1.2 \times 10^{-2} \) Therefore, HSO4- has the strongest conjugate acid because its \( K_a \) value is the highest.
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