The table below provides the acid-ionization constant, \(K_a\), and bond enthalpy for two hydrogen halides at \(298\text{ K}\). | Hydrogen Halide | \(K_a\) at \(298\text{ K}\) | \(\text{H}-\text{X}\) Bond Enthalpy (\(\text{kJ/mol}\)) | | :--- | :--- | :--- | | \(\text{HF}\) | \(6.3 \times 10^{-4}\) | \(567\) | | \(\text{HCl}\) | \(\gg 1\) | \(431\) | Which of the following statements best compares the acid strength of \(\text{HF}\) to that of \(\text{HCl}\) and provides the correct justification? • Nerd Notes

AP Chemistry

8.6 Molecular Structure of Acids and Bases

IntermediateMCQConceptual21.3k

The table below provides the acid-ionization constant, \(K_a\), and bond enthalpy for two hydrogen halides at \(298\text{ K}\).

Hydrogen Halide	\(K_a\) at \(298\text{ K}\)	\(\text{H}-\text{X}\) Bond Enthalpy (\(\text{kJ/mol}\))
\(\text{HF}\)	\(6.3 \times 10^{-4}\)	\(567\)
\(\text{HCl}\)	\(\gg 1\)	\(431\)

Which of the following statements best compares the acid strength of \(\text{HF}\) to that of \(\text{HCl}\) and provides the correct justification?

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