Of the conjugate acid-base pairs HF / F^-, HCl / Cl^-, and HCN / CN^-, complete the following eq

step 1 If the equilibrium constant is having a value greater than one, then the reaction must proceed t

Of the conjugate acid-base pairs HF / F^-, HCl / Cl^-, and...

Of the conjugate acid-base pairs $\mathrm{HF} / \mathrm{F}^{-}, \mathrm{HCl} / \mathrm{Cl}^{-},$ and $\mathrm{HCN} / \mathrm{CN}^{-},$ complete the following equation with the pair that gives an equilibrium constant $K_{\mathrm{c}} >1$ _____ $+\mathrm{H}_{2} \mathrm{PO}_{4}^{-} \longrightarrow$ _____ $+\mathrm{H}_{3} \mathrm{PO}_{4}$

Of the conjugate acid-base pairs $\mathrm{HF} / \mathrm{F}^{-}, \mathrm{HCl} / \mathrm{Cl}^{-},$ and
$\mathrm{HCN} / \mathrm{CN}^{-},$ complete the following equation with the
pair that gives an equilibrium constant $K_{\mathrm{c}} >1$
_____ $+\mathrm{H}_{2} \mathrm{PO}_{4}^{-} \longrightarrow$ _____ $+\mathrm{H}_{3} \mathrm{PO}_{4}$

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Key Concepts

Conjugate Acid–Base Pairs

Conjugate acid–base pairs consist of an acid and its corresponding base that differs by one proton. Analyzing reactions by comparing the relative acid strengths of these pairs helps to predict the outcome of the proton transfer process. When choosing between different conjugate pairs, one compares the acidities (pKa values) to determine which reaction is thermodynamically favored.

pKa and Equilibrium Constants

The pKa value of an acid quantifies its acidity; lower pKa indicates a stronger acid. For a proton transfer reaction, the equilibrium constant can be estimated by the difference in pKa values between the acid donating the proton and the acid formed in the reaction. A reaction in which the product acid has a higher pKa than the initial acid will generally have an equilibrium constant greater than one, favoring product formation.

Acid–Base Equilibria

Acid–base equilibria involve the transfer of protons between acidic and basic species. The direction of the reaction is determined by the relative acid strengths, where a proton is transferred from a stronger acid to the conjugate base of a weaker acid, driving the equilibrium towards the formation of the weaker acid.

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