Do the equilibria of the following acid-base reactions lie...

Do the equilibria of the following acid-base reactions lie to the right or the left? (The $\left.\mathrm{p} K_{\mathrm{a}} \text { of } \mathrm{H}_{2} \mathrm{O}_{2} \text { is } 11.6 .\right)$ $$\begin{aligned}\mathrm{HOOH}+\mathrm{HO}^{-} & \rightleftharpoons \mathrm{HOO}^{-}+\mathrm{H}_{2} \mathrm{O} \\ \mathrm{RC} \equiv \mathrm{CH}+\mathrm{HOO}^{-} & \rightleftharpoons \mathrm{RC} \equiv \mathrm{C}^{-}+\mathrm{HOOH} \end{aligned}$$

Do the equilibria of the following acid-base reactions lie to the right or the left? (The $\left.\mathrm{p} K_{\mathrm{a}} \text { of } \mathrm{H}_{2} \mathrm{O}_{2} \text { is } 11.6 .\right)$
$$\begin{aligned}\mathrm{HOOH}+\mathrm{HO}^{-} & \rightleftharpoons \mathrm{HOO}^{-}+\mathrm{H}_{2} \mathrm{O} \\ \mathrm{RC} \equiv \mathrm{CH}+\mathrm{HOO}^{-} & \rightleftharpoons \mathrm{RC} \equiv \mathrm{C}^{-}+\mathrm{HOOH} \end{aligned}$$

Key Concepts

Acid?Base Equilibria

Acid?base equilibria involve reactions where acids donate protons to bases, forming conjugate acid-base pairs. The position of the equilibrium depends on the relative strengths of the reacting acids and bases, with the system favoring the side that produces the weaker acid and base.

pKa

The pKa is a quantitative measure of acidity, indicating the tendency of an acid to donate its proton. It is defined as the negative logarithm of the acid dissociation constant (Ka), and helps predict the position of acid-base equilibria—the lower the pKa, the stronger the acid.

Conjugate Acid?Base Pairs

Conjugate acid?base pairs consist of an acid and its corresponding base, which differ by one proton. Understanding these pairs is crucial because the strength of the conjugate acid relative to its base (and vice versa) influences the direction in which an acid-base reaction will proceed.

Equilibrium Position Determination

Determining the equilibrium position in acid-base reactions involves comparing the acid strengths (via pKa values) of the reactants and products. The reaction tends to favor the formation of the weaker acid and base, shifting the equilibrium towards the side that stabilizes these species.

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