Place the species in each of the following groups in order...

Place the species in each of the following groups in order of increasing acid strength. Explain the order you chose for each group. a. $\mathrm{HIO}_{3}, \mathrm{HBrO}_{3}$ b. $\mathrm{HNO}_{2}, \mathrm{HNO}_{3}$ c. HOCI, HOI d. $\mathrm{H}_{3} \mathrm{PO}_{4}, \mathrm{H}_{3} \mathrm{PO}_{3}$

Place the species in each of the following groups in order of increasing acid strength. Explain the order you chose for each group.
a. $\mathrm{HIO}_{3}, \mathrm{HBrO}_{3}$
b. $\mathrm{HNO}_{2}, \mathrm{HNO}_{3}$
c. HOCI, HOI
d. $\mathrm{H}_{3} \mathrm{PO}_{4}, \mathrm{H}_{3} \mathrm{PO}_{3}$

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Key Concepts

Oxyacid Structure and Oxidation States

For compounds containing oxygen bonded to a central atom, the number of oxygens and the oxidation state of the central atom play a crucial role in determining acid strength. A higher oxidation state typically increases the electron-withdrawing power, which in turn stabilizes the conjugate base by delocalizing the negative charge, leading to a stronger acid.

Electronegativity and Inductive Effects

Electronegativity is vital in influencing acid strength as more electronegative atoms near the acidic proton pull electron density away, weakening the O-H bond. This inductive withdrawal makes it easier for the acid to lose a proton, thereby enhancing its acidity.

Resonance Stabilization

Conjugate bases that benefit from resonance stabilization can delocalize the negative charge over multiple atoms. This distribution of charge renders the conjugate base more stable, meaning that the corresponding acid more readily donates its proton, increasing the acid’s strength.

Molecular Structure and Bond Strength

The intrinsic strength of the bond between the hydrogen and the atom to which it is attached (often oxygen) is important. Factors such as the bond polarity and the presence of electron-withdrawing groups can weaken this bond, making proton donation easier and thus increasing the acid’s strength.

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