Write the chemical equation for the ionization of the...

Write the chemical equation for the ionization of the following weak acids. Assume only one hydrogen ionizes in all cases. (a) hydrazoic acid, $\mathrm{HN}_{3}$ (b) citric acid, $\mathrm{H}_{2} \mathrm{C}_{6} \mathrm{H}_{6} \mathrm{O}_{7}$ (c) squaric acid, $\mathrm{H}_{2} \mathrm{C}_{4} \mathrm{O}_{4}$

Write the chemical equation for the ionization of the following weak acids. Assume only one hydrogen ionizes in all cases.
(a) hydrazoic acid, $\mathrm{HN}_{3}$
(b) citric acid, $\mathrm{H}_{2} \mathrm{C}_{6} \mathrm{H}_{6} \mathrm{O}_{7}$
(c) squaric acid, $\mathrm{H}_{2} \mathrm{C}_{4} \mathrm{O}_{4}$

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Key Concepts

Polyprotic Acids

Polyprotic acids contain more than one ionizable hydrogen atom. However, when writing chemical equations for their ionization, it is common to focus on the first ionization step (assuming only one hydrogen ionizes) to simplify the analysis, especially when studying acid strength and equilibrium behavior.

Chemical Equation Writing

Writing chemical equations for acid ionization requires representing both the reactants and the products of the reaction accurately. The equations must be balanced in terms of both atoms and charge, reflecting the conservation of mass and charge during the ionization process.

Acid Ionization

Acid ionization refers to the process in which an acid donates a proton (hydrogen ion) to the surrounding solution, resulting in the formation of its conjugate base. This concept is fundamental in understanding how acids behave in water and how they interact with bases.

Weak Acids

Weak acids do not completely ionize in solution, meaning that only a portion of the acid molecules release a proton. As a result, an equilibrium is established between the undissociated acid, the hydrogen ion, and its conjugate base, distinguishing weak acids from strong acids which ionize fully.

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