What is the pH of a 0.1500 M H2 SO4 solution if (a) the ionization of HSO4^- is ignored? (b) the

step 1 So we're talking about H2S .O4 here. If we simply look at the first ionization that makes H plus

What is the pH of a 0.1500 M H2 SO4 solution if (a) the...

What is the $\mathrm{pH}$ of a $0.1500 \mathrm{M} \mathrm{H}_{2} \mathrm{SO}_{4}$ solution if (a) the ionization of $\mathrm{HSO}_{4}^{-}$ is ignored? (b) the ionization of $\mathrm{HSO}_{4}^{-}$ is taken into account? $\left(K_{\mathrm{a}}\right.$ for $\mathrm{HSO}_{4}^{-}$ is $1.1 \times 10^{-2} .$

What is the $\mathrm{pH}$ of a $0.1500 \mathrm{M} \mathrm{H}_{2} \mathrm{SO}_{4}$ solution if
(a) the ionization of $\mathrm{HSO}_{4}^{-}$ is ignored?
(b) the ionization of $\mathrm{HSO}_{4}^{-}$ is taken into account? $\left(K_{\mathrm{a}}\right.$ for $\mathrm{HSO}_{4}^{-}$ is $1.1 \times 10^{-2} .$

Key Concepts

pH Calculation

Calculated as the negative base-10 logarithm of the hydrogen ion concentration, the pH is a measure of the acidity of a solution. When multiple ionization steps contribute to the overall hydrogen ion concentration, it is essential to account for both complete and partial dissociations to obtain an accurate pH value.

Equilibrium Constant (Ka)

The equilibrium constant, denoted as Ka, quantifies the extent of ionization for a weak acid. It is defined as the ratio of the concentrations of the products (hydrogen ions and the conjugate base) to the concentration of the undissociated acid at equilibrium. In situations where a weak ionization is involved, such as the second step of a diprotic acid, the Ka value is crucial for calculating the additional concentration of hydrogen ions.

Strong Acid Ionization

This concept refers to the complete and rapid dissociation of strong acids in aqueous solution. For example, in the case of a diprotic acid, the first dissociation step is often treated as complete, meaning that all the acid molecules donate their proton, thereby significantly increasing the hydrogen ion concentration in the solution.

Weak Acid Ionization

Weak acid ionization describes the partial dissociation of an acid in solution, where only a fraction of the acid molecules donate a proton. For diprotic acids, the second dissociation step is typically weak, requiring equilibrium considerations to determine how much additional hydrogen ion concentration results from the partial ionization.

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