Calculate the pH of each solution. (a) [H3 O^+]=1.7 ×10^-8 M (b) [H3 O^+]=1.0 ×10^-7 M (c) [H3 O

step 1 The pH and the hydronium concentration are related to each other. pH is simply the negative log

Calculate the pH of each solution. (a) [H3 O^+]=1.7 ×10^-8 M...

Calculate the pH of each solution. (a) $\left[\mathrm{H}_{3} \mathrm{O}^{+}\right]=1.7 \times 10^{-8} \mathrm{M}$ (b) $\left[\mathrm{H}_{3} \mathrm{O}^{+}\right]=1.0 \times 10^{-7} \mathrm{M}$ (c) $\left[\mathrm{H}_{3} \mathrm{O}^{+}\right]=2.2 \times 10^{-6} \mathrm{M}$ (d) $\left[\mathrm{H}_{3} \mathrm{O}^{+}\right]=7.4 \times 10^{-4} \mathrm{M}$

Calculate the pH of each solution.
(a) $\left[\mathrm{H}_{3} \mathrm{O}^{+}\right]=1.7 \times 10^{-8} \mathrm{M}$
(b) $\left[\mathrm{H}_{3} \mathrm{O}^{+}\right]=1.0 \times 10^{-7} \mathrm{M}$
(c) $\left[\mathrm{H}_{3} \mathrm{O}^{+}\right]=2.2 \times 10^{-6} \mathrm{M}$
(d) $\left[\mathrm{H}_{3} \mathrm{O}^{+}\right]=7.4 \times 10^{-4} \mathrm{M}$

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Key Concepts

Hydronium Ion Concentration

The hydronium ion concentration (usually expressed in molarity, M) directly determines the pH of a solution. In acid-base chemistry, the amount of H3O+ present is critical, as it communicates the acid strength in the solution. Small changes in these concentrations can lead to significant shifts in pH due to the logarithmic relationship.

Logarithmic Properties in pH

Logarithms are essential in pH calculations because they convert multiplicative relationships into additive ones, simplifying the handling of very large or very small numbers. The use of the base-10 logarithm in the pH formula allows chemists to express acidic or basic strengths on a scale from 0 to 14, which is more intuitive for analysis and comparison.

pH Calculation

The calculation of pH is central to understanding the acidity or basicity of a solution. pH is defined as the negative base-10 logarithm of the hydronium ion concentration (-log[H3O+]). This transformation converts the wide range of hydrogen ion concentrations into a more manageable scale, making it easier to compare the relative strengths of acids and bases.

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