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Chapter 16: Problem 12

Define \(\mathrm{pH}\). Why do chemists normally choose to discuss the acidity of a solution in terms of \(\mathrm{pH}\) rather than hydrogen ion concentration, \(\left[\mathrm{H}^{+}\right] ?\)

Short Answer

Expert verified
\(\mathrm{pH}\) is defined as the negative logarithm (to base 10) of the concentration of hydrogen ions, \(\left[\mathrm{H}^{+}\right]\). It is easier and more convenient to discuss the acidity of a solution in terms of \(\mathrm{pH}\) rather than hydrogen ion concentration, \(\left[\mathrm{H}^{+}\right]\), because \(\mathrm{pH}\) varies on a simpler scale and a one-unit change in \(\mathrm{pH}\) corresponds to a tenfold change in \(\left[\mathrm{H}^{+}\right]\) which is more intuitive to comprehend.

Step by step solution

01

Definition of pH

The \(\mathrm{pH}\) of a solution is defined as the negative logarithm (to base 10) of the concentration of hydrogen ions, \(\left[\mathrm{H}^{+}\right]\) in a solution. The formula is expressed as: \(\mathrm{pH} = -\log[\mathrm{H}^{+}]\)
02

Why pH is used instead of \([H^{+}]\)

Chemists use \(\mathrm{pH}\) rather than \(\left[\mathrm{H}^{+}\right]\) for a few reasons. Firstly, the scale of hydrogen ion concentrations in solutions can vary widely from very large to very small values (for example, from 1.0 M to 0.0000001 M). Using \(\mathrm{pH}\) provides a convenient way to express these values on a simpler scale (from 0 to 14) making it easier to compare the concentrations in different solutions. Secondly, \(\mathrm{pH}\) is a logarithmic measurement, so a one-unit change in \(\mathrm{pH}\) corresponds to a tenfold change in \(\left[\mathrm{H}^{+}\right]\), which is more intuitive for understanding the relative acidity or alkalinity of solutions.

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Most popular questions from this chapter

A solution is made by dissolving \(18.4 \mathrm{~g}\) of \(\mathrm{HCl}\) in 662 \(\mathrm{mL}\) of water. Calculate the \(\mathrm{pH}\) of the solution. (Assume that the volume of the solution is also \(662 \mathrm{~mL} .)\)

Hydrocyanic acid (HCN) is a weak acid and a deadly poisonous compound that, in the gaseous form (hydrogen cyanide), is used in gas chambers. Why is it dangerous to treat sodium cyanide with acids (such as HCl) without proper ventilation?

\(\mathrm{H}_{2} \mathrm{SO}_{4}\) is a strong acid, but \(\mathrm{HSO}_{4}^{-}\) is a weak acid. Account for the difference in strength of these two related species.

List the factors on which the \(K_{\mathrm{a}}\) of a weak acid depends.

What are the concentrations of \(\mathrm{HSO}_{4}^{-}, \mathrm{SO}_{4}^{2-},\) and \(\mathrm{H}^{+}\) in a \(0.20 \mathrm{M} \mathrm{KHSO}_{4}\) solution? (Hint: \(\mathrm{H}_{2} \mathrm{SO}_{4}\) is a strong acid: \(K_{\mathrm{a}}\) for \(\left.\mathrm{HSO}_{4}^{-}=1.3 \times 10^{-2} .\right)\)
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