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Chapter 16: Problem 8

Can the \(\mathrm{pH}\) of a solution be negative? Explain.

Short Answer

Expert verified
Yes, the \(\mathrm{pH}\) of a solution can be negative. This occurs when the concentration of hydrogen ions (\(H_3O^+\)) in the solution is greater than 1, which indicates a highly acidic solution. Although the typical \(\mathrm{pH}\) scale ranges from 0 to 14, it can extend beyond this range based on the acidity or basicity of a solution.

Step by step solution

01

Definition of pH

The \(\mathrm{pH}\) of a solution is defined as the negative logarithm of the hydronium ion concentration (\([H_3O^+]\)), which is the concentration of hydrogen ions (H+). Mathematically, it is expressed as: $$ \mathrm{pH} = -\log_{10} [H_3O^+] $$
02

Range of \(\mathrm{pH}\)

Normally, the \(\mathrm{pH}\) scale ranges from 0 to 14, where a \(\mathrm{pH}\) of 7 is neutral, a \(\mathrm{pH}\) less than 7 is acidic, and a \(\mathrm{pH}\) greater than 7 is basic. In principle, the \(\mathrm{pH}\) scale can extend beyond this range based on the concentration of hydrogen ions in the solution.
03

Negative \(\mathrm{pH}\)

Since the \(\mathrm{pH}\) is a logarithmic scale, it is possible to have negative \(\mathrm{pH}\) values. Remember that the formula for \(\mathrm{pH}\) is: $$ \mathrm{pH} = -\log_{10} [H_3O^+] $$ To have a negative \(\mathrm{pH}\), \(-\log_{10} [H_3O^+]\) needs to be negative, meaning that the \(\log_{10} [H_3O^+]\) needs to be positive. This will happen when the concentration of hydrogen ions in the solution is more than 1: $$ [H_3O^+] > 1 $$ Solutions like this are strongly acidic, and can indeed have negative \(\mathrm{pH}\) values.
04

Conclusion

The \(\mathrm{pH}\) of a solution can be negative. This happens when the concentration of hydrogen ions (\(H_3O^+\)) in the solution is greater than 1, indicating a highly acidic solution. Although the conventional \(\mathrm{pH}\) scale ranges from 0 to 14, it can extend beyond this range depending on the acidity or basicity of a solution.

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Most popular questions from this chapter

Differentiate among the terms concentrated, dilute, weak, and strong in describing acids. Use molecularlevel pictures to support your answer.

Choose the answer that best completes the following statement and defend your answer. When \(100.0 \mathrm{mL}\) of water is added to \(100.0 \mathrm{mL}\) of \(1.00 \mathrm{M} \mathrm{HCl}\) a. the pH decreases because the solution is diluted. b. the pH does not change because water is neutral. c. the \(\mathrm{pH}\) is doubled because the volume is now doubled. d. the pH increases because the concentration of \(\mathrm{H}^{+}\) decreases. e. the solution is completely neutralized.

Explain why \(\mathrm{Cl}^{-}\) does not affect the \(\mathrm{pH}\) of an aqueous solution.

What is meant by "pH"? True or false: A strong acid always has a lower pH than a weak acid does. Explain.

Mixing together aqueous solutions of acetic acid and sodium hydroxide can make a buffered solution. Explain.
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