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Chapter 15: Problem 31

Describe a solution (solute and concentration) that has a negative pH value.

Short Answer

Expert verified
Answer: An example of a highly acidic solution with a negative pH value is a hydrochloric acid (HCl) solution with a concentration greater than 1 mol/L. The pH value is determined by the formula pH = -log10(H+), where H+ is the concentration of hydrogen ions equal to the concentration of the HCl solution, resulting in a negative pH value.

Step by step solution

01

1. Choose an acidic solute.

We will consider hydrochloric acid (HCl) as our acidic solute. Hydrochloric acid is a strong acid and will fully dissociate in water, producing a high concentration of hydrogen ions (\(H^{+}\)) and chloride ions (\(Cl^{-}\)).
02

2. Determine the concentration of the HCl solution.

In order to have a negative pH value, the concentration of hydrogen ions, \([H^{+}]\), must be greater than 1 mol/L. Since hydrochloric acid (HCl) dissociates completely in water, the concentration of hydrogen ions (\(H^{+}\)) will be equal to the concentration of the HCl solution. Therefore, we need an HCl solution with a concentration greater than 1 mol/L.
03

3. Calculate the pH value of the solution.

To calculate the pH value of our HCl solution, we use the formula \(pH = -log_{10}(H^{+})\). The concentration of hydrogen ions, \([H^{+}]\), is equal to the concentration of the HCl solution, so we have \(pH = -log_{10}(c)\), where \(c\) is the concentration of HCl solution. Since \(c > 1\) mol/L, the pH value will be negative.
04

4. Describe the solution.

The solution consisting of hydrochloric acid (HCl) with a concentration greater than 1 mol/L will have a negative pH value, making it a highly acidic solution.

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Most popular questions from this chapter

Are all Arrhenius acids also Bronsted-Lowry acids? Are all Bronsted-Lowry acids also Arrhenius acids? If yes, explain why. If not, give a specific example to demonstrate the difference.

When \(1,\) 2-diaminoethane, \(\mathrm{H}_{2} \mathrm{NCH}_{2} \mathrm{CH}_{2} \mathrm{NH}_{2},\) dissolves in water, the resulting solution is basic. Write the formula of the ionic compound that is formed when hydrochloric acid is added to a solution of 1,2 -diaminoethane.

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Identify the conjugate acid of each of the following species: \(\left(\mathrm{CH}_{3}\right)_{3} \mathrm{N}, \mathrm{CH}_{3} \mathrm{COO}^{-}, \mathrm{HSO}_{4}^{-},\) and \(\mathrm{OH}^{-}\)

Calculate the \(p \mathrm{H}\) of \(6.9 \times 10^{-8} \mathrm{MHBr}\)
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