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Chapter 14: Problem 17

Can the pH of a solution be negative? Explain.

Short Answer

Expert verified
Yes, the pH of a solution can be negative. This occurs in extremely acidic solutions with exceptionally high hydrogen ion concentrations (\([H^+]\)) which result in a negative logarithm value in the pH formula (pH = -log10[H+]). Though unusual, negative pH values represent a higher acidity level than solutions with pH close to 0.

Step by step solution

01

Basic pH Concept

The pH is a measure of the acidity or alkalinity of a solution. It is calculated using the formula: pH = -log10[H+] where [H+] is the concentration of hydrogen ions (in moles per liter) in the solution. A pH value of 7 is considered neutral, while a pH less than 7 is acidic and a pH greater than 7 is basic (alkaline).
02

Negative pH and the Formula

Since pH is calculated using the formula pH = -log10[H+], a negative pH would indicate a large hydrogen ion concentration, as the negative logarithm of a value greater than 1 will be a negative number. Thus, higher [H+] values will lead to more negative pH values.
03

Acidic Solution and High Hydrogen Ion Concentration

A solution with a high hydrogen ion concentration is considered very acidic. In extreme cases, the concentration may be so high that it results in a negative pH value. While unusual, negative pH values can occur in extremely acidic solutions.
04

Concluding Statement

To conclude, it is possible for the pH of a solution to be negative, albeit in very extreme cases where the hydrogen ion concentration is exceptionally high. This implies a highly acidic solution, representing a greater level of acidity than solutions with pH close to 0.

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Key Concepts

These are the key concepts you need to understand to accurately answer the question.

Hydrogen Ion Concentration
The concentration of hydrogen ions, denoted as \([H^+]\), plays a crucial role in determining the acidity of a solution. Essentially, it measures how many hydrogen ions are present in a liter of solution. This contributes to the overall pH scale that we use to understand the chemical nature of a solution.
  • More hydrogen ions mean the solution is more acidic.
  • Fewer hydrogen ions result in a more basic or alkaline solution.
Understanding \([H^+]\) concentration helps us evaluate how acidic or basic a solution is, as pH is calculated based on these concentrations. It's a central concept when it comes to evaluating solutions in chemistry.
Acidity and Alkalinity
Acidity and alkalinity are two aspects of the pH scale. This scale ranges from 0 to 14:
  • A pH less than 7 indicates an acidic solution.
  • A pH of 7 is considered neutral.
  • A pH greater than 7 indicates a basic or alkaline solution.
The pH scale helps us visualize and understand to what extent a solution is acidic or alkaline. This is important for several applications, from biological systems to industrial processes. Whenever a solution has a low pH, it contains higher amounts of hydrogen ions, making it stronger in terms of acidity.
Negative pH Values
While it might be surprising, negative pH values can occur. This happens in solutions with very high hydrogen ion concentrations. Let's break it down:
  • The pH formula, \(pH = -\log_{10}[H^+]\), shows that a large \([H^+]\) can produce a negative pH.
  • Such values indicate extremely acidic solutions.
  • Negative pH isn鈥檛 common but can appear in special cases, such as with strong acids like concentrated sulfuric acid.
Seeing a negative pH value is rare but when it occurs, it precisely indicates the solution鈥檚 highly acidic nature. Understanding this possibility provides a complete view of the pH spectrum and prepares us for exceptional chemical environments.

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Most popular questions from this chapter

Isocyanic acid \((\mathrm{HNCO})\) can be prepared by heating sodium cyanate in the presence of solid oxalic acid according to the equation $$ 2 \mathrm{NaOCN}(s)+\mathrm{H}_{2} \mathrm{C}_{2} \mathrm{O}_{4}(s) \longrightarrow 2 \mathrm{HNCO}(l)+\mathrm{Na}_{2} \mathrm{C}_{2} \mathrm{O}_{4}(s) $$ Upon isolating pure HNCO \((l),\) an aqueous solution of HNCO can be prepared by dissolving the liquid HNCO in water. What is the pH of a 100 -mL solution of HNCO prepared from the reaction of 10.0 g each of NaOCN and \(\mathrm{H}_{2} \mathrm{C}_{2} \mathrm{O}_{4},\) assuming all of the HNCO produced is dissolved in solution? \(\left(K_{\mathrm{a}} \text { of HNCO }\right.\) \(=1.2 \times 10^{-4} . )\)

For solutions of the same concentration, as acid strength increases, indicate what happens to each of the following (increases, decreases, or doesn't change). $$ \begin{array}{ll}{\text { a. }\left[\mathrm{H}^{+}\right]} & {\text { d. pOH }} \\ {\text { b. pH }} & {\text { e. } K_{\mathrm{a}}} \\ {\text { c. }\left[\mathrm{OH}^{-}\right]}\end{array} $$

Calculate the pH of the following solutions. a. 0.10\(M\) NaOH b. \(1.0 \times 10^{-10} M \mathrm{NaOH}\) c. 2.0 \(\mathrm{M} \mathrm{NaOH}\)

A typical vitamin \(\mathrm{C}\) tablet (containing pure ascorbic acid, \(\mathrm{H}_{2} \mathrm{C}_{6} \mathrm{H}_{6} \mathrm{O}_{6}\) ) weighs \(500 . \mathrm{mg}\) . One vitamin \(\mathrm{C}\) tablet is dissolved in enough water to make 200.0 \(\mathrm{mL}\) of solution. Calculate the \(\mathrm{pH}\) of this solution. Ascorbic acid is a diprotic acid.

Will the following oxides give acidic, basic, or neutral solutions when dissolved in water? Write reactions to justify your answers. a. \(\mathrm{Li}_{2} \mathrm{O}\) b. \(\mathrm{CO}_{2}\) c. \(\mathrm{SrO}\)
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