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Chapter 12: Problem 16

What is the pOH range for a basic solution?

Short Answer

Expert verified
The pOH range for a basic solution is less than 7.

Step by step solution

01

Understanding the pOH Scale

The pOH scale measures the hydroxide ion concentration in a solution, similar to how the pH scale measures the hydrogen ion concentration. The pOH scale ranges from 0 to 14, where lower values indicate higher hydroxide ion concentration (more basic) and higher values indicate lower hydroxide ion concentration (less basic or more acidic).
02

Defining a Basic Solution

A basic solution is any solution with a pH greater than 7. In terms of the pOH scale, this corresponds to a pOH less than 7 because pH and pOH are related by the equation: \[ \text{pH} + \text{pOH} = 14 \] This means as pH increases above 7, pOH must decrease below 7.
03

Determining the Basic Range for pOH

Since basic solutions have a pH greater than 7, their corresponding pOH values will be less than 7 due to the relation \[ \text{pH} + \text{pOH} = 14 \] . Hence, the pOH range for a basic solution is any value less than 7.

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Key Concepts

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

pH Scale
The pH scale is a measurement used to determine the acidity or basicity of a solution. Ranging from 0 to 14, it indicates the concentration of hydrogen ions (\[ [H^+] \]) in the solution. A pH value of 7 is considered neutral, meaning the solution has an equal concentration of hydrogen and hydroxide ions.
  • Values lower than 7 indicate acidic solutions, with higher hydrogen ion concentrations.
  • Values higher than 7 indicate basic solutions, where hydroxide ions are more concentrated.
The formula used to calculate pH is:\[ \text{pH} = -\log_{10} [H^+] \]This logarithmic scale means that each unit change represents a tenfold change in hydrogen ion concentration.
pOH Scale
Much like the pH scale, the pOH scale is used to measure the concentration of hydroxide ions (\[ [OH^-] \]) in a solution. It also ranges from 0 to 14, but operates opposite to the pH scale.
  • Lower pOH values (below 7) indicate basic solutions with higher hydroxide ion concentrations.
  • Higher pOH values (above 7) indicate acidic solutions with lower hydroxide ion concentrations.
The relationship between pH and pOH is crucial and is given by the equation:\[ \text{pH} + \text{pOH} = 14 \]This equation helps to find the pOH when the pH of a solution is known and vice versa.
Hydroxide Ion Concentration
The concentration of hydroxide ions in a solution plays a crucial role in determining whether a solution is acidic or basic. It is closely linked to the pOH scale:
  • High hydroxide ion concentration corresponds to low pOH values, indicating a basic solution.
  • Low hydroxide ion concentration corresponds to high pOH values, indicating an acidic solution.
The concentration of hydroxide ions can be calculated from pOH using the formula:\[ [OH^-] = 10^{-\text{pOH}} \]This equation provides a direct way to determine hydroxide ion concentration from the pOH value of the solution.
Acidic vs. Basic Solutions
Understanding the difference between acidic and basic solutions is fundamental in chemistry:
  • Acidic solutions have a pH less than 7, high hydrogen ion concentration, and are characterized by a pOH greater than 7.
  • Basic solutions have a pH greater than 7, high hydroxide ion concentration, and are characterized by a pOH less than 7.
These properties are essential in various chemical processes and reactions. Acidity and basicity affect the behavior of substances in a solution, influencing reactions they undergo and their applications. The interplay between \( ext{pH} \) and \( ext{pOH} \) guides the preparation and use of numerous chemical solutions in everyday life. It highlights why solutions that are more basic have lower pOH values.

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Most popular questions from this chapter

What is \(\left[\mathrm{H}^{+}\right]\) for a neutral solution?

A lab technician mixes a solution of \(0.55 \mathrm{M} \mathrm{HNO}_{3}\). Is the resulting \(\mathrm{H}^{+}\) concentration greater than, equal to, or less than 0.55 M? Explain your answer.

Write the reverse of the reaction for the autoionization of water. It is still an acid-base reaction? If so, label the acid and base.

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What is the \(\mathrm{pH}\) of a solution when \(\left[\mathrm{H}^{+}\right]\) is \(3.44 \times 10^{-4} \mathrm{M}\) ?
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