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Chapter 15: Problem 24

What is the color of bromthymol blue indicator in a solution of \(\mathrm{pH} 7 ?\)

Short Answer

Expert verified
Bromthymol blue is green at pH 7.

Step by step solution

01

Understand Bromthymol Blue Color Range

Bromthymol blue is an acid-base indicator that changes color depending on the pH of the solution. It is yellow in acidic environments (pH < 6), green around neutral pH (about 7), and blue in basic environments (pH > 7.6).
02

Determine the pH of the Solution

In this problem, the pH of the solution is given as 7.
03

Identify the Color at pH 7

Since bromthymol blue is green in a neutral pH environment and the solution has a pH of 7, the indicator will appear green.

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Key Concepts

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

Acid-Base Indicators
Acid-base indicators are substances that change color based on the acidity or basicity of a solution. They are especially useful in experiments to determine the pH level of a given solution. These indicators are usually weak acids or bases that dissociate at specific pH levels. When they dissociate, they form a different color, which is used to visually identify the pH range.

Some key points about acid-base indicators include:
  • They exhibit a visible color change over a specific pH range.
  • Each indicator has its unique pH transition range and different range of colors.
  • The choice of indicator depends on the desired pH range and the nature of the experiment.
Indicators like litmus, phenolphthalein, and methyl orange are among the commonly used ones. They help chemists and students quickly assess whether a solution is acidic, neutral, or basic through simple observation.
Bromthymol Blue
Bromthymol blue is one of the many acid-base indicators used to determine the pH of a solution. It is particularly useful due to its distinct color change, making it easy to use even for beginners. This indicator is most effective in the pH range of 6.0 to 7.6.

In environments:
  • Below pH 6, it appears yellow, indicating an acidic solution.
  • In neutral conditions, around pH 7, the indicator turns green.
  • Above pH 7.6, it shifts to blue, indicating a basic solution.
The ease with which bromthymol blue shifts colors allows users to easily observe pH changes without the need for complex instruments. It is often used in school laboratories and educational demonstrations to help students understand concepts related to pH and acidity.
Neutral pH
Neutral pH is defined as the midpoint of the pH scale, typically recognized as a pH of 7. In a neutral solution, the concentration of hydrogen ions \((H^+)\) equals the concentration of hydroxide ions \((OH^-)\). This balance results in a solution that is neither acidic nor basic.

Water is the most common example of a neutral substance. In laboratory settings, a neutral solution often serves as the benchmark against which acidic or basic solutions are measured.
  • Neutral solutions do not change the color of acid-base indicators like bromthymol blue, which appears green at neutral pH.
  • Understanding neutral pH is critical for conducting experiments that require precise pH control.
Grasping what neutral pH signifies helps in discerning how different substances can alter the pH and why maintaining pH balance is crucial in scientific processes.

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Most popular questions from this chapter

Write the net ionic equation for the reaction of the strong electrolytes nitric acid and potassium hydroxide.

State whether each of the following substances in an aqueous solution is highly ionized or slightly ionized: (a) weak acids (b) weak bases (c) slightly soluble ionic compounds

Classify each of the following acids as a strong or weak electrolyte: (a) \(\mathrm{HF}(a q)\) (b) \(\mathrm{HCl}(a q)\) (c) \(\mathrm{HNO}_{3}(a q)\) (d) \(\mathrm{HNO}_{2}(a q)\)

Classify each of the following Arrhenius bases as strong or weak given the degree of ionization: (a) lithium hydroxide, \(\mathrm{LiOH}(a q), \sim 100 \%\) (b) calcium hydroxide, \(\mathrm{Ca}(\mathrm{OH})_{2}(a q), \sim 100 \%\) (c) barium hydroxide, \(\mathrm{Ba}(\mathrm{OH})_{2}(a q), \sim 100 \%\) (d) ammonium hydroxide, \(\mathrm{NH}_{4} \mathrm{OH}(a q), \sim 1 \%\)

Classify each of the following Arrhenius acids as strong or weak given the degree of ionization: (a) acetic acid, \(\mathrm{HC}_{2} \mathrm{H}_{3} \mathrm{O}_{2}(a q), \sim 1 \%\) (b) carbonic acid, \(\mathrm{H}_{2} \mathrm{CO}_{3}(a q), \sim 1 \%\) (c) chlorous acid, \(\mathrm{HClO}_{2}(a q), \sim 1 \%\) (d) chloric acid, \(\mathrm{HClO}_{3}(a q), \sim 100 \%\)
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