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Chapter 16: Problem 3

What does it mean to say that a substance has a neutral pH?

Short Answer

Expert verified
A neutral pH of 7 means equal concentrations of hydrogen ions and hydroxide ions in a solution.

Step by step solution

01

Understanding pH Scale

pH is a scale used to specify how acidic or basic (alkaline) a water-based solution is. The pH scale ranges from 0 to 14, with 7 being considered neutral.
02

Neutral pH Explained

A neutral pH value of 7 means that the concentration of hydrogen ions \([H^+]\) in the solution is equal to the concentration of hydroxide ions \([OH^-]\). This balance signifies neither acidic nor basic properties.

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Key Concepts

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

Neutral pH
The concept of a neutral pH is fundamental in understanding the pH scale. On the scale, a pH of 7 is designated as neutral. This is where the concentration of hydrogen ions \( \text{[}H^+\text{]} \) and hydroxide ions \( \text{[}OH^-\text{]} \) are equal.

In a neutral solution:
  • There is no excess of acidic or basic characteristics.
  • The solution maintains a balanced state, with no dominance of hydrogen ions or hydroxide ions.
This state is typically found in pure water and has significant implications for chemical reactions, which often depend on the pH level of the environment.
Acidic Solutions
Acidic solutions have a pH less than 7. They have a higher concentration of hydrogen ions \( \text{[}H^+\text{]} \) compared to hydroxide ions \( \text{[}OH^-\text{]} \).

Key characteristics of acidic solutions include:
  • Taste: They usually taste sour. A common example is lemon juice.
  • Reactivity: They react with metals to produce hydrogen gas.
  • Conductivity: Acidic solutions can conduct electricity due to their ionic nature.
These characteristics make acids essential in numerous industrial and household processes. Their chemical behaviors are highly influenced by the concentration of hydrogen ions within them.
Basic Solutions
Basic solutions, also known as alkaline solutions, have a pH greater than 7. In these solutions, there are more hydroxide ions \( \text{[}OH^-\text{]} \) than hydrogen ions \( \text{[}H^+\text{]} \).

Important features include:
  • Taste: They tend to have a bitter taste.
  • Feel: They often feel slippery to touch, like soap.
  • Reactions: Basic solutions can neutralize acids, forming salts and water.
A common household base is baking soda. Basic solutions are integral in cleaning, manufacturing, and are crucial in biology for maintaining pH balance.
Hydrogen Ions
Hydrogen ions \( \text{[}H^+\text{]} \) play a critical role in defining the acidity of a solution. They are generated when an acid dissolves in water. The greater the concentration of hydrogen ions, the more acidic the solution becomes.

When studying hydrogen ions:
  • They are highly reactive and can influence the rate and outcome of reactions.
  • They are fundamental in processes like metabolism and respiration.
  • Their presence can drastically affect the environment, often determining the behavior of the solution.
Understanding how hydrogen ions work is essential in fields like chemistry and biology.
Hydroxide Ions
Hydroxide ions \( \text{[}OH^-\text{]} \) determine the basicity of a solution. When a base dissolves in water, it increases the concentration of hydroxide ions, which makes the solution basic.

Key points about hydroxide ions include:
  • They are important in neutralizing excess acids, forming water in the process.
  • Hydroxide ions are involved in reactions that involve the formation of salt.
  • They affect both chemical equilibrium and biological processes.
Hydroxide ions are crucial in many industrial processes, such as soap making and water purification. Their balancing role in solutions highlights their importance in chemistry and everyday life.

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Most popular questions from this chapter

Explain why aqueous washing soda, \(\mathrm{Na}_{2} \mathrm{CO}_{3},\) is a basic solution.

What is a neutralization reaction?

What \(\mathrm{H}^{+}\) concentration would you expect for the solutions below? $$ \begin{array}{ll}{\text { a. } \mathrm{pH}=9} & {\text { b. } \mathrm{pH}=7.3} \\\ {\text { c. } \mathrm{pH}=2.9} & {\text { d. } \mathrm{pH}=10.2}\end{array} $$

What is the relationship between \(\mathrm{pH}\) and \(\mathrm{H}^{+}\) concentration?

Predict the products for the reactions given below. Be sure to balance each equation. a. \(\mathrm{HF}(a q)+\mathrm{NaOH}(a q) \longrightarrow\) b. \(\mathrm{HCl}(a q)+\mathrm{Mg}(\mathrm{OH})_{2}(a q) \longrightarrow\) c. \(\mathrm{HF}(a q)+\mathrm{N} \mathrm{H}_{4} \mathrm{OH}(a q) \longrightarrow\) d. \(\mathrm{CH}_{3} \mathrm{COOH}(a q)+\mathrm{NaOH}(a q) \longrightarrow\) e. \(\mathrm{HNO}_{3}(a q)+\mathrm{Mg}(\mathrm{OH})_{2}(a q) \longrightarrow\) f. \(\mathrm{HNO}_{3}(a q)+\mathrm{NH}_{4} \mathrm{OH}(a q) \longrightarrow\) g. \(\mathrm{CH}_{3} \mathrm{COOH}(a q)+\mathrm{Mg}(\mathrm{OH})_{2}(a q) \longrightarrow\) \(\mathrm{h} . \mathrm{CH}_{3} \mathrm{COOH}(a q)+\mathrm{NH}_{4} \mathrm{OH}(a q) \longrightarrow\) i. \(\mathrm{H}_{2} \mathrm{SO}_{4}(a q)+\mathrm{HNO}_{3}(a q) \longrightarrow\) j. \(\mathrm{H}_{2} \mathrm{SO}_{4}(a q)+\mathrm{Mg}(\mathrm{OH})_{2}(a q) \longrightarrow\)
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