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Chapter 15: Problem 63

Which of the following \(\mathrm{pH}\) values indicate an acidic solution at \(25^{\circ} \mathrm{C} ?\) Which are basic and which are neutral? a) 4.6 b)7.0 c) 1.6 d) 10.5

Short Answer

Expert verified
pH 4.6 and 1.6 are acidic; pH 7.0 is neutral; pH 10.5 is basic.

Step by step solution

01

Understanding pH Scale

At a temperature of \(25^{\circ} \mathrm{C}\), the \(\mathrm{pH}\) scale ranges from 0 to 14. A \(\mathrm{pH}\) less than 7 indicates an acidic solution, a \(\mathrm{pH}\) of 7 indicates a neutral solution, and a \(\mathrm{pH}\) greater than 7 indicates a basic or alkaline solution.
02

Analyze Each Value

- For \(\mathrm{pH} = 4.6\): Since 4.6 is less than 7, this is an acidic solution. - For \(\mathrm{pH} = 7.0\): As it equals 7, this is a neutral solution. - For \(\mathrm{pH} = 1.6\): Being less than 7, this is an acidic solution. - For \(\mathrm{pH} = 10.5\): Since 10.5 is greater than 7, this is a basic solution.

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Key Concepts

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

Acidic Solutions
The pH scale is a tool that helps us determine the acidity or alkalinity of a solution. Solutions with a pH less than 7 are considered acidic. This occurs because they have a high concentration of hydrogen ions (\(H^+\)). Acidic solutions can vary in their level of acidity.
  • A solution with a pH of 1.6 is highly acidic, similar to the acidity found in gastric acid in your stomach.
  • Another example is a solution with a pH of 4.6, which is less acidic but still falls in the acidic range, similar to the acidity of certain fruit juices.
Acids can have many applications, ranging from use in cleaning products to playing critical roles in biological processes within our bodies. It's important to handle strong acids with care due to their corrosive nature.
Neutral Solutions
A neutral solution is perfectly balanced on the pH scale with a pH of 7. At this pH level, the concentration of hydrogen ions (\(H^+\)) and hydroxide ions (\(OH^-\)) is equal. This balance results in a solution that is neither acidic nor basic. The most common example of a neutral solution is pure water. It has a stable environment for most biological processes to occur. Neutral solutions also act as good starting points for various experiments and reactions because they do not bias a reaction towards acidity or basicity.Understanding neutral solutions is essential for fields such as chemistry and biology, where maintaining precise chemical balances is vital.
Basic Solutions
Basic solutions, also known as alkaline solutions, have a pH greater than 7 and are characterized by a higher concentration of hydroxide ions (\(OH^-\)). These solutions can neutralize acids and are typically slippery to the touch.

Common substances with basic properties include:
  • Sodium bicarbonate solution, typically used in baking.
  • Ammonia solution, often used as a household cleaner.
Given a solution with a pH of 10.5, it is clearly basic, as it is well above the neutral pH of 7. Basic solutions can have important applications, including neutralizing acidic substances and playing roles in various industrial processes. It's important to handle them with care due to their potential to cause harm on contact with the skin.

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Most popular questions from this chapter

An antiseptic solution at \(25^{\circ} \mathrm{C}\) has a hydroxide-ion concentration of \(8.4 \times 10^{-5} M .\) Is the solution acidic, neutral, or basic?

Morphine is a narcotic that is used to relieve pain. A solution of morphine has a pH of 9.61 at \(25^{\circ} \mathrm{C}\). What is the hydroxide-ion concentration?

Aqueous solutions of ammonia, \(\mathrm{NH}_{3},\) were once thought to be solutions of an ionic compound (ammonium hydroxide, \(\mathrm{NH}_{4} \mathrm{OH}\) ) in order to explain how the solutions could contain hydroxide ion. Using the Bronsted-Lowry concept, show how \(\mathrm{NH}_{3}\) yields hydroxide ion in aqueous solution without involving the species \(\mathrm{NH}_{4} \mathrm{OH}\).

A sample of vinegar has a hydronium-ion concentration of \(3.0 \times 10^{-3} M .\) What is the \(\mathrm{pH}\) of the vinegar?

How is sodium hydroxide prepared commercially?
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