/*! This file is auto-generated */ .wp-block-button__link{color:#fff;background-color:#32373c;border-radius:9999px;box-shadow:none;text-decoration:none;padding:calc(.667em + 2px) calc(1.333em + 2px);font-size:1.125em}.wp-block-file__button{background:#32373c;color:#fff;text-decoration:none} Problem 12 Which is more acidic, a solution... [FREE SOLUTION] | 91影视

91影视

Log out

Learning Materials

Features

Discover

Chapter 15: Problem 12

Which is more acidic, a solution having a pH of 4 or one having a pH of 5 ?

Short Answer

Expert verified
A solution with a pH of 4 is more acidic than one with a pH of 5.

Step by step solution

01

Understanding pH scale

The pH scale measures the acidity or alkalinity of a solution. It ranges from 0 to 14, where 7 is neutral. Values lower than 7 indicate acidity, and values higher than 7 indicate alkalinity.
02

Comparing pH values

The acidity of a solution is inversely related to its pH value. Lower pH values signify higher acidity. Thus, between a pH of 4 and a pH of 5, the solution with a pH of 4 has a lower pH and is therefore more acidic.
03

Understanding logarithmic nature of pH

The pH scale is logarithmic, meaning each whole number change on the pH scale represents a tenfold change in hydrogen ion concentration. Therefore, a solution with a pH of 4 has ten times more hydrogen ions than a solution with a pH of 5.
04

Conclusion

Based on the pH values, comparing their acidity, and logarithmic nature of the pH scale, it is clear that the solution with a pH of 4 is more acidic than the solution with a pH of 5.

Unlock Step-by-Step Solutions & Ace Your Exams!

  • Full Textbook Solutions

    Get detailed explanations and key concepts

  • Unlimited Al creation

    Al flashcards, explanations, exams and more...

  • Ads-free access

    To over 500 millions flashcards

  • Money-back guarantee

    We refund you if you fail your exam.

Over 30 million students worldwide already upgrade their learning with 91影视!

Key Concepts

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

Acidity
The concept of acidity is central to understanding the behavior of solutions in chemistry. Acidity refers to a solution's ability to donate protons or hydrogen ions ( \( H^+ \) ). The more \( H^+ \) ions a solution can donate, the more acidic it is.
Acids are substances that increase the concentration of hydrogen ions when dissolved in water, leading to a lower pH value.
In terms of the pH scale, which ranges from 0 to 14:
  • Solutions with a pH less than 7 are considered acidic.
  • The lower the pH value, the higher the acidity.
Thus, a solution with a pH of 4 is more acidic than one with a pH of 5, because it can donate more hydrogen ions.
Hydrogen Ion Concentration
Hydrogen ion concentration is a key factor in determining the acidity of a solution. The concentration of hydrogen ions ( \( [H^+] \) ) in a solution dictates its pH level.
A higher concentration of \( H^+ \) ions means a lower pH and higher acidity.
The relationship between hydrogen ion concentration and pH is given by the formula:\[ pH = -\log_{10} [H^+] \]
This formula highlights that:
  • If the \( [H^+] \) is high, the pH value will be low.
  • Conversely, if \( [H^+] \) is low, the pH will be high.
In our exercise, a solution with a pH of 4 has a higher hydrogen ion concentration than one with a pH of 5, making it more acidic.
Logarithmic Scale
The pH scale is logarithmic, meaning it operates on powers of ten. This feature of the pH scale implies that each numerical step on the scale changes the hydrogen ion concentration by a factor of ten.
For example, a solution with a pH of 4 is actually ten times more acidic than a solution with a pH of 5 because \( 10^{-4} \) is ten times larger than \( 10^{-5} \).
The logarithmic nature also means small pH changes can reflect large changes in acidity:
  • A decrease by 1 unit in pH results in a tenfold increase in hydrogen ion concentration.
  • This is why the solution with pH 4 is significantly more acidic than pH 5.
Understanding this logarithmic relationship is crucial for interpreting the pH scale accurately.

One App. One Place for Learning.

All the tools & learning materials you need for study success - in one app.

Get started for free

Most popular questions from this chapter

List the following compounds in order of increasing acid strength: \(\mathrm{HBrO}_{2}, \mathrm{HClO}_{2}, \mathrm{HBrO}\)

Natural gas frequently contains hydrogen sulfide, \(\mathrm{H}_{2} \mathrm{~S}\). \(\mathrm{H}_{2} \mathrm{~S}\) is removed from natural gas by passing it through aqueous ethanolamine, \(\mathrm{HOCH}_{2} \mathrm{CH}_{2} \mathrm{NH}_{2}\) (an ammonia derivative), which reacts with the hydrogen sulfide. Write the equation for the reaction. Identify each reactant as either a Lewis acid or a Lewis base. Explain how you arrived at your answer.

What is meant by the self-ionization of water? Write the expression for \(K_{w} .\) What is its value at \(25^{\circ} \mathrm{C} ?\)

For each of the following, state whether the solution at \(25^{\circ} \mathrm{C}\) is acidic, neutral, or basic: (a) A beverage solution has a pH of 3.5. (b) A \(0.50 M\) solution of potassium bromide, KBr, has a pH of \(7.0 .\) (c) A \(0.050 M\) solution of pyridine, \(\mathrm{C}_{5} \mathrm{H}_{5} \mathrm{~N}\), has a pH of \(9.0\). (d) A solution of iron(III) chloride has a pH of \(5.5\).

Obtain the \(\mathrm{pH}\) corresponding to the following hydronium-ion concentrations. a. \(1.0 \times 10^{-8} M\) b. \(5.0 \times 10^{-12} M\) c. \(7.5 \times 10^{-3} M\) d. \(6.35 \times 10^{-9} M\)
See all solutions

Recommended explanations on Chemistry Textbooks

Chemical Reactions

Read Explanation

Ionic and Molecular Compounds

Read Explanation

Chemistry Branches

Read Explanation

Chemical Analysis

Read Explanation

Physical Chemistry

Read Explanation

The Earths Atmosphere

Read Explanation
View all explanations

What do you think about this solution?

We value your feedback to improve our textbook solutions.

Study anywhere. Anytime. Across all devices.