/*! 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 114 Arrange the following 0.10\(M\) ... [FREE SOLUTION] | 91影视

91影视

Log out

Learning Materials

Features

Discover

Chapter 14: Problem 114

Arrange the following 0.10\(M\) solutions in order from most acidic to most basic. See Appendix 5 for \(K_{\mathrm{a}}\) and \(K_{\mathrm{b}}\) values. $$ \mathrm{CaBr}_{2}, \mathrm{KNO}_{2}, \mathrm{HClO}_{4}, \quad \mathrm{HNO}_{2}, \quad \mathrm{HONH}_{3} \mathrm{ClO}_{4} $$

Short Answer

Expert verified
The given solutions can be arranged in order from most acidic to most basic as follows: HClO4 > HNO2 > HONH3ClO4 > KNO2.

Step by step solution

01

Identify acidic and basic solutions

CaBr2 is a salt, but it is formed from the reaction of a strong base (Ca(OH)2) and a strong acid (HBr), so the solution will be neutral. KNO2 is a salt formed from the reaction of a strong base (KOH) and a weak acid (HNO2), making the solution basic. HClO4 is a strong acid, making the solution acidic. HNO2 is a weak acid, making the solution acidic. HONH3ClO4 is the salt formed from the reaction of a weak base (HONH2) and a strong acid (HClO4), making the solution acidic.
02

Find Ka and Kb values

From Appendix 5, we get the \(K_{\mathrm{a}}\) and \(K_{\mathrm{b}}\) values for the relevant acidic/basic substances: \(K_{\mathrm{a}}\) (HClO4) = \(1 \times 10^{10}\), strong acid \(K_{\mathrm{a}}\) (HNO2) = \(4.5 \times 10^{-4}\), weak acid \(K_{\mathrm{b}}\) (KNO2) = \(1.61 \times 10^{-11}\), weak base \(K_{\mathrm{a}}\) (HONH2) = \(1.1 \times 10^{-11}\), very weak base. (Note: We don't need to consider CaBr2 since it's neutral.)
03

Arrange solutions in order of acidity

Based on the \(K_{\mathrm{a}}\) and \(K_{\mathrm{b}}\) values, we can arrange the solutions in order from most acidic to most basic: 1. HClO4 (strong acid, \(K_{\mathrm{a}} = 1 \times 10^{10}\)) 2. HNO2 (weak acid, \(K_{\mathrm{a}} = 4.5 \times 10^{-4}\)) 3. HONH3ClO4 (very weak base, \(K_{\mathrm{a}} = 1.1 \times 10^{-11}\)) (Note: Due to the presence of strong acid HClO4, the overall solution will be acidic.) 4. KNO2 (weak base, \(K_{\mathrm{b}} = 1.61 \times 10^{-11}\)) The solution for the given exercise can be represented as follows: HClO4 > HNO2 > HONH3ClO4 > KNO2

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.

strong acid
A strong acid is a substance that completely dissociates in water, releasing a high concentration of hydrogen ions (\(H^+\)). This results in a very low pH, typically below 3. The degree to which an acid dissociates is represented by its acid dissociation constant (\(K_a\)).

- **Example:** - Perchloric acid (\(HClO_4\)), with a \(K_a\) of \(1 \times 10^{10}\), fully dissociates and has a strong acidic solution.- Strong acids often have large \(K_a\) values, indicating fully ionized forms.

The presence of strong acids significantly lowers the pH of a solution, making it highly acidic. Examples include hydrochloric acid (\(HCl\)), sulfuric acid (\(H_2SO_4\)), and our current focus, perchloric acid (\(HClO_4\)). Understanding strong acids is crucial because they are common in both industrial and laboratory settings.
weak acid
Weak acids only partially dissociate in water, meaning they do not release all their hydrogen ions into the solution. This partial dissociation results in a higher pH compared to strong acids, typically ranging from 3 to 6.

- **Example:** - Nitrous acid (\(HNO_2\)), with a \(K_a\) of \(4.5 \times 10^{-4}\), indicates a low level of ionization.- \(K_a\) values for weak acids are lower than those of strong acids, signifying less hydrogen ion release.

Due to their higher pH and weaker acid strength, weak acids are often used as buffers in solutions to maintain pH stability. They are crucial for many biological and chemical systems.
neutral salt
Neutral salts are formed from the reaction of a strong acid and a strong base, resulting in a product that doesn't affect the pH of a solution. The ions from these salts do not hydrolyze with water, leading to a neutral pH of around 7.

- **Example:** - Calcium bromide (\(CaBr_2\)) is a neutral salt formed from calcium hydroxide (\(Ca(OH)_2\)) and hydrobromic acid (\(HBr\)).- The neutrality of these salts makes them ideal for applications where solution pH needs to remain unaffected.

Understanding the role of neutral salts is essential when preparing solutions that require stable pH levels. This stability is significant in processes such as chemical synthesis and biological environments.

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

Saccharin, a sugar substitute, has the formula \(\mathrm{HC}_{7} \mathrm{H}_{4} \mathrm{NSO}_{3}\) and is a weak acid with \(K_{\mathrm{a}}=2.0 \times 10^{-12} .\) If 100.0 \(\mathrm{g}\) of saccharin is dissolved in enough water to make 340 \(\mathrm{mL}\) of solution, calculate the \(\mathrm{pH}\) of the resulting solution.

An antacid purchased at a local drug store has a pOH of \(2.3 .\) Calculate the \(\mathrm{pH},\left[\mathrm{H}^{+}\right],\) and \(\left[\mathrm{OH}^{-}\right]\) of this solution. Is the antacid acidic or basic?

For the following, mix equal volumes of one solution from Group I with one solution from Group II to achieve the indicated pH. Calculate the pH of each solution. $$\begin{aligned} \text { Group I: } & 0.20 M \mathrm{NH}_{4} \mathrm{Cl}, 0.20 \mathrm{MCl}, 0.20 M \mathrm{C}_{6} \mathrm{H}_{5} \mathrm{NH}_{3} \mathrm{Cl} \\ & 0.20 M\left(\mathrm{C}_{2} \mathrm{H}_{5}\right)_{3} \mathrm{NHCl} \end{aligned}$$ $$\begin{aligned} \text { Group II: } 0.20 \quad M\quad \mathrm{KOI}, 0.20 \quad\mathrm{M} \quad\mathrm{NaCN}, 0.20\quad \mathrm{M}\quad \mathrm{KOCl}, 0.20 \\ \mathrm{M}\quad \mathrm{NaNO}_{2} \end{aligned}$$ a. the solution with the lowest pH b. the solution with the highest pH c. the solution with the pH closest to 7.00

Making use of the assumptions we ordinarily make in calculating the \(\mathrm{pH}\) of an aqueous solution of a weak acid, calculate the pH of a \(1.0 \times 10^{-6}-\mathrm{M}\) solution of hypobromous acid \(\left(\mathrm{HBrO}, K_{\mathrm{a}}=2 \times 10^{-9}\right) .\) What is wrong with your answer? Why is it wrong? Without trying to solve the problem, explain what has to be included to solve the problem correctly.

Calculate the concentrations of all species present in a \(0.25-M\) solution of ethylammonium chloride \(\left(\mathrm{C}_{2} \mathrm{H}_{5} \mathrm{NH}_{3} \mathrm{Cl}\right)\)
See all solutions

Recommended explanations on Chemistry Textbooks

Kinetics

Read Explanation

Chemical Analysis

Read Explanation

Organic Chemistry

Read Explanation

Physical Chemistry

Read Explanation

The Earths Atmosphere

Read Explanation

Chemical Reactions

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.