/*! 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 3 When a chemical loses a hydrogen... [FREE SOLUTION] | 91影视

91影视

Log out

Learning Materials

Features

Discover

Chapter 10: Problem 3

When a chemical loses a hydrogen ion, is it behaving as an acid or a base?

Short Answer

Expert verified
It is behaving as an acid.

Step by step solution

01

Understanding Acids and Bases

Start by understanding the definitions of acids and bases according to the Br酶nsted-Lowry theory. An acid is a substance that can donate a proton (hydrogen ion, H^+), while a base is a substance that can accept a proton.
02

Analyzing the Given Chemical Behavior

In the problem, the chemical is losing a hydrogen ion. According to the Br酶nsted-Lowry theory, when a substance donates a proton, it is considered an acid.
03

Conclusion Based on Analysis

Since the chemical is losing, or donating, a hydrogen ion, it is behaving as an acid according to the Br酶nsted-Lowry theory.

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.

Acid
In chemistry, an acid is a fascinating substance defined by its ability to donate protons (hydrogen ions, \(H^+\)). This action is central to the Br酶nsted-Lowry acid-base theory. When an acid donates a proton, it transforms into what's known as its conjugate base. This dynamic interplay is akin to a handoff in a relay race, where the acid energetically passes on its hydrogen ion. Some common everyday acids include lemon juice, vinegar, and even gastric acid in your stomach. These substances can be identified by their characteristic sour taste and ability to react with bases.
Base
A base, according to the Br酶nsted-Lowry theory, is a substance that can accept a proton. Essentially, bases are the "receivers" in chemical reactions with acids. When a base captures a hydrogen ion (\(H^+\)), it forms its conjugate acid counterpart. This acceptance process can be understood as a welcoming gesture, where the base eagerly integrates the proton. Examples of bases include baking soda and soap, both commonly used in everyday life. Bases feel slippery to the touch due to their ability to react with oils and fats, making them effective cleaning agents.
Proton Donation
Proton donation is the hallmark characteristic of an acid in the Br酶nsted-Lowry theory. During a chemical reaction, an acid donates its hydrogen ion to another molecule or ion, which is typically a base. This exchange is not only a transfer of a positively charged particle but also of potential energy and the ability to influence chemical properties. Through this donation, acids not only reveal their acidic nature but also facilitate a variety of important chemical processes, like nutrient absorption, cellular metabolism, and even corrosion in materials science.
Hydrogen Ion (H^+)
The hydrogen ion, often abbreviated as \(H^+\), plays a pivotal role in chemistry as the simplest and most fundamental ion. It is essentially a proton, devoid of any electrons, which gives it a positive charge. This seemingly simple ion profoundly influences chemical reactions and can alter pH levels, determining whether a solution is acidic, neutral, or basic. In aqueous solutions, \(H^+\) ions often combine with water molecules to form hydronium ions \(H_3O^+\), further demonstrating their reactive nature. Understanding \(H^+\) is essential for grasping many key concepts in both biological and chemical systems.

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

What does sulfur dioxide have to do with acid rain?

When the hydronium ion concentration of a solution is \(1 \times 10^{-10}\) mole per liter, what is the \(\mathrm{pH}\) of the solution? Is the solution acidic or basic?

What is the hydroxide ion concentration in an aqueous solution when the hydronium ion concentration is \(1 \times 10^{-10}\) mole per liter?

When the hydronium ion concentration of a solution equals 1 mole per liter, what is the \(\mathrm{pH}\) of the solution? Is the solution acidic or basic?

Which is the stronger acid: \(\mathrm{H}-\mathrm{F}\) or \(\mathrm{H}-\mathrm{I}\) ?
See all solutions

Recommended explanations on Chemistry Textbooks

Inorganic Chemistry

Read Explanation

Nuclear Chemistry

Read Explanation

Organic Chemistry

Read Explanation

Making Measurements

Read Explanation

Chemical Reactions

Read Explanation

Ionic and Molecular Compounds

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.