/*! 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 48 Explain the formation of hydroni... [FREE SOLUTION] | 91影视

91影视

Log out

Learning Materials

Features

Discover

Chapter 6: Problem 48

Explain the formation of hydronium ion and ammonium ion.

Short Answer

Expert verified
Question: Explain the formation of hydronium and ammonium ions in an aqueous solution. Answer: Hydronium ions (H3O+) are formed when acids dissolve in water and donate a proton (H+) to water molecules. For example, hydrochloric acid (HCl) dissociates into an anion (Cl-) and a free H+ ion, which forms a hydronium ion with water. On the other hand, ammonium ions (NH4+) are formed when ammonia (NH3) dissolves in water and accepts a proton from water molecules, creating ammonium ions and hydroxide ions (OH-). These ions are crucial in understanding the acidic and basic properties of water-soluble compounds.

Step by step solution

01

Understand the context and importance of hydronium and ammonium ions

Hydronium ions and ammonium ions are formed when acids and bases react in an aqueous solution. These ions are essential in understanding the concept of acidity and alkalinity in chemistry, and they contribute to the essential properties of water-soluble acids and bases.
02

Discuss the formation of hydronium ion

When an acid is dissolved in water, it donates a proton (H+) to water molecules. The acid dissociates to form an anion and a free H+ ion. The water molecules attract the free H+ protons, forming hydronium ions (H3O+). The reaction can be represented as follows: Acid + H2O -> Anion + H3O+ For example, in the case of hydrochloric acid (HCl): HCl + H2O -> Cl- + H3O+ The formation of hydronium ions is responsible for the acidic properties of an aqueous solution.
03

Discuss the formation of ammonium ion

When ammonia (NH3) is dissolved in water, it acts as a base by accepting the proton (H+) from water molecules. This proton transfer causes the formation of ammonium ions (NH4+) in the solution. The reaction can be represented as follows: NH3 + H2O -> NH4+ + OH- Here, ammonia accepts a proton (H+) from water, leading to the formation of ammonium ions and hydroxide ions (OH-). The presence of hydroxide ions is responsible for the basic properties of the aqueous solution.
04

Summarize the formation of hydronium and ammonium ions

In summary, the formation of hydronium and ammonium ions occurs through the reaction of acids and bases in aqueous solutions. Hydronium ions (H3O+) are formed when acids donate a proton to water, while ammonium ions (NH4+) are formed when ammonia (NH3) accepts a proton from water. These ions play a crucial role in understanding the acidic and basic properties of water-soluble compounds.

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.

Acids and Bases
Acids and bases are chemical substances that play key roles in many chemical reactions. When considering them in the context of the hydronium and ammonium ion formation, both act in distinct, yet related ways.

  • An acid typically donates protons (H+) to other substances. This proton donation is the defining characteristic that makes a substance an acid.
  • A base, on the other hand, accepts protons. This acceptance of protons is what defines a substance as a base.
In reactions, acids and bases work together to either donate or accept protons, resulting in the formation of new ions like hydronium (H3O+) and ammonium (NH4+). Understanding these definitions is crucial for grasping how these processes occur in aqueous solutions.
Aqueous Solutions
Aqueous solutions, where water is the solvent, provide the medium in which acids and bases react. Water, being polar, has a unique ability to dissolve and dissociate substances into ions.

  • In these solutions, acids dissociate to release their protons into the water, forming hydronium ions.
  • Similarly, bases react with water by accepting protons, which can lead to the formation of ions like ammonium.
The fact that water is involved in these reactions highlights its critical role as a solvent and participant, allowing the characteristic behaviors of acids and bases to be observed and measured.
Proton Transfer
Proton transfer is the movement of protons from one molecule to another, which is a fundamental concept in chemistry.

  • In the case of hydronium ion formation, the proton transfer occurs when an acid donates a proton to a water molecule, enhancing the solution's acidity by creating hydronium ions (H3O+).
  • Conversely, when ammonia acts as a base, it accepts a proton from a water molecule, leading to the formation of ammonium ions (NH4+) and making the solution basic.
Proton transfer is the essence of acid-base reactions and illustrates the dynamic exchanges that impact the solution's chemical properties.
Acidity and Alkalinity
Acidity and alkalinity refer to the concentration of hydronium ions (H3O+) and hydroxide ions (OH-) in a solution.

  • Solutions with high concentrations of hydronium ions are acidic, showing properties such as sour taste and reactivity with metals.
  • Solutions with high concentrations of hydroxide ions are alkaline, having characteristics such as a bitter taste and slipperiness.
The formation of hydronium and ammonium ions directly influences these properties. The balance of proton donors (acids) and acceptors (bases) in a solution determines its position on the pH scale, representing acidity and alkalinity levels. This balance is key to understanding various chemical phenomena and reactions in aqueous 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

Define indicator. Why are different indicators used in different \(\mathrm{pH}\) ranges?

Define oxyacid. Give two examples.

What are the \(\mathrm{pH}\) values of the following solutions at \(25^{\circ} \mathrm{C}\) ? (i) \(0.001 \mathrm{M}\) of \(\mathrm{HCl}\) (ii) \(0.05 \mathrm{M}\) of \(\mathrm{H}_{2} \mathrm{SO}_{4}\) (iii) \(0.01 \mathrm{M}\) of \(\mathrm{NaOH}\)

The formula of the basic salt formed by treating calcium hydroxide with \(\mathrm{HCl}\) is

Give one example of acid-base reaction without formation of water.
See all solutions

Recommended explanations on Chemistry Textbooks

Organic Chemistry

Read Explanation

The Earths Atmosphere

Read Explanation

Physical Chemistry

Read Explanation

Kinetics

Read Explanation

Inorganic Chemistry

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.