Bronsted-Lowry Reactions & Examples - Video & Lesson Transcript

Home » What Is A Bronsted Lowry Base » Bronsted-Lowry Reactions & Examples - Video & Lesson Transcript

Maybe your like

Study.com Log In Sign Up Menu
  • Plans
  • Courses
    • By Subject
    • Arts
    • Business
    • Computer Science
    • Education & Teaching
    • English (ELA)
    • Foreign Language
    • Health & Medicine
    • History
    • Humanities
    • Math
    • Psychology
    • Science
    • Social Science
  • Subjects
    • Art
    • Architecture
    • Art History
    • Design
    • Performing Arts
    • Visual Arts
    • Business
    • Accounting
    • Business Administration
    • Business Communication
    • Business Ethics
    • Business Intelligence
    • Business Law
    • Economics
    • Finance
    • Healthcare Administration
    • Human Resources
    • Information Technology
    • International Business
    • Operations Management
    • Real Estate
    • Sales & Marketing
    • Computer Science
    • Computer Engineering
    • Computer Programming
    • Cybersecurity
    • Data Science
    • Software
    • Education & Teaching
    • Education Law & Policy
    • Pedagogy & Teaching Strategies
    • Special & Specialized Education
    • Student Support in Education
    • Teaching English Language Learners
    • English
    • Grammar
    • Literature
    • Public Speaking
    • Reading
    • Vocabulary
    • Writing & Composition
    • Health & Medicine
    • Counseling & Therapy
    • Health
    • Medicine
    • Nursing
    • Nutrition
    • History
    • US History
    • World History
    • Humanities
    • Communication
    • Ethics
    • Foreign Languages
    • Philosophy
    • Religious Studies
    • Math
    • Algebra
    • Basic Math
    • Calculus
    • Geometry
    • Statistics
    • Trigonometry
    • Psychology
    • Clinical & Abnormal Psychology
    • Cognitive Science
    • Developmental Psychology
    • Educational Psychology
    • Organizational Psychology
    • Social Psychology
    • Science
    • Anatomy & Physiology
    • Astronomy
    • Biology
    • Chemistry
    • Earth Science
    • Engineering
    • Environmental Science
    • Physics
    • Scientific Research
    • Social Science
    • Anthropology
    • Criminal Justice
    • Geography
    • Law
    • Linguistics
    • Political Science
    • Sociology
  • Teachers
  • Certifications
    • Teacher Certification Exams
    • Praxis Test Prep
    • FTCE Test Prep
    • TExES Test Prep
    • CSET & CBEST Test Prep
    • All Teacher Certification Test Prep
    • Nursing Exams
    • NCLEX Test Prep
    • TEAS Test Prep
    • HESI Test Prep
    • All Nursing Test Prep
    • Real Estate Exams
    • Real Estate Sales
    • Real Estate Brokers
    • Real Estate Appraisals
    • All Real Estate Test Prep
    • Military Exams
    • ASVAB Test Prep
    • AFOQT Test Prep
    • All Military Test Prep
    • Finance Exams
    • SIE Test Prep
    • Series 6 Test Prep
    • Series 65 Test Prep
    • Series 66 Test Prep
    • Series 7 Test Prep
    • CPP Test Prep
    • CMA Test Prep
    • All Finance Test Prep
    • Human Resources Exams
    • SHRM Test Prep
    • PHR Test Prep
    • aPHR Test Prep
    • PHRi Test Prep
    • SPHR Test Prep
    • All HR Test Prep
    • Counseling & Social Work Exams
    • NCE Test Prep
    • NCMHCE Test Prep
    • CPCE Test Prep
    • ASWB Test Prep
    • CRC Test Prep
    • All Counseling & Social Work Test Prep
    • Allied Health & Medicine Exams
    • ASCP Test Prep
    • CNA Test Prep
    • CNS Test Prep
    • All Medical Test Prep
    • TOEFL Exam
    • TOEFL 2026 Test Prep
    • TOEFL 2025 Test Prep
  • College Degrees
  • Sign Up
  • Lesson
  • Transcript
Joanna Tatomir, Nissa Garcia
  • Author Joanna Tatomir

    Joanna holds a PhD in Biology from the University of Michigan and is currently working towards a degree in Veterinary Medicine at Michigan State University. She has taught a combination of ESL and STEM courses to secondary and university students.

    View bio
  • Instructor Nissa Garcia

    Nissa has a masters degree in chemistry and has taught high school science and college level chemistry.

    View bio
See the Bronsted-Lowry base definition. Learn about identifying bronsted lowry acids and bases and explore Bronsted-Lowry reactions.

Table of Contents

  • Bronsted-Lowry Base
  • Bronsted-Lowry Acid and Base Reaction
  • Identifying Bronsted-Lowry Acids and Bases
  • Bronsted-Lowry Base Examples
  • Bronsted-Lowry Reactions
  • Lesson Summary
Show Frequently Asked Questions

How do you identify Bronsted-Lowry acids and bases?

Bronsted-Lowry acids and bases can be identified based on their ability to donate or accept protons. Bronsted-Lowry acids donate protons, while Bronsted-Lowry bases accept protons.

What is an example of a Bronsted-Lowry base that is not considered an Arrhenius base?

Bronsted-Lowry bases are not defined by the ability to accept hydrogen ions in an aqueous solution. Some examples of Bronsted-Lowry bases that are not considered Arrhenius bases include Cl-, Br-, S2-, and F-.

Is HCl a Bronsted-Lowry base?

HCl is not considered a Bronsted-Lowry base because it cannot accept a hydrogen ion. Instead, it is considered a Bronsted-Lowry acid, as it donates a proton.

What are some examples of a Bronsted-Lowry base?

There are numerous examples of Bronsted-Lowry bases. A strong base is O2-. Weak bases include OH-, NH3, and H2O. Chloride and bromide ions represent extremely weak bases.

What is the difference between Bronsted-Lowry acids and bases?

A Bronsted-Lowry acid refers to any substance able to donate a hydrogen ion. A Bronsted-Lowry base refers to a substance capable of accepting a hydrogen ion.

Create an account

Table of Contents

  • Bronsted-Lowry Base
  • Bronsted-Lowry Acid and Base Reaction
  • Identifying Bronsted-Lowry Acids and Bases
  • Bronsted-Lowry Base Examples
  • Bronsted-Lowry Reactions
  • Lesson Summary
Show

Bronsted-Lowry Base

Chemical compounds are characterized by a number of different properties, such as molecular mass, polarity, and the shape of the molecule. Another important property associated with chemicals is the acidity or basicity of the substance. When measured on the pH scale, acids and bases reflect the ability for a compound to accept or donate hydrogen ions. There are three primary methods for classifying acids and bases:

  • The Arrhenius theory of acids and bases
  • The Lewis model of acids and bases
  • The Bronsted-Lowry definition of acids and bases

Arrhenius, a Swedish chemist, defined an acid by the ability of a compound to produce hydrogen ions ({eq}H^+ {/eq}) when dissolved in water. By contrast, Arrhenius classified compounds that released hydroxide ions in water as bases. This method was considered simplistic as it was unable to explain how ions aside from hydrogen were able to produce basic conditions when dissolved in water.

The Lewis model of acids looks at compounds in terms of their ability to serve as electron acceptors and donors. In this model, compounds able to accept electrons are referred to as acids, while compounds serving as electron donors represent bases. This model moved beyond the Arrhenius theory by eliminating the need to define acids and bases by hydrogen ions alone.

The Bronsted-Lowry definition once again returned to the movement of hydrogen ions between compounds. Under these conventions, a Bronsted-Lowry acid is defined as a proton ({eq}H^+ {/eq}) donor, while the Bronsted-Lowry base is defined as a proton acceptor. Unlike the Arrhenius model, however, the Bronsted-Lowry model allows for the creation of hydrogen ions by other molecules, such as sodium ({eq}Na^+ {/eq}), chlorine ({eq}Cl^- {/eq}), and fluorine ({eq}F^- {/eq}).

Under this classification system, both acids and bases can be characterized as either a compound, like {eq}HCl {/eq} or {eq}H_2O {/eq}; an organic molecule, such as {eq}CH_3COOH {/eq} or {eq}NH_3 {/eq}; or ionic in nature, as with salts like {eq}Na^+F^- {/eq} or bases like {eq}OH^- {/eq}.

Observing the number of hydrogen ions present both before and after a reaction represents the sole means for determining whether a substance represents a Bronsted-Lowry acid or base. When the number of hydrogens decreases as a substance moves from a reactant to its associated product, then this compound would be classified as a Bronsted-Lowry acid. By contrast, when the number of hydrogen ions increases from the reactant to the corresponding product, then the compound reflects the Bronsted-Lowry base definition.

Therefore, Bronsted-Lowry acids release protons ({eq}H^+ {/eq}), while Bronsted-Lowry bases are able to accept lone pairs of electrons.

Conjugate Acid and Conjugate Base

Looking at the number of hydrogen ions present before and after a reaction serves as the primary method for determining an acid or base in the Bronsted-Lowry system. When looking at the Bronsted-Lowry acid on the left side of a chemical equation, the loss of protons as this substance is used in a reaction results in the production of a conjugate base on the right side of the equation. Similarly, by observing a Bronsted-Lowry base on the left side of the equation, the addition of protons to this substance on the right side reflects the production of a conjugate acid. Each Bronsted-Lowry acid and base consists of a complimentary conjugate base and conjugate acid.

To unlock this lesson you must be a Study.com Member. Create your account

An error occurred trying to load this video.

Try refreshing the page, or contact customer support.

You must cCreate an account to continue watching

Register to view this lesson

Are you a student or a teacher? I am a student I am a teacher

Create Your Account To Continue Watching

As a member, you'll also get unlimited access to over 88,000 lessons in math, English, science, history, and more. Plus, get practice tests, quizzes, and personalized coaching to help you succeed.

Get unlimited access to over 88,000 lessons.

Try it now Try it now.
Already registered? Log in here for access
Back

Resources created by teachers for teachers

Over 30,000 video lessons & teaching resources‐all in one place. Video lessons Quizzes & Worksheets Classroom Integration Lesson Plans

I would definitely recommend Study.com to my colleagues. It’s like a teacher waved a magic wand and did the work for me. I feel like it’s a lifeline.

Jennifer B. Teacher Jennifer B. Try it now Back

Just checking in. Are you still watching?

Yes! Keep playing. Your next lesson will play in 10 seconds
  • 0:00 What Is A Bronsted-Lowry Base?
  • 2:10 Examples Of…
  • 5:05 Lesson Summary
View Video Only Save Timeline 79K views 79K views

Bronsted-Lowry Acid and Base Reaction

A general chemical equation can be used to represent the reaction between a Bronsted-Lowry acid and base using the following abbreviations:

  • Bronsted-Lowry acid: {eq}HA {/eq}
  • Bronsted-Lowry base: {eq}Z {/eq}
  • Conjugate base: {eq}A^- {/eq}
  • Conjugate acid: {eq}HZ^+ {/eq}

Using these abbreviations, the general chemical equation of a Bronsted-Lowry acid-base reaction is:

{eq}HA + Z = A^- + HZ^+ {/eq}

Reaction Example

For example, looking at the reaction between ammonia and {eq}HCl {/eq} (hydrogen chloride), the corresponding Bronsted-Lowry equation is:

{eq}HCl + NH_3 \rightarrow NH_4^+ + Cl^- {/eq}

In this example, the Bronsted-Lowry acid is {eq}HCl {/eq}, the Bronsted-Lowry base is {eq}NH_3 {/eq}, the conjugate base is {eq}Cl^- {/eq}, and the conjugate acid is {eq}NH_4^+ {/eq}.

To unlock this lesson you must be a Study.com Member. Create your account

Identifying Bronsted-Lowry Acids and Bases

The following examples provide additional practice for identifying Bronsted-Lowry acids and bases and their associated conjugate acids and bases:

Water and Ammonia

The reaction between water and ammonia is represented by the following equation.

{eq}H_2O + NH_3 \rightarrow OH^- + NH_4^+ {/eq}

  • Acid: {eq}H_2O {/eq}
  • Base: {eq}NH_3 {/eq}
  • Conjugate base: {eq}OH^- {/eq}
  • Conjugate acid: {eq}NH_4^+ {/eq}

The reaction between water and ammonia.

bronsted lowry acid and base

Fluoride Ion and Water

The following equation provides a Bronsted-Lowry acid example and a Bronsted-Lowry base example.

{eq}F^- + H_2O \rightarrow HF + OH^- {/eq}

  • Acid: {eq}H_2O {/eq}
  • Base: {eq}F^- {/eq}
  • Conjugate base: {eq}OH^- {/eq}
  • Conjugate acid: {eq}HF {/eq}

Acetic Acid and Water

Below is the equation for the reaction between acetic acid and water.

{eq}CH_3COOH + H_2O \rightarrow CH_3COO^- + H_3O^- {/eq}

  • Acid: {eq}CH_3COOH {/eq}
  • Base: {eq}H_2O {/eq}
  • Conjugate base: {eq}CH_3COO^- {/eq}
  • Conjugate acid: {eq}H_3O^- {/eq}

The reaction between acetic acid and water.

bronsted lowry acid and base

Aniline and Water

The reaction between aniline and water is expressed by equation below.

{eq}C_6H_5NH_2 + H_2O \rightarrow C_6H_5NH_3^+ + OH^- {/eq}

  • Acid: {eq}H_2O {/eq}
  • Base: {eq}C_6H_5NH_2 {/eq}
  • Conjugate base: {eq}OH^- {/eq}
  • Conjugate acid: {eq}C_6H_5NH_3 {/eq}

To unlock this lesson you must be a Study.com Member. Create your account

Bronsted-Lowry Base Examples

The following Bronsted-Lowry bases list is arranged in order of decreasing base strength. The associated conjugate acid is also provided in parentheses.

  • {eq}O_2^- (OH^-) {/eq}
  • {eq}S^{2-} (HS^-) {/eq}
  • {eq}OH^- (H_2O) {/eq}
  • {eq}PO_4^{3-} (HPO_4^{2-}) {/eq}
  • {eq}CO_3^{2-} (HCO_3^-) {/eq}
  • {eq}NH_3 (NH_4^+) {/eq}
  • {eq}CN^- (HCN) {/eq}
  • {eq}HPO_4^{2-} (H_2PO_4^-) {/eq}
  • {eq}SO_3^{2-} (HSO_3^-) {/eq}
  • {eq}HS^- (H_2S) {/eq}
  • {eq}F^- (HF) {/eq}
  • {eq}H_2O (H_3O^+) {/eq}
  • {eq}NO_3^- (HNO_3) {/eq}
  • {eq}Cl^- (HCl) {/eq}
  • {eq}Br^- (HBr) {/eq}

When looking at the reaction between trimethylamine and water:

{eq}(CH_3)_3N + H_2O \rightarrow (CH_3)_3NH^+ + OH^- {/eq}

The Bronsted-Lowry base is {eq}(CH_3)_3N {/eq}, the Bronsted-Lowry acid is {eq}H_2O {/eq}, the conjugate acid is {eq}(CH_3)_3NH^+ {/eq}, and the conjugate base is {eq}OH^- {/eq}.

To unlock this lesson you must be a Study.com Member. Create your account

Bronsted-Lowry Reactions

As described above, the main difference between the Bronsted-Lowry and Arrhenius models is that: the Bronsted-Lowry definition does not require hydrogen ions to dissociate in water; and the reaction does not have to occur in an aqueous (or water-based) medium.

For example, the reaction of acetic acid with an aqueous solution, in this case water, produces the following equation: {eq}CH_3COOH + H_2O \rightarrow CH_3COO^- + H_3O^- {/eq}. The reaction of acetic acid with a non-aqueous solution, for example ammonia, results in: {eq}CH_3COOH + NH_3 \rightarrow CH_3COONH_4 {/eq}. Both equations represent examples of Bronsted-Lowry reactions.

Bronsted-Lowry acid-base theory also differs from the Lux-Flood acid-base model due to the use of different acceptor and donor molecules. In the Bronsted-Lowry model, hydrogen ions are accepted and donated between bases and acids, while in the Lux-Flood model, oxide ions ({eq}O_2^- {/eq}) are exchanged between bases and acids.

Amphoteric Substance

An amphoteric substance refers to any compound able to act as both an acid and a base. Water ({eq}H_2O {/eq}) represents one substance that can behave as a Bronsted-Lowry acid and base. Water can therefore be considered an amphoteric substance. As seen in some of the examples shown earlier in the lesson, water can act as a Bronsted-Lowry acid:

  • {eq}H_2O + NH_3 \rightarrow OH^- + NH_4^+ {/eq}
    • Acid: {eq}H_2O {/eq}
    • Base: {eq}NH_3 {/eq}
    • Conjugate base: {eq}OH^- {/eq}
    • Conjugate acid: {eq}NH_4^+ {/eq}

Water can also act as a Bronsted-Lowry base:

  • {eq}CH_3COOH + H_2O \rightarrow CH_3COO^- + H_3O^- {/eq}
    • Acid: {eq}CH_3COOH {/eq}
    • Base: {eq}H_2O {/eq}
    • Conjugate base: {eq}CH_3COO^- {/eq}
    • Conjugate acid: {eq}H_3O^- {/eq}

To unlock this lesson you must be a Study.com Member. Create your account

Lesson Summary

A Bronsted-Lowry acid refers to any substance able to donate a proton ({eq}H^+ {/eq}), while a Bronsted-Lowry base is any substance able to accept a hydrogen ion. Each Bronsted-Lowry acid and base possesses a complimentary conjugate base and conjugate acid. Identifying the acid-conjugate base and base-conjugate acid pairs in an equation can be determined by looking at the change in hydrogen ions between the reactants and the products. An acid will lose protons to form its conjugate base. Conversely, a base will gain protons to form its conjugate acid. Using these conventions:

  • Bronsted-Lowry acid: {eq}HA {/eq}
  • Bronsted-Lowry base: {eq}Z {/eq}
  • Conjugate base: {eq}A^- {/eq}
  • Conjugate acid: {eq}HZ^+ {/eq}

The general equation for a Bronsted-Lowry reaction is: {eq}HA + Z = A^- + HZ^+ {/eq}.

The Bronsted-Lowry model differs from the Arrhenius model in that it does not rely upon the dissociation of protons in an aqueous solution in order define an acid and a base. Moreover, while the Bronsted-Lowry model relies upon the exchange of hydrogen ions between acids and bases, the Lux-Flood model instead uses oxide ions to define acids and bases. In the Bronsted-Lowry system, any substance able to act as both an acid and a base is referred to as an amphoteric substance. Water represents an excellent example of an amphoteric substance.

To unlock this lesson you must be a Study.com Member. Create your account

Video Transcript

What Is a Bronsted-Lowry Base?

Back in 1923, two scientists, Johannes Nicolaus Bronsted and Thomas Martin Lowry published a theory on the behavior of acidic and basic solutions. Bronsted came from Denmark, and Lowry came from England. It was a great coincidence that they published the same theory independently but at the same time. That is why this theory, the Bronsted-Lowry definition of acids and bases, was named after the two of them.

For this lesson, we will be focusing on basic solutions and how they behave, according to Bronsted and Lowry. We refer to these solutions as Bronsted-Lowry bases. A Bronsted-Lowry base is a solution that behaves as a proton acceptor, and these protons are in the form of a hydrogen (H+) ion. The solution that behaves as a proton donor is called a Bronsted-Lowry acid. In general, this is the interaction between Bronsted-Lowry acids and bases:

A Bronsted-Lowry Base is a Proton Acceptor

We can see that when the Bronsted-Lowry 'accepts' the hydrogen (H+) ion coming from the acid, the hydrogen (H+) ion attaches itself to the Bronsted-Lowry base. The proton (H+ ion) has a charge of positive one, so when the base (B) accepts the proton, its charge increases by positive one (HB+). Since the acid (HA) lost or donated a proton, its charge decreases by one, and in this case, it results in a negative charge (A-). The arrow going forward and backward at the same time is an equilibrium sign, which tells us that the reaction can either go forward or backward.

Let's take a close look again at the Bronsted-Lowry acid-base reaction. We can see that when an acid donates a proton, the resulting product is a conjugate base. When the base accepts a proton, the resulting product that is formed is a conjugate acid. When we think of the meaning of the word 'conjugate', it means 'joined together' or 'coupled'. In the same way, an acid/base and its resulting conjugate base/acid are what we call conjugate acid-base pairs.

Conjugate Acid-Base Pairs

Examples of Bronsted-Lowry Reactions

What is the telltale sign that a substance is a Bronsted-Lowry base in chemical reactions? To find the answer, we look at which substance gains a hydrogen atom - the substance that gains a hydrogen atom is our Bronsted-Lowry base since it accepts protons in the form of hydrogen (H+) ions.

Here, let's take a look at some examples of Bronsted-Lowry acid-base interactions. We will practice identifying conjugate acid-base pairs and identifying which substances are Bronsted bases.

  • Example 1: Reaction between water and ammonia
Water and Ammonia Acid-Base Reaction

We can first identify the substances. Let's take a look at the following illustration below. Ammonia is the Bronsted-Lowry base because it is the 'proton acceptor' - it accepts a hydrogen atom from water. On the other hand, water is the Bronsted-Lowry acid because it is the 'proton donor'. The conjugate acid is the ammonium ion (NH sub 4+) because it is the substance produced after the proton, hydrogen, is accepted. The conjugate base is the hydroxide ion (OH-) because this is the substance produced when H2O donated the proton. The conjugate acid-base pairs are: H sub 2O/OH- and NH sub 3/NH sub 4+.

Water and Ammonia Acid-Base Reaction
  • Example 2: Sulfuric acid and water
Sulfuric Acid and Water Acid-Base Reaction

We can first identify the substances. Water is the Bronsted-Lowry base because it is the 'proton acceptor' - it accepted a hydrogen atom from sulfuric acid (H sub 2 SO sub 4). Meanwhile, we identify sulfuric acid as the Bronsted-Lowry acid because it donated a proton to water. The conjugate acid is the hydronium ion (H sub 3 O+) because it is the substance produced after water accepted a hydrogen proton. The conjugate base is bisulfate (HSO sub 4-) because this is the substance produced when sulfuric acid donated or lost a proton. The conjugate acid-base pairs are: H sub2 SO sub 4/HSO sub 4- and H sub 2 O/H sub 3 O+.

Sulfuric Acid and Water Acid-Base Reaction
  • Example 3: Bicarbonate and water
Bicarbonate and Water Acid-Base Reaction

In this reaction, the bicarbonate ion reacts with water. The proton transfer is shown in the illustration below. Here, the bicarbonate ion accepts one hydrogen atom (proton) from water, making it is the Bronsted-Lowry base, and produces the conjugate acid carbonic acid (H sub 2 CO sub 3). Water acts as the acid because it donates a hydrogen atom (proton) to bicarbonate ion. When water loses a proton, it produces the conjugate base, which is the hydroxide (OH-) ion. The conjugate acid-base pairs are therefore: H sub 2 O/OH- and HCO sub 3-/H sub 2CO sub3.

Bicarbonate and Water Acid-Base Reaction

Lesson Summary

A Bronsted-Lowry base is a substance that accepts a proton in the form of a hydrogen (H) atom. This is why when we look at the Bronsted-Lowry acid-base reaction, the Bronsted-Lowry base is identified as the substance that gains a hydrogen atom. In contrast, the Bronsted-Lowry acid is the substance that donates the proton.

As a result, the Bronsted-Lowry acid-base reaction produces a conjugate acid and a conjugate base. The conjugate acid is the substance that results when the Bronsted-Lowry base accepts a proton, and the conjugate base is the compound that results after the acid has donated a proton. Because of this, the conjugate acid-base pairs differ by one hydrogen atom.

Register to view this lesson

Are you a student or a teacher? I am a student I am a teacher

Unlock Your Education

See for yourself why 30 million people use Study.com

Become a Study.com member and start learning now.

Become a Member

Already a member? Log In

Back

Resources created by teachers for teachers

Over 30,000 video lessons & teaching resources‐all in one place. Video lessons Quizzes & Worksheets Classroom Integration Lesson Plans

I would definitely recommend Study.com to my colleagues. It’s like a teacher waved a magic wand and did the work for me. I feel like it’s a lifeline.

Jennifer B. Teacher Jennifer B. Try it now Back

Recommended Lessons and Courses for You

  • Related Lessons
  • Related Courses

Recommended Lessons for You

Conjugate Base | Definition & Examples Conjugate Base | Definition & Examples Lewis Base Definition, Reactions & Examples Lewis Base Definition, Reactions & Examples Strong Base | Overview, Examples & Characteristics Strong Base | Overview, Examples & Characteristics Arrhenius Base | Definition, Characteristics & Examples Arrhenius Base | Definition, Characteristics & Examples Bronsted-Lowry Acid | Definition, Theory & Examples Bronsted-Lowry Acid | Definition, Theory & Examples Lewis Acid & Base | Definition & Examples Lewis Acid & Base | Definition & Examples Oxidation Number Meaning, Rules & Examples Oxidation Number Meaning, Rules & Examples

Related Courses

Chemistry 101: General Chemistry Chemistry 101: General Chemistry SAT Subject Test Chemistry: Practice and Study Guide SAT Subject Test Chemistry: Practice and Study Guide Holt McDougal Earth Science: Online Textbook Help Holt McDougal Earth Science: Online Textbook Help Glencoe Earth Science: Online Textbook Help Glencoe Earth Science: Online Textbook Help Holt Chemistry: Online Textbook Help Holt Chemistry: Online Textbook Help Glencoe Chemistry - Matter And Change: Online Textbook Help Glencoe Chemistry - Matter And Change: Online Textbook Help Holt McDougal Modern Chemistry: Online Textbook Help Holt McDougal Modern Chemistry: Online Textbook Help Holt McDougal Physics: Online Textbook Help Holt McDougal Physics: Online Textbook Help Analytical Chemistry: Help & Review Analytical Chemistry: Help & Review OSAT Physics (014) Study Guide and Test Prep OSAT Physics (014) Study Guide and Test Prep HESI Admission Assessment (A2) Study Guide and Exam Prep HESI Admission Assessment (A2) Study Guide and Exam Prep HSC Chemistry: Exam Prep & Syllabus HSC Chemistry: Exam Prep & Syllabus AP Chemistry Study Guide and Exam Prep AP Chemistry Study Guide and Exam Prep Fundamentals of Nursing Fundamentals of Nursing FTCE Physics 6-12 (032) Study Guide and Exam Prep FTCE Physics 6-12 (032) Study Guide and Exam Prep SAT Subject Test Biology: Practice and Study Guide SAT Subject Test Biology: Practice and Study Guide Chemistry: High School Chemistry: High School Weather and Climate Weather and Climate Supplemental Science: Study Aid Supplemental Science: Study Aid UExcel Anatomy & Physiology: Study Guide & Test Prep UExcel Anatomy & Physiology: Study Guide & Test Prep Start today. Try it now Chemistry 101: General Chemistry

14 chapters | 133 lessons | 11 flashcard sets

Ch 1. Experimental Chemistry and Introduction to Matter
  • Metric System | Measurements, Conversion & Units 8:47
  • Unit Conversion and Dimensional Analysis 10:29
  • Significant Figures and Scientific Notation | Rules & Examples 10:12
  • Chemistry Lab Equipment | Names, Types & Uses 8:44
  • Physical & Chemical Properties | Overview, Difference & Examples 7:22
  • Physical vs. Chemical Changes in Matter | Overview & Differences 6:42
  • Separating Mixtures | Methods & Examples 8:26
  • Condensation | Definition, Examples & Process 4:09
Ch 2. Atom Ch 3. The Periodic Table Ch 4. Nuclear Chemistry Ch 5. Chemical Bonding Ch 6. Liquids and Solids Ch 7. Gases Ch 8. Solutions Ch 9. Stoichiometry Ch 10. Chemical Reactions Ch 11. Equilibrium Ch 12. Kinetics Ch 13. Thermodynamics Ch 14. Studying for Chemistry 101

Bronsted Lowry Base | Definition, Reactions & Examples Related Study Materials

Related Lessons

Conjugate Base | Definition & Examples Conjugate Base | Definition & Examples Lewis Base Definition, Reactions & Examples Lewis Base Definition, Reactions & Examples Strong Base | Overview, Examples & Characteristics Strong Base | Overview, Examples & Characteristics Arrhenius Base | Definition, Characteristics & Examples Arrhenius Base | Definition, Characteristics & Examples Bronsted-Lowry Acid | Definition, Theory & Examples Bronsted-Lowry Acid | Definition, Theory & Examples Lewis Acid & Base | Definition & Examples Lewis Acid & Base | Definition & Examples Oxidation Number Meaning, Rules & Examples Oxidation Number Meaning, Rules & Examples

Related Courses

Chemistry 101: General Chemistry Chemistry 101: General Chemistry SAT Subject Test Chemistry: Practice and Study Guide SAT Subject Test Chemistry: Practice and Study Guide Holt McDougal Earth Science: Online Textbook Help Holt McDougal Earth Science: Online Textbook Help Glencoe Earth Science: Online Textbook Help Glencoe Earth Science: Online Textbook Help Holt Chemistry: Online Textbook Help Holt Chemistry: Online Textbook Help Glencoe Chemistry - Matter And Change: Online Textbook Help Glencoe Chemistry - Matter And Change: Online Textbook Help Holt McDougal Modern Chemistry: Online Textbook Help Holt McDougal Modern Chemistry: Online Textbook Help Holt McDougal Physics: Online Textbook Help Holt McDougal Physics: Online Textbook Help Analytical Chemistry: Help & Review Analytical Chemistry: Help & Review OSAT Physics (014) Study Guide and Test Prep OSAT Physics (014) Study Guide and Test Prep HESI Admission Assessment (A2) Study Guide and Exam Prep HESI Admission Assessment (A2) Study Guide and Exam Prep HSC Chemistry: Exam Prep & Syllabus HSC Chemistry: Exam Prep & Syllabus AP Chemistry Study Guide and Exam Prep AP Chemistry Study Guide and Exam Prep Fundamentals of Nursing Fundamentals of Nursing FTCE Physics 6-12 (032) Study Guide and Exam Prep FTCE Physics 6-12 (032) Study Guide and Exam Prep SAT Subject Test Biology: Practice and Study Guide SAT Subject Test Biology: Practice and Study Guide Chemistry: High School Chemistry: High School Weather and Climate Weather and Climate Supplemental Science: Study Aid Supplemental Science: Study Aid UExcel Anatomy & Physiology: Study Guide & Test Prep UExcel Anatomy & Physiology: Study Guide & Test Prep
  • Related Topics
    Browse by Courses
  • Biology 102: Basic Genetics
  • Biology 103: Microbiology
  • AP Biology Study Guide and Exam Prep
  • MTTC Integrated Science (Secondary) (094) Study Guide and Test Prep
  • Holt Science Spectrum - Physical Science: Online Textbook Help
  • Holt Science Spectrum - Physical Science with Earth and Space Science: Online Textbook Help
  • NYSTCE Biology (160) Study Guide and Exam Prep
  • OSAT Physics (014) Study Guide and Test Prep
  • TASC Science: Prep and Practice
  • GACE Health Education (613) Study Guide and Test Prep
  • OAE Earth and Space Science (014) Study Guide and Test Prep
  • MTTC Earth/Space Science (020) Study Guide and Test Prep
  • AEPA Earth Science (AZ045) Study Guide and Test Prep
  • CSET Science Study Guide and Test Prep
  • Biology 106: Pathophysiology
    Browse by Lessons
  • Bronsted-Lowry Definition, Equation & Examples
  • What is an Alkali? - Lesson for Kids
  • Weak Bases & Base Ionization Constants
  • Weak Bases: Examples & Overview
Create an account to start this course today Used by over 30 million students worldwide Create an account Like this lesson Share

Explore our library of over 88,000 lessons

Search Browse Browse by subject Upgrade to enroll Upgrade to Premium to enroll in Chemistry 101: General Chemistry Enrolling in a course lets you earn progress by passing quizzes and exams. Track course progress Take quizzes and exams Earn certificates of completion You will also be able to:
  • Create a Goal
  • Create custom courses
  • Get your questions answered
Upgrade to Premium to add all these features to your account! Upgrade Now Upgrade to Premium to add all these features to your account!

Tag » What Is A Bronsted Lowry Base