Bronsted-Lowry Acid | Theory, List & Examples
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- Author Chase Smith
Chase is a 14 year veteran science teacher with a specialization is chemistry/STEM. He has a Bachelors Degree in Chemistry and a Master's Degree in Instructional Media with a specialization in STEM.
View bio - Instructor Nissa Garcia
Nissa has a masters degree in chemistry and has taught high school science and college level chemistry.
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Table of Contents
- Bronsted-Lowry Theory
- Bronsted-Lowry Acid Definition
- Bronsted-Lowry Acid Examples
- Lesson Summary
What is acid according to the Bronsted-Lowry concept?
A Bronsted-Lowry acid must be a proton donor. This would be paired with an atom that would be accepting a proton known as a Bronsted-Lowry base.
Is water a Bronsted-Lowry acid?
Bronsted-Lowry sees water as the potential to be either an acid or a base. Since water has the ability to either accept or donate a proton, it could fit into either category.
How do you identify a Bronsted-Lowry acid?
A Bronsted-Lowry acid can best be identified as a compound on the reactants side of the equation which either loses a hydrogen ion on the product's side or at least a positively charged particle.
What is a Bronsted-Lowry acid example?
An example of a Bronsted-Lowry acid would be H3O+. If it reacted with another compound and donated a proton to become H2O, it would then fit the definition.
Create an accountTable of Contents
- Bronsted-Lowry Theory
- Bronsted-Lowry Acid Definition
- Bronsted-Lowry Acid Examples
- Lesson Summary
Bronsted-Lowry Theory
The Bronsted-Lowry Theory of acids was created by two men working at the same time period on essentially the same concept. These two men believed that there was a shortcoming to the Arrhenius definition that needed to be addressed with an alteration to the thinking. The Bronsted-Lowry theory of acid/base definition focuses on the idea of a proton being donated and accepted in a reaction rather than solely focusing on a solution's behavior in water as Arrhenius had done.
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Bronsted-Lowry Acid Definition
A Bronsted-Lowry acid is defined as a substance which donates a proton in a chemical reaction. A Bronsted-Lowry base, conversely, is a substance that accepts a proton in a chemical reaction.
While a proton in the mentioned definition often turns out to be a hydrogen ion, Bronsted-Lowry accounted for the possibility that hydrogen will not be involved. In cases where water is not present, Bronsted-Lowry's definitions of acids/bases still hold.
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The key to determining which substance is the acid and which substance is the base in the reactants is to examine the two products that are created from the reaction. In each reaction, there will be what is referred to as a conjugate acid, and a conjugate base. The conjugate base will be a negatively charged ion, and the conjugate acid will be a positively charged particle. These two products were created because of either the loss of or acceptance of an electron from its counterpart. Examples of this in action are the best way to get the full picture:
{eq}NH_{3}\: \: +\: \: H_{2}O\: \: \rightarrow \: \: NH_{4}^{+}\: \: +\: OH^{-} {/eq}
In this example, by examining the products, it is easier to make a determination on which reactant is the acid and which is the base. The NH4 contains a positive charge, which is the signal that it is labeled as the conjugate acid. The conjugate acid will be matched up with the compound in the reactants that is identical except that it will have one less hydrogen. In this example, NH4+ has a conjugate partner of NH3. The partner of the conjugate acid is the Bronsted-Lowry base. This means that NH3 is our Bronsted-Lowry base in this example.
The other product in this reaction, OH-, is labeled as the conjugate base due to its negative charge. In order to determine its partner, the key is to determine the reactant that is identical except that it will have one more hydrogen. The reactant with one more hydrogen than OH- is H20. With OH- being the conjugate base, the partner to the conjugate base is the Bronsted-Lowry acid. H20 is the Bronsted-Lowry acid in this reaction.
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Bronsted-Lowry Acid Examples
The Bronsted-Lowry acid/base definition requires a bit of analysis. For each example, the following table will provide examples of equations and the acid/base pairs that go along with them.
| Chemical Equation | BL acid | BL base | Conjugate acid | Conjugate base |
|---|---|---|---|---|
| HCl + H20 -----> Cl- + H30+ | HCl | H20 | H30+ | Cl- |
| C6H5NH2 + H20 ---> C6H5NH3+ + OH- | H20 | C6H5NH2 | C6H5HN3+ | OH- |
| HBr + NH3 --->. NH4+ + Br- | HBr | NH3 | NH4+ | Br- |
| CH3OH + HNO3 ---> CH3OH2+ + NO3- | HNO3 | CH3OH | CH3OH2+ | NO3- |
| H2SO4 + H20 --->. HSO4- + H3O+ | H2SO4 | H2O | H3O+ | HSO4- |
From this table, take notice that each of the conjugate acids is the negatively charged particle in the product. By finding the negative ion and matching it up with its partner, the Bronsted-Lowry acid can be determined. In the first example in the table, the acid/conjugate base pair would be HCl/ Cl-. The Bronsted-Lowry base/conjugate acid pair in the first line would be H20/H30+.
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Lesson Summary
A Bronsted-Lowry acid is best defined as a proton donor in a chemical reaction. A Bronsted-Lowry basewould then be classified as a proton acceptor in a chemical reaction. In order to determine which reactant is the acid and which is the base, it is best to analyze the products of the chemical reaction. The negatively charged particle of the products is labeled as the conjugate base. To match the conjugate base with a partnered compound, find the reactant that has one additional proton (usually a hydrogen) to the conjugate base. The compound in the reactants that has one more proton than its conjugate base is known as the Bronsted-Lowry acid. A conjugate acid can be determined by examining the products for a positively charged ion. The product that has a positive charge will be matched up with a reactant that has one less proton (typically a hydrogen). The reactant with one less hydrogen than its conjugate acid is named the Bronsted-Lowry base.
An example of an acid/base chemical reaction is the best way to understand the terminology.
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The Bronsted-Lowry acid is C2H3O2H with a conjugate base pair of C2H3O2--. The Bronsted-Lowry base is H20 with a conjugate acid pair of H3O+. The C2H3O2H is a proton donor, while the H20 is a proton acceptor. While this example contains the presence of water, the Bronsted-Lowry definition is more useful than its predecessor, the Arrhenius method, due to the fact that water is not needed in order to determine which reactant is indeed the acid/base.
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Video Transcript
What is a Bronsted-Lowry Acid?
What makes a solution an acid? There have been different definitions proposed by different scientists. However, there were two scientists who independently proposed essentially the same theory about the definition of acids and bases.
In 1923, Johannes Nicolaus Bronsted and Thomas Martin Lowry, from Denmark and England respectively, published the same theory on how acidic and basic solutions behaved. According to Bronsted and Lowry, acids are solutions that donate protons and bases are solutions that accept protons.
These scientists came up with this theory independently and relatively at the same time, so the theory has both of their names attached to it: Bronsted-Lowry Theory of Acids and Bases.
A Bronsted-Lowry acid is a solution that donates protons, and is known as a proton donor. It donates protons in the form of a hydrogen ion (H+). This is reinforced by the definition of an acid, which is a solution that has an excess of hydrogen ions (H+). The Bronsted-Lowry base, on the other hand, is a solution that accepts protons, and is known as a proton acceptor.
Going back to a Bronsted-Lowry acid, in general it must contain a hydrogen ion that it can give up. When the acid gives up the hydrogen ion, which has a charge equal to positive one (+1), the charge of the acid decreases by positive one (+1). A Bronsted-Lowry acid-base reaction generally looks like this:
 |
Here the Bronsted-Lowry acid, HA, gives up or donates its hydrogen ion, and the Bronsted-Lowry base, B, accepts the hydrogen ion. As a result, when the hydrogen ion attaches itself to the base, the base gains a charge of positive one, as shown by the positive charge at the products side, HB+. In the products side, you also see that after losing the hydrogen ion, A- is all by itself and has a charge of negative one because it donated its hydrogen ion. The double arrow between the reactants and the products is what we call an equilibrium sign, which means that it is possible for the reaction to occur forwards and backwards.
In this reaction, we see that the products of the acid-base reaction are a conjugate acid and a conjugate base. A conjugate acid is the substance that is produced after the base accepts the proton. When this occurs, its charge increases by +1. A conjugate base, on the other hand, is produced after the acid donates its proton. When this occurs, its charge decreases by +1. A conjugate acid-base pair is a set of two substances, where one substance differs from the other substance by one proton or hydrogen atom. In this reaction, the conjugate acid base pairs are: HA/A- and B/HB+.
How do we know again which substance is the Bronsted-Lowry acid? We do this by counting the hydrogen ion for each substance in the chemical reaction. If a substance lost a hydrogen ion, then it is a Bronsted-Lowry acid.
Bronsted-Lowry Acid-Base Reactions
Let us go over a few Bronsted-Lowry acid-base reactions and practice identifying Bronsted-Lowry acids, as well as conjugate acids and bases.
First, let's look at the reaction between acetic acid and water.
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Let's identify the substances. Acetic acid (CH3COOH) is the Bronsted-Lowry acid because it is the proton donor - it donated its hydrogen ion to water. Water is the Bronsted-Lowry base because it is the proton acceptor. The conjugate base is CH3COO- because it is the substance produced after the proton, hydrogen, is donated. The conjugate acid is H3O+ because this is the substance produced when the H2O accepted the proton. The conjugate acid-base pairs are: CH3COOH/CH3COO- and H2O/H3O+. If we label the reaction accordingly, it will look like this:
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Let's now look at the reaction between ammonia (NH3) and hydrochloric acid (HCl).
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If we identify each substance, then NH3 is the Bronsted-Lowry base, HCl is the Bronsted-Lowry acid, NH4+ is the conjugate acid and Cl- is the conjugate base. The conjugate acid-base pairs are: HCl/Cl- and NH3/NH4+.
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Let's take a look at one more example:
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In this reaction, the Bronsted-Lowry acid is HNO2, and the Bronsted-Lowry base is PO43-, the conjugate acid is HPO42-, and the conjugate base is NO2-. The conjugate acid-base pairs are: HNO2/NO2- and PO43-/HPO42-.
Lesson Summary
A Bronsted-Lowry acid is a substance that donates a proton in the form of a hydrogen ion. The Bronsted-Lowry base, in turn, accepts this proton, and the resulting products are a conjugate acid and a conjugate base. The conjugate acid is the result of the base accepting the proton, so the charge increases by +1. The conjugate base results from the acid that loses the proton, so the charge decreases by +1.
When we identify Bronsted-Lowry acids, we identify it as the substance that loses the hydrogen ion or proton. Bronsted-Lowry acid-base reactions have two conjugate acid-base pairs that consist of the Bronsted-Lowry acid/conjugate base and the Bronsted-Lowry base/conjugate acid.
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