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6.10.2 - the brönsted- lowry Acids and bases

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Introduction to Brönsted-Lowry Theory

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Teacher
Teacher

Today, we will explore the Brönsted-Lowry theory of acids and bases. Can anyone tell me what an acid is according to this theory?

Student 1
Student 1

Isn't it something that donates protons?

Teacher
Teacher

Exactly! An acid is defined as a proton donor. And what about bases?

Student 2
Student 2

Bases accept protons!

Teacher
Teacher

Correct! So acids donate protons, and bases accept them. This is a broader definition than the one from Arrhenius.

Student 3
Student 3

So, does that mean that water can act as both?

Teacher
Teacher

Yes! Water can act as both an acid and a base depending on the reaction.

Teacher
Teacher

Remember the acronym PAB—Proton-Accepting Base. It can help you recall that bases accept protons.

Teacher
Teacher

In summary, the Brönsted-Lowry definitions expand our understanding and will allow us to discuss dynamic systems of proton transfer.

Conjugate Acid-Base Pairs

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Teacher
Teacher

Now that we know acids and bases, let’s talk about conjugate pairs. Can someone explain this concept?

Student 2
Student 2

I think it's about an acid turning into a base after donating a proton?

Teacher
Teacher

Exactly! When an acid donates a proton, it becomes its conjugate base. For example, when hydrochloric acid donates a proton, it becomes chloride ion.

Student 1
Student 1

What about the reverse? How does that work?

Teacher
Teacher

Great question! The conjugate base can gain a proton to revert to its acid form. So, we can say HCl and Cl– are a conjugate acid-base pair.

Teacher
Teacher

You can remember the phrase 'Donor and Acceptor' using the mnemonic DAC—Donor Acids Create conjugates.

Teacher
Teacher

To conclude, understanding conjugate acid-base pairs helps us predict the direction of acid-base reactions.

Applications and Examples of Brönsted-Lowry

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Teacher
Teacher

Let’s look at some examples of Brönsted-Lowry acids and bases in action. Who can give me an example?

Student 3
Student 3

I remember the ammonia and water example where ammonia accepts a proton.

Teacher
Teacher

Correct! Ammonia becomes NH4+, acting as a Brönsted base. What about an example of an acid?

Student 4
Student 4

Hydrochloric acid in water!

Teacher
Teacher

That’s right! It dissociates to form H3O+ and Cl–. So in a solution, it's dynamic—H3O+ and Cl– will easily transfer protons between them.

Teacher
Teacher

Can anyone explain why this theory is significant in biological systems?

Student 1
Student 1

Because many biological systems involve proton transfer, like enzyme catalysis.

Teacher
Teacher

Yes! Remember: Biological reactions often revolve around proton transfer—keep this in mind as you study further.

Introduction & Overview

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Quick Overview

The Brönsted-Lowry theory defines acids as proton donors and bases as proton acceptors, expanding the understanding of acid-base chemistry.

Standard

This section elaborates on the Brönsted-Lowry theory, illustrating the roles of different substances in proton transfer reactions and the concept of conjugate acid-base pairs, which enriches the understanding of acid-base interactions beyond the Arrhenius definition.

Detailed

The Brönsted-Lowry theory, proposed by chemists Johannes Brönsted and Thomas Lowry, revolutionizes the classical definition of acids and bases. In this theory, acids are substances that donate hydrogen ions (protons), while bases are those that accept hydrogen ions. This theory allows for a broader range of acid-base reactions, including those that do not occur in aqueous solutions. Key concepts include the formation of conjugate acid-base pairs, where an acid transforms into its conjugate base after donating a proton, and a base transforms into a conjugate acid upon accepting a proton. Examples include the reaction of ammonia with water, where ammonia accepts a proton to become ammonium, showcasing the dual acidic and basic nature of water.

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Audio Book

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Definition of Brönsted-Lowry Acids and Bases

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The Danish chemist, Johannes Brönsted and the English chemist, Thomas M. Lowry gave a more general definition of acids and bases. According to Brönsted-Lowry theory, acid is a substance that is capable of donating a hydrogen ion H+ and bases are substances capable of accepting a hydrogen ion, H+. In short, acids are proton donors and bases are proton acceptors.

Detailed Explanation

Brönsted-Lowry theory expands the definition of acids and bases beyond the traditional Arrhenius definitions. In this theory, an acid is identified by its ability to donate a proton (H+), while a base is defined by its ability to accept a proton. For example, hydrochloric acid (HCl) donates a proton to water, forming hydronium ions (H3O+), while ammonia (NH3) accepts a proton from water, forming ammonium ions (NH4+). This theory helps us understand acid-base reactions in a broader range of contexts, not limited to aqueous solutions.

Examples & Analogies

Think of acids and bases as two dance partners in a ballroom. The acid, which is the proton donor, hands off a token (the hydrogen ion) to its partner, who is the base (the proton acceptor). This exchange allows them to create a new dance (the resulting chemical reaction), showcasing how they can interact in various environments, not just on the dance floor (in water).

Examples of Brönsted-Lowry Acid-Base Reactions

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Consider the example of dissolution of NH3 in H2O represented by the following equation: H2O + NH3 ⇌ NH4+ + OH–. In this reaction, water acts as a proton donor and ammonia acts as a proton acceptor, identifying them as Brönsted-Lowry acid and base, respectively.

Detailed Explanation

In the reaction between ammonia (NH3) and water (H2O), ammonia accepts a proton from water. This results in the formation of ammonium ions (NH4+) and hydroxide ions (OH–). In this case, water donates a proton and is classified as the Brönsted-Lowry acid, while ammonia, which accepts the proton, is the Brönsted-Lowry base. This interaction highlights the dynamic nature of acid-base reactions and how reactants can switch roles depending on the context.

Examples & Analogies

Imagine a game of catch where one player (water) throws a ball (the proton) to another player (ammonia). The player who catches the ball becomes a different character in the game (the ammonium ion) while the thrower, after throwing the ball, transforms into another version of themselves, now having one less ball to throw (the hydroxide ion). This illustrates how the roles of acids and bases can change in chemical reactions.

Conjugate Acid-Base Pairs

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The acid-base pair that differs only by one proton is called a conjugate acid-base pair. Therefore, OH– is called the conjugate base of an acid H2O, and NH4+ is called conjugate acid of the base NH3.

Detailed Explanation

Conjugate acid-base pairs are vital in understanding acid-base chemistry. They represent the relationship between an acid and a base that differ by a single proton. For instance, when a strong acid donates a proton, it forms a weaker base, known as its conjugate base. Conversely, when a base accepts a proton, it forms a weak acid, known as its conjugate acid. This dynamic highlights how substances can behave differently depending on their protonation state.

Examples & Analogies

Consider a tennis game where a player can either serve (be an acid) or receive (be a base). If the player serves a ball (donates a proton), they are now like the conjugate base because they have one less ball to serve. When they receive a ball (accept a proton), they become the conjugate acid because they have that ball back to serve again. This cycle demonstrates how substances can switch between being acids and bases.

Definitions & Key Concepts

Learn essential terms and foundational ideas that form the basis of the topic.

Key Concepts

  • Proton Donation: In the Brönsted-Lowry theory, acids donate protons and bases accept protons.

  • Conjugate Pairs: An acid-base pair that differs by the presence or absence of a single proton.

  • Dual Role of Water: Water can act as both an acid and a base depending on the situation.

Examples & Real-Life Applications

See how the concepts apply in real-world scenarios to understand their practical implications.

Examples

  • Example of NH3 acting as a base: NH3 + H2O ↔ NH4+ + OH–.

  • Example of HCl acting as an acid in water: HCl + H2O ↔ H3O+ + Cl–.

Memory Aids

Use mnemonics, acronyms, or visual cues to help remember key information more easily.

🎵 Rhymes Time

  • Protons fly from acids high, bases take them, oh so sly!

🧠 Other Memory Gems

  • Can A Base Steal A Proton? (CAB-SP), remembering that Bases Accept protons in Brönsted-Lowry terms.

📖 Fascinating Stories

  • Imagine a party where acids hand out balloons (protons) and bases gather them with open hands. The more balloons a base gathers, the more it becomes a 'party-goer' or an 'acidic character' by holding onto those balloons!

🎯 Super Acronyms

PAB = Proton-Accepting Base, to remember the role of Bases in the Brönsted-Lowry theory.

Flash Cards

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Glossary of Terms

Review the Definitions for terms.

  • Term: BrönstedLowry Acid

    Definition:

    A substance that donates a hydrogen ion (proton).

  • Term: BrönstedLowry Base

    Definition:

    A substance that accepts a hydrogen ion (proton).

  • Term: Conjugate Acid

    Definition:

    The species formed when a base gains a proton.

  • Term: Conjugate Base

    Definition:

    The species formed when an acid donates a proton.