Acids and Bases Overview

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Questions and Answers

According to the Arrhenius theory, what ions do acids and bases produce in water?

Acids produce hydrogen ions $H^{+}$ while bases produce hydroxide ions $OH^{-}$ in water.

What is the role of hydronium ions in the context of acid dissociation?

Hydronium ions ($H_{3}O^{+}$) represent the hydrated form of hydrogen ions produced by acids in solution.

How does ammonia demonstrate a limitation of the Arrhenius theory?

Ammonia does not contain hydroxide ions but produces them when it reacts with water, illustrating that not all bases fit the Arrhenius definition.

Define a conjugate acid-base pair and give an example.

<p>A conjugate acid-base pair consists of two related substances that differ by a proton; for example, $NH_{4}^{+}$ (ammonium) and $NH_{3}$ (ammonia).</p> Signup and view all the answers

Explain the difference between the roles of acids and bases according to the Brønsted-Lowry theory.

<p>In the Brønsted-Lowry theory, acids are proton donors while bases are proton acceptors during a reaction.</p> Signup and view all the answers

Flashcards

Arrhenius Acid

A substance that produces hydrogen ions ($H^{+}$) when dissolved in water.

Arrhenius Base

A substance that produces hydroxide ions ($OH^{-}$) when dissolved in water.

Brønsted-Lowry Acid

A proton donor.

Brønsted-Lowry Base

A proton acceptor.

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Conjugate Acid-Base Pair

Two molecules that differ by a proton ($H^{+}$ ion) are related.

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Study Notes

Acid & Bases

Arrhenius Theory:
- Acid: A substance that dissociates in water to produce hydrogen ions (H⁺).
- Base: A substance that dissociates in water to form hydroxide ions (OH^-).
- Example: HCl(aq) → H⁺(aq) + Cl^-(aq)
- Example: NaOH(aq) → Na⁺(aq) + OH^-(aq)
Limitations of Arrhenius Theory:
- Not all acids and bases are explained correctly
- Protons are always hydrated, so a hydrated proton is called a hydronium ion (H₃O⁺).
- Ammonia does not contain hydroxide ions, but it does produce them when reacted with water.

Brønsted-Lowry Theory

Acid: A proton donor (H⁺ ion can be removed)
Base: A proton acceptor (accepts a proton, H⁺)
Example:
- HCl + H₂O → H₃O⁺ + Cl⁻
- H₂O acts as a base, accepting a proton from the acid HCl