Chemistry Acids and Bases Overview

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Questions and Answers

What is the fundamental concept in chemistry that is explored in this presentation?

Acids and bases

According to the Arrhenius theory, what do acids produce when dissolved in water?

  • Chloride ions (Cl-)
  • Sodium ions (Na+)
  • Hydroxide ions (OH-)
  • Hydrogen ions (H+) (correct)

Which of the following is an example of an Arrhenius base?

  • Sodium hydroxide (NaOH) (correct)
  • Carbon dioxide (CO2)
  • Ammonia (NH3)
  • Hydrochloric acid (HCl)

The Brønsted-Lowry theory defines acids as proton donors.

<p>True (A)</p> Signup and view all the answers

What does ammonia (NH3) do in the Brønsted-Lowry theory?

<p>Ammonia accepts a proton from water, forming NH4+ and OH-</p> Signup and view all the answers

Flashcards

Arrhenius Acids

Compounds that release hydrogen ions (H+) when dissolved in water.

Arrhenius Bases

Compounds that produce hydroxide ions (OH-) when dissolved in water.

Brønsted-Lowry Theory

The theory that describes acids and bases in terms of proton (H+) transfer.

Brønsted-Lowry Acid

A substance that donates a proton (H+) in a chemical reaction.

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Brønsted-Lowry Base

A substance that accepts a proton (H+) in a chemical reaction.

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Conjugate Base

The species formed when an acid loses a proton.

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Conjugate Acid

The species formed when a base gains a proton.

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Strong Acids

Acids that completely ionize (dissociate) in water, releasing all of their hydrogen ions.

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Weak Acids

Acids that only partially ionize in water, releasing some of their hydrogen ions.

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Strong Bases

Bases that completely ionize in water, releasing all of their hydroxide ions.

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Weak Bases

Bases that only partially ionize in water, releasing some of their hydroxide ions.

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Acid Strength

The ability of an acid to donate a proton.

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Base Strength

The ability of a base to accept a proton.

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pH Scale

A measure of the hydrogen ion concentration in a solution. Values range from 0 to 14, with lower values indicating higher acidity.

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Acidic Solution

A solution with a pH less than 7. It contains more hydrogen ions (H+) than hydroxide ions (OH-).

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Basic Solution

A solution with a pH greater than 7. It contains more hydroxide ions (OH-) than hydrogen ions (H+).

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Neutral Solution

A solution with a pH of 7. It contains equal amounts of hydrogen ions (H+) and hydroxide ions (OH-).

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Amphoteric Substance

A substance that can act as both an acid and a base.

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Acid-Base Reaction

A chemical reaction that involves the transfer of a proton from an acid to a base.

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Study Notes

Acids and Bases Overview

  • Acids and bases are fundamental concepts in chemistry
  • Different definitions, properties, and applications of these compounds are explored

Arrhenius Theory of Acids and Bases

  • Definition: Acids produce hydrogen ions (H+) when dissolved in water. Bases produce hydroxide ions (OH-) when dissolved in water.
  • Examples: Hydrochloric acid (HCl) releases H+ ions, while sodium hydroxide (NaOH) releases OH- ions.

Brønsted-Lowry Definition of Acids and Bases

  • Proton Transfer: Acids are proton donors (H+), and bases are proton acceptors (H+).
  • Examples: HCl donates a proton to water, forming H3O+, and ammonia (NH3) accepts a proton from water, forming NH4+ and OH-.

Conjugate Acids and Bases

  • Conjugate Acid-Base Pairs: An acid and its conjugate base differ by a proton, and a base and its conjugate acid differ by a proton.
  • Examples: HCl (acid) and Cl- (conjugate base) differ by a proton, and NH3 (base) and NH4+ (conjugate acid) differ by a proton.

Strong and Weak Acids and Bases

  • Strong Acids: Ionize completely.

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