Introductory Chemistry II: Acids and Bases
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Questions and Answers

Which acid-base theory emphasizes the role of proton donors and acceptors?

  • Arrhenius Theory
  • Lux-Flood Theory
  • Lewis Theory
  • Brønsted-Lowry Theory (correct)

What characterizes Lewis acids and bases?

  • They require an aqueous solution to operate.
  • They involve electron pair acceptors and donors. (correct)
  • They are defined based on proton transfer.
  • They strictly follow Arrhenius definitions.

What type of substances does the self-ionizing definition of acids and bases apply to?

  • Nonaqueous media (correct)
  • Protic substances only
  • Only aqueous solutions
  • Ionic compounds

Which theory is considered the most general in defining acids and bases?

<p>Lewis Theory (D)</p> Signup and view all the answers

In which of the following reactions would a Lewis base be characterized as donating an electron pair?

<p>A substance combining with a Lewis acid (B)</p> Signup and view all the answers

What does HSAB stand for in the classification of metal ions and ligands?

<p>Hard and Soft Acids and Bases (C)</p> Signup and view all the answers

Which of the following compounds is an example of a strong acid in liquid solutions?

<p>H2SO4 (A)</p> Signup and view all the answers

Which type of oxides typically exhibit acidic properties according to trends in acid-base properties?

<p>Non-metallic oxides (D)</p> Signup and view all the answers

What does an Arrhenius acid release when dissolved in water?

<p>H+ ions (B)</p> Signup and view all the answers

Which of the following is a strong acid according to the Arrhenius definition?

<p>HClO4 (A)</p> Signup and view all the answers

Why is NH3 (ammonia) not classified as an Arrhenius base?

<p>It does not contain hydroxide groups. (B)</p> Signup and view all the answers

An Arrhenius base is characterized by producing which ion when dissolved in water?

<p>OH- (C)</p> Signup and view all the answers

How does a strong acid behave in an aqueous solution according to the Arrhenius theory?

<p>It completely ionizes. (A)</p> Signup and view all the answers

Which of the following substances is considered a strong base?

<p>LiOH (D)</p> Signup and view all the answers

What happens when HCl gas is dissolved in water according to the Arrhenius definition?

<p>It increases the concentration of H3O+ ions. (A)</p> Signup and view all the answers

Which statement about Arrhenius acids is true?

<p>They are only defined in terms of water. (D)</p> Signup and view all the answers

What is a characteristic of acids?

<p>They turn blue litmus red. (A)</p> Signup and view all the answers

Which of the following definitions pertains to acids and bases?

<p>Solvent System Definition (C)</p> Signup and view all the answers

What happens to the pH level of a solution when it is more acidic?

<p>The pH decreases. (B)</p> Signup and view all the answers

What taste is primarily associated with bases?

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

Which statement correctly describes a base's effect on litmus paper?

<p>It turns it blue. (B)</p> Signup and view all the answers

What do both Arrhenius and Brønsted-Lowry definitions focus on regarding acids and bases?

<p>The production of hydroxide or hydrogen ions. (D)</p> Signup and view all the answers

What is the typical pH range of a basic solution?

<p>Greater than 7 (D)</p> Signup and view all the answers

Which of the following is a common reaction of acids?

<p>Reacting with bases to form salts. (C)</p> Signup and view all the answers

Which statement correctly describes weak acids?

<p>Weak acids undergo reversible reactions with corresponding ions. (A)</p> Signup and view all the answers

What characterizes a weak base, such as ammonium hydroxide?

<p>It exists in both ionized and un-ionized forms in solution. (A)</p> Signup and view all the answers

Which of the following describes a limitation of the Arrhenius concept of acids and bases?

<p>It considers only H+ and OH- ions in aqueous solutions. (C)</p> Signup and view all the answers

In an Arrhenius acid-base reaction, what are the products of the reaction between hydrochloric acid and sodium hydroxide?

<p>Sodium chloride and water (D)</p> Signup and view all the answers

Which of the following best describes a strong Arrhenius base?

<p>It completely dissociates in water to produce OH- ions. (B)</p> Signup and view all the answers

How can you differentiate between strong and weak Arrhenius acids?

<p>By their level of ionization in water. (C)</p> Signup and view all the answers

Which ion would be produced by the dissociation of calcium hydroxide in water?

<p>OH- and Ca2+ (A)</p> Signup and view all the answers

What is one characteristic difference between the definitions of Bronsted-Lowry acids and bases compared to Arrhenius acids and bases?

<p>Bronsted-Lowry bases can accept protons, not just produce OH- ions. (B)</p> Signup and view all the answers

Flashcards

Arrhenius Acid

A substance that increases the concentration of H+ ions in an aqueous solution.

Brønsted-Lowry Acid

A substance that donates a proton (H+).

Solvent-oriented definition of acid-base

Defines acids and bases in terms of how they interact with different solvents or specific media (non-aqueous).

Self-ionizing solvent

A solvent that can ionize on its own, creating ions like H+ and OH- (e.g., water).

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Lewis Acid

A substance that accepts an electron pair.

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Lewis Base

A substance that donates an electron pair.

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Acidic Oxide

An oxide that reacts with water to form an acid.

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HSAB Theory

Hard and Soft Acid and Base theory. It classifies metal ions and ligands based on their electron-donating or electron-accepting characteristics.

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Acid

A substance with an aqueous solution characterized by a sour taste, turning blue litmus red, reacting with bases and metals to form salts, and having a pH less than 7.

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Base

A substance with an aqueous solution characterized by a bitter taste, slipperiness, turning red litmus blue, reacting with acids to form salts, and having a pH greater than 7.

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pH less than 7

Indicates an acidic solution, having a higher concentration of hydrogen ions.

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pH greater than 7

Indicates a basic solution, having a higher concentration of hydroxide ions.

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Arrhenius acid/base

The concept of acid and base describing the behaviour of acids and bases in water.

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Brønsted-Lowry definition

A definition of acids and bases that involves proton exchange.

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Solvent System Definition

A concept of acid and base, which is relevant to other solvents (beyond just water).

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Lewis Definition

A concept of acid and base involving electron-pair acceptance/donation.

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Arrhenius base

A substance that ionizes in water to produce OH- ions.

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Strong acid

An acid that ionizes completely in water.

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Strong base

A base that dissociates completely in water.

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Hydronium ion

H3O+, the form of H+ in aqueous solution (water).

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Hydroxide ion

OH-, the ion that indicates a base.

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Ionization

The process of forming ions from a neutral molecule.

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Dissociation

The separation of ions in a molecule into ions.

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Weak Acids

Acids that do not completely ionize in solution, resulting in a reversible reaction with their corresponding ions. They do not release all their hydrogen ions (H+) when dissolved in water.

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Weak Bases

Bases that do not completely ionize in solution, resulting in a reversible reaction with their corresponding ions. They do not release all their hydroxide ions (OH-) when dissolved in water.

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Dissociation constant (K)

A measure of the extent to which a weak acid or base ionizes in solution. It represents the ratio of the products (ions) to reactants (acid/base) at equilibrium.

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Limitations of Arrhenius theory?

The Arrhenius concept is limited to aqueous solutions only, focusing on H+ and OH-. It does not apply to non-aqueous solutions or substances that do not involve these ions.

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Arrhenius acid-base reaction?

A reaction between an Arrhenius acid (producing H+) and Arrhenius base (producing OH-), resulting in the formation of water (H2O) and a salt.

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Strong Arrhenius bases

Bases that completely ionize in water, releasing all their hydroxide ions (OH-), making the solution highly alkaline.

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Strong vs. Weak Arrhenius Acids

Strong acids completely ionize in solution releasing all their hydrogen ions (H+), while weak acids only partially ionize, releasing some H+ ions.

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Ionization of calcium hydroxide

Ca(OH)2 (aq) → Ca2+ (aq) + 2OH- (aq)

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Study Notes

Course Information

  • Course Title: Introductory Chemistry II
  • Course Code: CHEM 1820
  • Instructor: Dr. Joyann Marks
  • Email: [email protected]
  • Lecture Topic: Acids and Bases
  • Lecture Number: 1

Office Hours

  • Mondays: 2-3 PM
  • Wednesdays: 2-3 PM
  • Thursdays: 1-2 PM
  • Virtual appointments available via calendly.com/joyannmarks/uwichem
  • Email for scheduling outside of these times: [email protected]
  • Tutorials not available Tuesdays and Fridays at 10 AM due to scheduling conflicts

Learning Outcomes

  • Discuss acid-base properties of protic and aprotic substances and explain why the Lewis definition is most general.
  • Describe reactions in liquid NH3, HF, H2SO4, and BrF3.
  • Classify metal ions and ligands according to HSAB concepts.
  • Account for trends in acid-base properties of oxides, metal ions, and ligands.

Objectives for Acids and Bases

  • Review Arrhenius and Brønsted-Lowry theories of acids and bases.
  • Discuss solvent-oriented definitions of acids and bases.
  • Discuss self-ionizing and non-self-ionizing non-aqueous media.
  • Discuss Brønsted Lowry as a special case.
  • Discuss acidic and basic oxides (Lux-Flood definition).
  • Discuss trends in acid-base properties of oxides.
  • Discuss Lewis acid-base theory.
  • Discuss water as a Lewis base.
  • Discuss HSAB (Hard and Soft Acid and Base) concepts.
  • Discuss reactions of Lewis acids and bases.

Acids

  • Acid properties: sour taste, turning blue litmus red, reaction with bases to form salts.
  • Aqueous solutions have a pH less than 7. Lower pH means higher acidity and concentration of hydrogen ions (using Arrhenius/Brønsted-Lowry definitions).

Bases

  • Base properties: bitter taste, slippery to the touch, turning red litmus blue, react with acids to form salts.
  • Aqueous solutions have a pH greater than 7. Higher pH means higher basicity and concentration of hydroxide ions (using Arrhenius/Brønsted-Lowry definitions).

Definitions of Acids and Bases

  • Arrhenius acid and bases
  • Brønsted-Lowry Definition
  • Solvent System Definition
  • Lewis Definition
  • Lux-Flood Definition

Arrhenius Acids and Bases

  • Acid: substance that ionizes in water to produce H+ ions.
  • Base: substance that ionizes in water to produce OH- ions.
  • Limitations: Only applicable to aqueous solutions; doesn't account for bases like NH3.

Arrhenius Acids

  • An Arrhenius acid, when dissolved in water, increases the concentration of H3O+ (hydronium) ions.
  • Chemists often use H+(aq) as shorthand for H3O+(aq); this representation is for hydrogen ion in water.
  • Example: HCl(aq) → H+(aq) + Cl-(aq), where H+(aq) is actually H3O+(aq).

Arrhenius Bases

  • An Arrhenius base, when dissolved in water, increases the concentration of OH-(aq) hydroxide ions.
  • Example: NaOH(aq) → Na+(aq) + OH-(aq)

Strong Acids and Bases

  • Strong acid: ionizes completely in water.
  • Some strong acids (HCl, HBr, HI, HNO3, HClO4, H2SO4).
  • Strong base: dissociates completely in water.
  • Some strong bases (NaOH, LiOH, KOH, Ca(OH)2, Sr(OH)2, Ba(OH)2)

Weak Acids and Bases

  • Weak acid/base: partially/incomplete ionization in water
  • Example: acetic acid, HC2H3O2)(or CH3COOH) is a weak acid

Limitations of the Arrhenius Concept

  • Limited to aqueous solutions
  • Doesn’t account for properties of substances not involving OH⁻ or H⁺ ions.
  • The OH⁻ ion is singled out as the source of basicity when other species play a similar role in reactions.
  • Broader definitions of acids/bases are needed.

Arrhenius Acid-Base Reaction

  • Involves the reaction of an Arrhenius acid and an Arrhenius base.
  • Produces water and a salt.
  • Example: HCl(aq) + NaOH(aq) → NaCl(aq) + H2O(l)

Additional Information

  • Relevant textbooks and online resources provided for further study.

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Description

Test your understanding of the properties and behaviors of acids and bases in chemistry. This quiz will cover topics such as the Lewis definition, Arrhenius and Brønsted-Lowry theories, and reactions involving various substances. Perfect for students enrolled in CHEM 1820.

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