Acids and Bases Concepts Quiz
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Questions and Answers

According to the Arrhenius definition, what is an acid in aqueous solution?

  • A substance that produces hydroxide ions
  • A substance that increases the concentration of hydronium ions (correct)
  • A substance that forms electron pairs
  • A substance that acts as a proton donor

What is a limitation of the Arrhenius concept of acids and bases?

  • It requires the presence of water to be effective (correct)
  • It can only define acids and bases in solid form
  • It does not account for electron sharing
  • It defines bases only in terms of their acidic properties

Under the Bronsted-Lowry theory, how is an acid defined?

  • As a substance that releases hydroxide ions
  • As a substance that accepts protons
  • As a Lewis acid
  • As a proton donor (correct)

What characterizes a Lewis acid according to the Lewis definition?

<p>It is electron deficient (A)</p> Signup and view all the answers

Which of the following substances can act as a Lewis acid?

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

Which of the following best describes a base in the Arrhenius theory?

<p>A substance that produces hydroxide ions in water (C)</p> Signup and view all the answers

What is a common example of a protocol chemical that does not fit under the Arrhenius definition?

<p>Dry hydrochloric acid (HCl) (A)</p> Signup and view all the answers

Which statement is true regarding the relationship between Bronsted-Lowry and Lewis theories?

<p>All Bronsted-Lowry acids are Lewis acids (A)</p> Signup and view all the answers

What role does ammonia (NH3) play when it reacts with hydrochloric acid (HCl)?

<p>Lewis base (B)</p> Signup and view all the answers

In the reaction of sodium oxide (Na2O) with sulfur trioxide (SO3), which species is the Lewis acid?

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

What limitation is associated with the Lewis concept regarding acid-base reactions?

<p>It does not address the behavior of protonic acids like HCl. (D)</p> Signup and view all the answers

When classifying acids, which characteristic defines strong acids?

<p>Completely ionized in water (B)</p> Signup and view all the answers

What factors influence the strength of a nonmetal hydride (HX) acid?

<p>Electronegativity of the central nonmetal and X–H bond strength (B)</p> Signup and view all the answers

Which of the following statements about Lewis acids is correct?

<p>Lewis acids accept electron pairs. (B)</p> Signup and view all the answers

Which molecule acts as a Lewis base in the reaction between ammonia (NH3) and boron trifluoride (BF3)?

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

Which of the following statements accurately describes weak acids?

<p>They are partially ionized in water. (B)</p> Signup and view all the answers

In the Brønsted–Lowry concept, what distinguishes an acid from a base?

<p>An acid donates a proton, while a base accepts a proton. (A)</p> Signup and view all the answers

Which reaction demonstrates the concept of a conjugate acid-base pair?

<p>NH3 and NH4+ (C)</p> Signup and view all the answers

In the reaction of HCl and NH3 in benzene, which species acts as the acid?

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

In the reaction of NH3 with H2O, which species is the base in the forward reaction?

<p>NH3 (A)</p> Signup and view all the answers

What is a limitation of the Brønsted–Lowry concept?

<p>It cannot explain reactions in non-protonic solvents. (A)</p> Signup and view all the answers

What is the correct representation of proton transfer in the reaction of H3O+ with NH3?

<p>H3O+ donates a proton to NH3. (C)</p> Signup and view all the answers

What role does OH− play in the reverse reaction of NH4+ with OH−?

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

Which of the following statements is true regarding proton transfer reactions?

<p>They involve the transfer of protons between substances. (A)</p> Signup and view all the answers

What is formed as a product in the neutralization reaction between an acid and a base?

<p>Salt (C), Water (D)</p> Signup and view all the answers

Which of the following is an example of an acidic salt?

<p>NaHSO4 (D)</p> Signup and view all the answers

What type of salt results from the partial neutralization of a strong base with a weak acid?

<p>Basic salt (B)</p> Signup and view all the answers

What is a key characteristic of double salts?

<p>Formed by combining two different salts (D)</p> Signup and view all the answers

Which property of salt can vary, resulting in different tastes?

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

What is the boiling point of sodium chloride?

<p>1,464 degrees Celsius (B)</p> Signup and view all the answers

What process describes the reaction of salt with water?

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

Which of the following is a characteristic of mixed salts?

<p>They consist of fixed proportions of two salts (A)</p> Signup and view all the answers

What primarily determines the trend of acid strength across a period?

<p>The electronegativity of the nonmetal X (B)</p> Signup and view all the answers

How does acid strength change down a group?

<p>Acid strength increases due to weaker bonds (A)</p> Signup and view all the answers

Which of the following compounds is an example of a strong base?

<p>NaOH (B)</p> Signup and view all the answers

What is formed as a result of an acid-base neutralization reaction?

<p>Water and a salt (B)</p> Signup and view all the answers

In the reaction between hydrochloric acid and sodium hydroxide, what is the net ionic equation?

<p>H+(aq) + OH−(aq) → H2O(l) (A)</p> Signup and view all the answers

What does the term 'salt' refer to in chemistry?

<p>An ionic compound that contains a cation from a base and an anion from an acid (A)</p> Signup and view all the answers

What is the effect of increased electronegativity on the X—H bond?

<p>It weakens the bond (C)</p> Signup and view all the answers

What distinguishes a strong acid from a weak acid?

<p>The ability to dissociate completely in solution (D)</p> Signup and view all the answers

What type of salt is formed by the neutralisation of a strong acid and a strong base?

<p>Neutral salt (C)</p> Signup and view all the answers

What characterizes the salts formed from weak acids and strong bases?

<p>They are basic in nature. (A)</p> Signup and view all the answers

What occurs during the hydrolysis of a salt formed from a strong acid and a weak base?

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

In which category would the salt NH4Cl fall?

<p>Acidic salt (C)</p> Signup and view all the answers

Which ion is produced when CH3COONa undergoes hydrolysis?

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

What defines a neutral salt in terms of ionization in solution?

<p>It does not hydrolyze. (D)</p> Signup and view all the answers

What is the effect of combining a weak acid with a weak base?

<p>Can produce either acidic, basic, or neutral salts. (C)</p> Signup and view all the answers

Which of the following salts would be classified as basic?

<p>CH3COONa (D)</p> Signup and view all the answers

Flashcards

Arrhenius acid

A substance that increases the concentration of hydronium ions (H3O+) when dissolved in water.

Arrhenius base

A substance that increases the concentration of hydroxide ions (OH−) when dissolved in water.

Brønsted-Lowry acid

A proton donor.

Brønsted-Lowry base

A proton acceptor.

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Lewis acid

A molecule or ion capable of coordinating with unshared electron pairs.

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Lewis base

A molecule or ion having unshared electron pairs available for sharing with acids.

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Acid-base reaction (general)

A reaction where an acid donates a proton to a base.

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Limitations of Arrhenius theory

Doesn't apply to non-aqueous solutions, and can't fully explain the acidity/basicity of certain substances like AlCl3.

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Lewis Acid

A substance that can accept a pair of electrons to form a covalent bond.

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Lewis Base

A substance that can donate a pair of electrons to form a covalent bond.

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Lewis Acid-Base Reaction

A reaction in which an electron pair is transferred from a Lewis base to a Lewis acid.

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Strong Acid

An acid that completely ionizes in water.

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Weak Acid

An acid that only partially ionizes in water.

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Acid Strength

The ability of an acid to donate a proton.

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Acid Strength, Factors

Electronegativity and bond strength of the X-H bond determine the ease of proton release.

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Limitations of Lewis Concept

Doesn't easily quantify the relative strengths of acids and bases; doesn't apply to all acid-base reactions.

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Brønsted-Lowry Acid

A substance that donates a proton (H+).

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Brønsted-Lowry Base

A substance that accepts a proton (H+).

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Conjugate Acid-Base Pair

Two species in an acid-base reaction that differ by one proton (H+).

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Conjugate Acid

The species formed when a base gains a proton.

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Conjugate Base

The species formed when an acid loses a proton.

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Proton Transfer Reaction

A chemical reaction in which a proton (H+) moves from one molecule or ion to another.

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Limitations of Brønsted-Lowry Theory

It does not apply to reactions in non-protonic solvents and cannot explain reactions involving acidic and basic oxides in the absence of a solvent.

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Non-protonic solvent

A solvent that is not capable of donating or accepting protons.

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Acid Strength Across a Period

Acid strength increases from left to right across a period due to increasing electronegativity of the nonmetal. More electronegative nonmetals pull electrons away from the hydrogen atom, making the hydrogen ion (H+) easier to release.

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Acid Strength Down a Group

Acid strength increases as you go down a group in the periodic table because the X-H bond weakens and becomes longer, making the hydrogen ion (H+) easier to lose.

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Strong Base

A strong base completely dissociates (separates into ions) in solution, releasing hydroxide ions (OH-).

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Neutralization Reaction

A reaction between an acid and a base that produces water and a salt.

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Salt in Chemistry

An ionic compound; it's formed from the combination of a cation (positive ion) and an anion (negative ion).

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Acid-base reaction (general)

A specific type of chemical reaction between an acid and a base that leads to the formation of water and a salt. The general reaction equation typically implies the ionic form of the acid participating in an aqueous environment.

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Hydride Acid Strength Trend

Acid strength of hydrides increases from Group 6A (16) to 7A (17).

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Neutralization Reaction Equation

The net ionic equation for most neutralization reactions is: H+(aq) + OH−(aq) →H2O(l).

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Salt Definition

An ionic compound with a cation other than H+ and an anion other than OH−, formed by the neutralization reaction of an acid and a base.

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Acidic Salt

A salt formed by partial neutralization of a diprotic or polyprotic acid, containing ionizable H+ along with another cation.

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Basic Salt

A salt formed by partial neutralization of a strong base by a weak acid which, upon hydrolysis, forms a basic solution.

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Double Salt

A salt containing more than one cation or anion, formed by the combination of two different salts crystallized in the same ionic lattice.

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Mixed Salt

A salt containing a fixed ratio of two salts, with either a common cation or a common anion

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Salt Properties: Color

Typically colorless, transparent, or white.

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Salt Properties: Taste

Can have various tastes, like salty, sour, sweet, bitter, savoury(umami).

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Saltwater Conductivity

Saltwater is a good conductor of electricity due to the presence of ions.

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Hydrolysis of Salts

The interaction between cations or anions of salts and water, often resulting in the regeneration of acids and bases.

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Neutral Salts

Salts formed from strong acid and strong base; they generally do not hydrolyze and have a neutral pH.

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Acidic Salts

Salts formed from strong acid and weak base; they tend to produce acidic solutions.

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Basic Salts

Salts formed from weak acid and strong base; they generally produce basic solutions.

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Salt of weak acid and strong base

These salts hydrolyze in water, resulting in an increase in hydroxide ion concentration, making the solution alkaline.

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Salt of strong acid and weak base

These salts hydrolyze in water, resulting in an increase in hydronium ion concentration, making the solution acidic.

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pH of solution

A measure of the concentration of hydrogen ions (H+) in a solution.

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Salts of Weak Acid and Weak Base

Their pH depends on the relative strengths of the acid and base that form them. It may be acidic, basic, or neutral.

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Study Notes

Acids and Bases

  • Arrhenius definition: acids produce hydrogen ions (H+), bases produce hydroxide ions (OH−)
  • Lowry-Brønsted definition: acids are proton donors, bases are proton acceptors
  • Lewis definition: acids are electron pair acceptors, bases are electron pair donors
  • Three different theories: Arrhenius, Brønsted-Lowry, and Lewis
  • Arrhenius concept: an acid increases the concentration of hydronium ions (H3O+) when dissolved in water; a base increases the concentration of hydroxide ions (OH−) when dissolved in water
  • Limitations of Arrhenius concept: requires water, doesn't explain non-aqueous solutions, doesn't explain acidic character of some salts
  • Brønsted-Lowry concept: acid-base reactions are proton-transfer reactions; an acid donates a proton, a base accepts a proton
  • Conjugate acid-base pairs: differ by one proton (e.g., NH3 and NH4+)
  • Limitations of Brønsted-Lowry: doesn't explain reactions in non-protonic solvents (e.g., SO2, N2O4)

Lewis Concept

  • Lewis acid: accepts an electron pair
  • Lewis base: donates an electron pair
  • Lewis concept is more general; applies to a wider range of reactions
  • Limitations of Lewis concept: doesn't offer a way to compare acid/base strength

Acid and Base Strength

  • Factors that affect acid strengths: electronegativity of the central atom, strength of the X-H bond
  • Factors that affect acid strengths (oxoacids): electronegativity of the central non-metal, number of oxygen atoms
  • Hydrohalic acid strength increases down the group
  • Strong acids completely ionize in water; weak acids do not
  • Strong bases completely dissociate in solution

Neutralization Reactions

  • Water and a salt are produced
  • General reaction: acid + base → water + salt

Salts

  • Salts are ionic compounds
  • Types of salts:
  • Acidic salt: formed by partial neutralization of a diprotic or a polyprotic acid; contains ionizable hydrogens
  • Basic salt: formed by partial neutralization of a strong base by a weak acid
  • Double salt: contains more than one cation or anion
  • Mixed salt: fixed proportion of two salts; share a common cation or common anion
  • Properties of salts: colour, taste, odour

Hydrolysis of Salts

  • Hydrolysis: reaction of a salt with water
  • Types of hydrolysis:
    • Acidic hydrolysis: salt of strong acid, weak base is acidic
    • Basic hydrolysis: salt of weak acid, strong base is basic
    • Neutral hydrolysis: salt of strong acid, strong base is neutral

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Description

Test your understanding of the different definitions and theories of acids and bases. This quiz covers Arrhenius, Brønsted-Lowry, and Lewis theories along with their limitations. Challenge yourself on conjugate acid-base pairs and more!

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