Characteristics of Acids and Bases
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Questions and Answers

What are the characteristics of acids?

  • Slippery
  • Sour (correct)
  • pH less than 7 (correct)
  • Bitter

    • What are the characteristics of bases?

  • Sour
  • Bitter (correct)
  • Squeaky
  • pH greater than 7 (correct)

    • What is HCl?

    Hydrochloric acid

    What is HC2H3O2?

    <p>Acetic acid</p> Signup and view all the answers

    What is H2SO4?

    <p>Sulfuric acid</p> Signup and view all the answers

    What is HNO2?

    <p>Nitrous acid</p> Signup and view all the answers

    What is HNO3?

    <p>Nitrate</p> Signup and view all the answers

    What is H3PO4?

    <p>Phosphoric acid</p> Signup and view all the answers

    What is HBr?

    <p>Hydrobromic acid</p> Signup and view all the answers

    What is H2SO3?

    <p>Sulfurous acid</p> Signup and view all the answers

    What does the suffix 'ate-', 'ite', 'ide-' correspond to?

    <p>IC</p> Signup and view all the answers

    What are the products of the self-ionization of water?

    <p>OH- and H3O+</p> Signup and view all the answers

    What is the degree or amount of ionization for a strong acid?

    <p>Strong, complete ionization (100%)</p> Signup and view all the answers

    Are strong acids/bases strong or weak electrolytes?

    <p>True</p> Signup and view all the answers

    Classify the following: KOH, Ca(OH)2, HCl, H2SO4, NH3, HC2H3O2.

    <p>Strong; Strong; Strong; Strong; Weak; Weak</p> Signup and view all the answers

    What does the Arrhenius Theory state?

    <p>An acid gives an H+ and a base gives OH-; acids start with H, bases end with OH.</p> Signup and view all the answers

    What is the Bronsted-Lowry definition of acids and bases?

    <p>Acid is a proton H+ donor; Base is a proton H+ acceptor.</p> Signup and view all the answers

    In the reaction HCl + H2O, what is the acid and its conjugate base?

    <p>HCl is the acid; Cl- is the conjugate base.</p> Signup and view all the answers

    In the reaction HCl + H2O, what is the base and its conjugate acid?

    <p>H2O is the base; H3O+ is the conjugate acid.</p> Signup and view all the answers

    Differentiate between strong vs. weak and concentrated vs. dilute solutions.

    <p>Both A and B</p> Signup and view all the answers

    What is a Lewis acid?

    <p>An electron pair acceptor</p> Signup and view all the answers

    What is a Lewis base?

    <p>An electron pair donor</p> Signup and view all the answers

    What is a neutralization reaction?

    <p>Acid + Base = Salt + Water</p> Signup and view all the answers

    What type of reaction involves an acid-base titration?

    <p>Neutralization</p> Signup and view all the answers

    What indicates an acidic solution?

    <p>Greater concentration of hydrogen ions than water</p> Signup and view all the answers

    What indicates an alkaline solution?

    <p>Aqueous solution having a pH greater than 7 or having a [OH-] greater than $10^{-7}$.</p> Signup and view all the answers

    What is pH?

    <p>Measure of the acidity or basicity of an aqueous solution.</p> Signup and view all the answers

    What relative to hydroxide determines a solution's pH?

    <p>Hydronium ion</p> Signup and view all the answers

    What is a hydroxide ion?

    <p>A particle with a negative one (-1) charge that has two atoms: one oxygen and one hydrogen atom.</p> Signup and view all the answers

    What is amphoteric?

    <p>Able to react both as a base and as an acid.</p> Signup and view all the answers

    What is a neutralization reaction?

    <p>A chemical reaction where a base and an acid react to form a salt.</p> Signup and view all the answers

    What is titration?

    <p>The slow addition of one solution of a known concentration to another of unknown concentration until neutralization is reached.</p> Signup and view all the answers

    What changes color in acidic and basic solutions?

    <p>Phenolphthalein</p> Signup and view all the answers

    When acids react with active metals, what gas is released?

    <p>H2</p> Signup and view all the answers

    In a neutral solution, what equals $1.0 imes 10^{-7}$?

    <p>H+ and OH-</p> Signup and view all the answers

    Study Notes

    Characteristics of Acids and Bases

    • Acids: sour taste, pH less than 7, conduct electricity, have a squeaky feel.
    • Bases: bitter taste, pH greater than 7, conduct electricity, feel slippery.

    Common Acids

    • HCl: Hydrochloric acid, commonly found in stomach acid.
    • HC2H3O2: Acetic acid, a component of vinegar.
    • H2SO4: Sulfuric acid, used in batteries and industrial processes.
    • HNO2: Nitrous acid, often used in food preservation.
    • HNO3: Nitric acid, a strong oxidizing agent.
    • H3PO4: Phosphoric acid, used in fertilizers and food flavoring.
    • HBr: Hydrobromic acid, used in metal processing.
    • H2SO3: Sulfurous acid, formed when sulfur dioxide dissolves in water.

    Ionization and Electrolytes

    • Self-ionization of water produces hydroxide ions (OH⁻) and hydronium ions (H₃O⁺).
    • Strong acids/bases fully ionize in solution, categorized as strong electrolytes.
    • Weak acids/bases partially ionize in solution and are weak electrolytes.

    Acid-Base Theories

    • Arrhenius Theory: Acids release H⁺, bases release OH⁻; acids start with H, bases end with OH.
    • Brønsted-Lowry Theory: Acids are proton donors (H⁺), bases are proton acceptors.

    Acid-Base Reactions

    • Neutralization reaction: An acid reacts with a base to form salt and water.
    • Acid-base titration: A process of slowly adding a known concentration of titrant to a solution of unknown concentration until neutralization, typically indicated by color change.

    Solution Properties

    • Acidic solutions have a greater concentration of hydrogen ions than water.
    • Alkaline solutions have a pH greater than 7 or a hydroxide ion concentration greater than 10⁻⁷.
    • pH measures acidity or basicity of an aqueous solution.
    • Hydronium ion concentration relative to hydroxide ion determines solution pH.

    Important Ions

    • Hydroxide ion (OH⁻): Composed of one oxygen and one hydrogen atom, negatively charged.
    • Amphoteric substances can react as both acids and bases.

    Indicators and Reactions

    • Phenolphthalein is an acid-base indicator, turning colorless in acidic solutions and pink in basic.
    • When acids react with active metals, hydrogen gas (H₂) is released.

    Neutrality and Properties

    • In a neutral solution, H⁺ concentration equals OH⁻ concentration, both at 1.0 x 10⁻⁷ M.

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    Description

    This quiz covers the essential characteristics of acids and bases, including their definitions and common examples like hydrochloric and sulfuric acids. It is designed to help students understand the basic properties of these important chemical compounds.

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