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 (A), OUS (B), HYDRO-IC (C)</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 (A)</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 (A)</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

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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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