Essential Concepts

  • Properties of Acids/Bases
  • Naming Acids/Bases
  • The pH Concept
  • Arrhenius/Brønsted-Lowry Definitions
  • Identifying Conjugate Acid-Base Pair
  • Identifying Strong Acids/Bases
  • Acid/Base Dissociation
  • Neutralization Reactions

Standard 29: Define acids and bases and distinguish between Arrhenius and Bronsted-Lowry definitions and predict products in acid base reactions that form water.

  1. Name the following acids/bases:

  1. H2SO3
  2. HF
  3. H3PO3
  4. HMnO4
  5. HClO3
  6. HCN

  1. Write the formulas of the following acids:

  1. dichromic acid
  2. hydroiodic acid
  3. nitrous acid
  4. hydrosulfuric acid
  5. phosphoric acid
  6. acetic acid
  1. According to the Bronsted-Lowry theory, what is an acid?
  2. What salt is formed when hydrochloric acid is neutralized by a potassium hydroxide solution?
  3. Which statement describes the characteristics of an Arrhenius base?
  4. It changes red litmus to blue and has a pH greater than 7
  5. It changes blue litmus to red and has a pH less than 7
  6. It changes blue litmus to red and has a pH greater than 7
  7. It changes red litmus to blue and has a pH less than 7
  8. In the reaction NH3 + HCl  NH4+ + Cl-

The NH3 acts as

  1. A Bronsted acid only
  2. Neither a Bronsted acid nor a Bronsted base
  3. A Bronsted base only
  4. Both a Bronsted acid and a Bronsted base
  1. When dissolved in water, an Arrhenius base yields
  2. Hydrogen ions
  3. Oxide ions
  4. Hydroxide ions
  5. Hydronium ions

Standard 30: Define pH and use the hydrogen or hydroxide ion concentrations to calculate the pH of a solution.

  1. What is [H+] when the hydroxide ion concentration is 3.58  10-9? Is this solution an acid or a base?
  2. What is the hydrogen ion concentration when the pH is 3.75?
  3. What is the pH of a solution with a H+ concentration of 4.51  10-3? Is this solution an acid or a base?
  4. What is the pH of a solution of 0.15 M HNO3?
  5. What is the pOH of a solution of 0.5 M HCl?
  6. What is the pOH of a solution of 0.12 M NaOH?
  7. What is the pH of a solution of 0.10 M Ba(OH)2?
  8. What is the pOH of a solution with a H+ concentration of 9.53  10-1 M?
  9. What is the hydroxide ion concentration when the pH is 9.25?
  10. What is the pOH of a solution with a H+ concentration of 1.20  10-4 M?
  11. What is the pH when the hydroxide ion concentration is 3.58  10-9 M? Is this solution an acid or a base?
  12. What is [OH-] when the pH is 12.54?

Standard 31: Distinguish between degrees of dissociation for strong and weak acids and bases.

  1. The diagrams below show three different compounds in solution. Which of these could be a strong acid?
  2. X only
  3. Y only
  4. X and Y only
  5. Y and Z only
  1. Which of the following dissociates/ionizes completely in aqueous solution?
  2. NH3
  3. Ca(OH)2
  4. CuOH
  5. Fe(OH)3
  1. Which of the following is a strong acid?
  2. HCN
  3. HF
  4. HClO4
  5. HClO

  1. Write the equation for dissociation of acetic acid in water.
  2. Write the equation for dissociation of ammonia in water.
  3. Write the equation for dissociation of nitric acid in water.
  4. Write the equation for dissociation of barium hydroxide in water.

Standard 32: Understand acid-base reactions

  1. Write the balanced neutralization reaction between sulfuric acid and lithium hydroxide. Name the salt that is formed as a product. Is the salt acidic, basic or neutral?
  2. Write the balance neutralization reaction between carbonic acid and barium hydroxide. Name the salt that is formed as a product. Is the salt acidic, basic, or neutral?
  3. A 12.4 mL solution of HClO4 is completely neutralized by 19.8 mL of 0.0100 M KOH. What is the concentration of the HClO4 solution?