Acids and Bases

• Know the three definitions of acids and bases: Arrhenius, Bronsted-Lowry, and Lewis.
• Know the properties of acids and bases.
• Know how acids and bases react.
• Know the difference between strong and weak acids (and strong and weak bases).
• Be able to give at least one example of a strong acid, a strong base, a weak acid, and a weak base.
• Understand conjugate acids and bases.
• A conjugate acid is what is left over after a base acts like a base (i.e., after it has accepted or gained a proton).
• A conjugate base is what is left over after an acid acts like an acid (i.e., after it has donated or lost a proton).
• Be able to calculate the pH of any solution, given the concentration of acid or base. (Applies only to strong acids and strong bases.)
• Be able to calculate pH, pOH, [H+], or [OH-] for any solution where one of these variables is given.
• Understand neutralization.
• Understand titration and related calculations.

Practice problems: (Answers)

1. What is the pH, pOH, [H+], or [OH-] for a 0.00156 molar solution of hydrochloric acid?
2. What is the pH, pOH, [H+], or [OH-] for a 0.00156 molar solution of sodium hydroxide?
3. What is the pH, pOH, [H+], or [OH-] for a 0.00156 molar solution of sulfuric acid?
4. How many milliliters of 0.250 molar sodium hydroxide are required to reach the equivalence point in the titration of 15.00 milliliters of 0.512 molar hydrochloric acid?
5. How many milliliters of 0.250 molar potassium hydroxide are required to titrate 25.00 milliliters of 0.512 molar sulfuric acid to the equivalence point?