Acid-Base and Redox Reactions Test Review

Objectives:

In order to be successful on this test you must be able to:

  1. Give the name and/or formula of the following acids: hydrochloric acid, nitric acid, sulfuric acid, phosphoric acid, acetic acid.
  2. Identify an acid or base as strong or weak and use this information to discuss the electrolytic properties and their relative pH values.
  3. Identify an acid, base, or an acid-base reaction as following the Arrhenius definitions and/or Bronsted-Lowry definitions and explain why.
  4. Predict the products of an acid-base reaction using all appropriate symbols and balancing.
  5. Use basic knowledge of the pH scale to predict the pH of an acidic solution as pH<7 or basic solution with pH>7.
  6. Use the pH and pOH equations to calculate any of the following quantities from any starting point: pH, pOH, [H+], [OH-].
  7. Determine the oxidation number for every element in a given compound.
  8. If given a redox reaction, determine what elements are oxidized and reduced, as well as the oxidizing and reducing agents.
  9. If given a redox reaction, correctly split the reaction into two half reactions and then balance the reaction.
  10. Explain how the factors of temperature, concentration, and surface area affect the rate of a reaction based on Collision Theory.
  11. Explain what it means for a system to be in equilibrium in terms of
  12. Concentrations of products and reactants
  13. Rates of the forward and reverse reaction
  14. Observable changes in the system.

Practice Problems:

  1. What is the pH of a solution with a [H+] = 4.50x10-9M?
  1. What is the pOH of a solution with a [H+] = 3.91x10-6M?
  2. What is the [OH-] of a solution with a pOH = 5.35?
  3. What is the [OH-] of a solution with a pH = 11.29?

For each of the following, write the balanced reaction that occurs using all appropriate symbols and balancing the reaction using lowest whole number coefficients. If No Reaction occurs, simply write NR.

  1. Solutions of phosphoric acid and strontium hydroxide are mixed.
  2. A solution of acetic acid is added to solid copper(II) hydroxide

For the following reactions, identify the reactant acting as the acid and the reactant acting as the base.

  1. S2-+ 2H3O+H2S + 2H2O
  2. NH4++ H2ONH3+ H3O+
  3. Which of the following are Bronsted-Lowry bases but are NOT Arrhenius bases?

NH3, NaOH, Ca(OH)2, NaOCl, K2CO3, Fe(OH)3

For the following reactions, identify the elements oxidized and reduced, the species that is the oxidizing agent and reducing agent. Then balance the reaction.

  1. Hypochlorite ions react with sulfide ions in acidic conditions to form chloride ions and solid sulfur.
  2. Manganese(II) ions react with bismuthate ions(BiO3-) in acidic conditions to form bismuth(III) ions andpermanganate ions.