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Acid-Base Reactions, Oxidation-Reduction Reactions, and Water

Directions: Respond to the questions below.

  1. Balance the following equations: 
    1. HBr(aq) + Ca(OH)2(aq) —>
    2. HNO3(aq) + Al(OH)3(aq) —>
  2. How many moles of KOH are dissolved in 125 mL of 0.500 M KOH?
  3. The pH of tap water can vary widely.  The pH of one sample collected in Springfield, Ohio was found to be 8.2. 
    1. Is this sample of tap water acidic or basic?
    2. What is the concentration of hydronium in the sample?
    3. What is the concentration of OH– in the sample?
    4. The bedrock in Springfield, Ohio is composed mainly of limestone (CaCO3).  How might this account for the pH value that was observed?
  4. How many milliliters of 0.50 M HBr are needed to neutralize 0.045 moles of LiOH?
  5. One of the chemical reactions that takes place when bleach and ammonia are combined is shown here: NaOCl + NH3 —> NaONH3 + Cl2
    1. Which reactant undergoes oxidation?
    2. Which reactant undergoes reduction?
    3. Which reactant acts as the oxidizing agent?
    4. Is this chemical equation balanced?  If not, balance it.
  6. Describe how combustion and oxidation differ.
  7. Oxygen in the air reacting with substances in food can cause spoilage.  Why are antioxidants added to food?
  8. Both surface water and groundwater (natural waters) often contain dissolved ions.  Name three positive and three negative ions that are often found in natural waters.
  9. Determine the amount of heat required to convert 14.0 g of ice at 0°C to 14.0 g of liquid water at 50°C.
  10. What is the difference between “biodegradable” and “nonbiodegradable”?  If you had a choice between using a biodegradable and a nonbiodegradable detergent to clean your clothes, which would you choose?

 
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