Skip to main content
Chemistry LibreTexts

4.E: Types of Chemical Reactions

  1. Classify each of the following substances as: 1) acid, base, or neutral, and 2) strong or weak. Then 3) write a balanced equation for the ionization of the substance in water:
  1. \(\ce{HNO3}\)
  2. \(\ce{HClO}\)
  3. \(\ce{NH3}\)
  4. \(\ce{NaNO3}\)
  5. \(\ce{Ba(OH)2}\)

 

  1. A common method of preparing solutions is to make up a concentrated solution and then dilute it to the desired concentration.
  1. What is the molarity of a solution prepared by dissolving 29.2 g \(\ce{NaCl}\) in enough water to make 0.250 liters of solution?
  2. What volume of the above solution is needed to make 125 ml of a 0.350 M \(\ce{NaCl}\) solution?

 

  1. What mass of glucose (\(\ce{C6H12O6}\)) is needed to prepare 200.0 ml of a 2.50 M glucose solution?

 

  1. Solid magnesium is added to 125 ml of 2.00 M hydrochloric acid to produce dissolved magnesium chloride and hydrogen gas.
  1. Write a balanced equation for this reaction.
  2. If excess magnesium is added, how many moles of hydrogen gas are produced?

 

  1. Indicate whether a precipitate will form when the following solutions are mixed.  If a precipitate forms, write a net ionic equation for the reaction.
  1. iron(III) nitrate and potassium hydroxide
  2. ammonium chloride and lithium carbonate
  3. sodium sulfide and nickel(II) sulfate

 

  1. Name two solutions which could be mixed to form strontium sulfate.

 

  1. Write a balanced net ionic equation for the acid-base reaction between \(\ce{HNO3}\) with \(\ce{KOH}\).

 

  1. How many ml of 2.00 M \(\ce{NaOH}\) would be required to neutralize 12.5 ml of 0.0800 M \(\ce{HBr}\)?

 

  1. When solutions of lead(II) nitrate and aluminum chloride are mixed, a precipitate forms.
  1. Write a balanced formula equation for the reaction.
  2. What volume of a 0.200 M lead(II) nitrate solution is needed to completely form a precipitate when added to 2.48 mL of 0.300 M aluminum chloride?
  3. What is the mass of precipitate formed in (b)?

 

  1. What mass of precipitate is formed when 71.3 mL of 0.500 M iron(III) nitrate are mixed with 112 mL of 0.800 M sodium carbonate?

 

  1. How many ml of 2.50 M \(\ce{HNO3}\) contain enough nitric acid to dissolve an old copper penny with a mass of 3.94 grams?

\(\mathrm{3Cu(s) + 8HNO_3(aq) \rightarrow 3Cu(NO_3)_2(aq) + 2NO(g) + 4H_2O}\)

Extra Questions

1.  When iron(III) chloride and sodium hydroxide are mixed a precipitate forms.

  1. Write a balanced formula equation for this reaction.
  2. What volume of 0.200 M iron(III) chloride is needed to completely precipitate the product when mixed with 30.0 mL of 0.500 M sodium hydroxide?
  3. What mass of precipitate is formed?

 

2.  What mass of precipitate is formed when 25.0 mL of 0.200 M silver nitrate are mixed with 10.0 mL of 0.150 M aluminum chloride?

 

3.  What volume of 0.0500 M Ba(OH)2 is needed to neutralize 25.0 mL of 0.300 M HNO3?

 

4.  How many grams of KCl are needed to make 50.0 mL of a 2.00 M KCl solution?

 

5.  What volume of 6.00 M HCl is needed to prepare 30.0 mL of a 0.500 M HCl solution?

 

6.  What mass of precipitate is formed when 40.0 mL of 0.250 M barium nitrate are mixed with excess potassium sulfite?