Chemical Reactions Problem Set

1. Titration/acid base problem. 0.4563 g of Mg(OH)₂ is weighed out and disolved in 50.00 mL of H₂O. This is titrated against a solution of HNO₃. The initial volume of the burette is 2.35 ml. The final volume of the burette is 47.98 ml. What can you determine?

2. Acid Base equations and reactions. A base solution is made by disolving 4.987 g of Potassium Hydroxide in 500.0 ml of water. 36.84 ml of this base solution is used to titrate 25.00 ml of sulfuric acid. Write the total, total ionic, and net ionic equations for these reactions. What can you calculate from this information? What are your results?

3. When the following solutions are mixed, does a precipitate form? Write out the total, total ionic, and net ionic equations.
   1. silver nitrate and rubidium chloride
   2. lead nitrate and potassium chloride
   3. mercury (I) nitrate and hydrochloric acid
   4. calcium chloride and sodium carbonate
   5. magnesium nitrate and calcium chloride
   6. potassium sulfate and barium chloride

4. Precipitation Reactions and Solubility.
   1. Step 1: 0.8765 g of silver (I) nitrate is placed in a 250 mL volumetric flask diluted to the mark with deionized water. Determine the concentration of each ion in solution.
   2. Step 2: 1.8793 g of potassium chloride is placed in a 250 mL volumetric flask diluted to the mark with deionized water. Determine the concentration of each ion in solution.
   3. Step 3: 50.0 mL of the silver (I) nitrate solution and 50.0 mL of the potassium chloride solution are mixed together in an erlenmyer flask. Determine the mass of any precipitate formed and the concentration of each ion in solution.

Scott Van Bramer
Department of Chemistry
Widener University
Chester, PA 19013

© copyright 1996, S.E. Van Bramer
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Last Updated: Friday, November 03, 2000 10:29:05 AM