week1 - solubility equilibrium is established. a. What is...

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Chemistry 114 week 1 worksheet Spring 2008 1. Write the balanced chemical equations for the solubility of each of the following and the solubility-product expressions (the equilibrium expressions) for: a. calcium chromate b. silver cyanide c. nickel (II) sulfide 2. The solubility of silver carbonate is 0.032 M at 20 ˚C. Calculate its K sp . [1.3 x 10 -4 ] 3. Which compound in each pair is more soluble in water? You will need to use a table of K sp values to answer this question. a. Barium sulfate or calcium sulfate b. Calcium phosphate or magnesium phosphate c. Silver chloride or lead (II) sulfate d. silver bromide or silver carbonate
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Chemistry 114 week 1 worksheet Spring 2008 4. Solid AgCl is placed into a flask and water is added. Assume enough solid is used that the
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Unformatted text preview: solubility equilibrium is established. a. What is the molar solubility of AgCl? b. More water is added to the flask. When the solubility equilibrium is reestablished, does the molar solubility change? Does the amount of solid AgCl left in the flask change? 5. Find the molar solubility of BaCrO 4 ( K sp = 2.1 x 10-10 ) in a. pure water [S = 1.4 x 10-5 M] b. 1.5 x 10-3 M Na 2 CrO 4 [S = 1.4 x 10-7 M] 6. Does any solid PbCl 2 form when 3.5 mg of NaCl is dissolved in .250 L of 0.12 M Pb(NO 3 ) 2 ? As you solve this problem, write out the reaction equation that is being examined. [no solid will form] 7. The solubility of calcium sulfate is 0.209 g per 100. mL solution at 20 C. Calculate its K sp . [2.36 x 10-4 .]...
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This note was uploaded on 04/07/2008 for the course CHEM 114 taught by Professor Jursich during the Spring '08 term at Ill. Chicago.

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week1 - solubility equilibrium is established. a. What is...

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