Name Haley oyle 20yle Sec. QUESTIONS 1. Why must the Erlenmyer flask and graduated cylinder be dried in an oven before the reaction is run? a. Write an equation showing why the crude aspirin dissolves in the saturated NaHCO3 solution. b. Write an equation showing why the aspirin precipitates from when HCl is added to the saturated NaHCO3 solution.

2. Do the following calculations:a) Calculate the experimental % hydrolysis for 1 M NaC2H3O2 and 1 M Na2CO3 .(experimental means you can only use your measurements- do not look up any K values)b) Calculate the theoretical % hydrolysis for 1 M NaC2H3O2 and 1 M Na2CO3(these are done using published K values)c) Calculate % error or % difference between experimental and theoretical % hydrolysis values.  Data: Part 1 1M of: NaCH3CO2 ph=8.79 NaCl ph = 6.89 NH4Cl ph=5.06 NH4CH3CO2 ph = 6.90 Na2CO3 ph=11.82 Part 2 NH4Cl(s) - smell weak NH4CH3CO2 (s)- smell medium (NH4)2CO3(s)- smell strong Part 3 0.1 M NaH2PO4 ph=8.56 0.1 M Na2HPO4 ph=4.65 Part 4 2g of Al2(SO4) (s) + 10 ml H2O (50 ml beaker) ph = 7.96 2g NaHCO3(s) + 10 ml H2O (50 ml beaker) ph = 3.07

Please don't provide handwrittin solution...

This series demonstrates a progression as 0.5 M solution of sodium carbonate (?? ?? ) as it is added drop-by-drop to a test tube containing 0.2 M solution of lead (II) nitrate (??(?? ) ) 1. What observations indicate that a chemical reaction has occurred? 2. Break up the reactants into ions. Switch the cations. Use the “criss-cross” method to get the balanced formulas for the products. Write the balanced molecular equation for this reaction, including phase labels. 3. Write the complete ionic equation for this reaction. 4. Write the net ionic equation for this reaction. 5. What is the precipitate?