Fall 2020 CHM 1046L QUESTIONS


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Responses must be submitted to the dropbox no later than 5:00 pm (1700 hours), Wednesday 4 November 2020. Submissions received after this deadline will receive a score of zero. Submission not submitted to the dropbox will receive a score of zero. Responses must be typed except for figures, equations, etc. as necessary. All graphs should be generated using computer software of your choice. Responses must be collated and submitted as a single pdf file. Handwritten responses will receive a score of zero.




All questions are worth 10 points


  1. You are given 50.g of an unknown chloride containing white ionic solid that is water soluble. Assuming you have unlimited access to our laboratory, how would you go about identifying the unknown. Write a brief experimental protocol taking into account the amount of unknown that you have. Explain how you would expect your results to differentiate between aluminum chloride, potassium chloride, strontium chloride, and zinc chloride.


  1. When an aqueous solution of mercury(II) chloride is added to an aqueous solution of sodium oxalate, bubbles are formed (suggesting the formation of carbon dioxide gas) as well as a solid that settles out.


  1. Write a balanced chemical equation for this reaction. Hint – do not forget about spectator ions.
  2. Given the following data, determine the rate law for this reaction.













  mercury(II) sodium oxalate rate of  
Experiment disappearance  
chloride (M) (M)  
  of oxalate (M/s)  
1 0.164 0.15 3.2 x 10-5  
2 0.164 0.45 2.9 x 10-4  
3 0.082 0.45 1.4 x 10-4  
4 0.246 0.15 4.8 x 10-5  
  1. What is the reaction rate when the initial concentration of mercury (II) chloride is 0.100 M and that of sodium oxalate is 0.250 M if the temperature is the same as that used to obtain the data shown?




  1. A student performed the hydrolysis of ethyl ethanoate equilibrium experiment that was conducted in the laboratory with the following data and information:


Part A – Solution Preparation (Volumes added)


  Flask A Flask B Flask C
~3M HCl (mL) 5.00 5.00 5.00
ethyl ethanoate (mL) 5.00 4.00 3.00
water (mL) 0.00 1.00 2.00



Part B – Titrating 5.00 mL samples of ~3M HCl with 0.495 M Barium


Hydroxide Solution


    Trial 1 Trial 2 Trial 3 Trial 4 Trial 5
initial buret (mL) 0.04 17.01 1.25 16.21 0.76
final buret (mL) 17.01 31.99 16.21 31.18 15.75
  Part C – Titrating Flasks A-C with 0.495 M Barium  
    Hydroxide Solution    
      Flask A Flask B Flask C  
  initial buret (mL) 0.84 1.05 0.67  
  final buret (mL) 43.59 41.37 37.08  


















Barium Hydroxide used = 0.495M


Densities of Solutions Used


~3M HCl (g/mL) 1.05
ethyl ethanoate (g/mL) 0.893
water (g/mL) 1.00


Given the above data and information:


  1. Determine the actual concentration, standard deviation, and relative standard deviation, of hydrochloric acid used. Clearly indicate which trials were selected and why.


  1. Determine the equilibrium constant for each flask. Show calculations for at least one flask.


  1. Determine the average, standard deviation, and relative standard deviation of the equilibrium constant.


  1. How does this value compare to the experimental value you determined earlier this semester? How does it compare to the literature value? Explain.




  1. Write a balanced chemical equation for the reaction of hydrochloric acid with aqueous ammonia solution.


  1. Prepare a theoretical titration curve where 0.120 M hydrochloric acid is added in increments of 0.20 mL to 30.00 mL of 0.116 M ammonia solution.
  2. Clearly identify the equivalence point on your graph and how you determined that specific volume to be the equivalence point. What is the pH at this volume? Is this to be expected?


  1. Can you identify pKb from your graph? If so, clearly identify the pKb on your graph and how you determined that specific datapoint (volume, pH) to be pKb. If not, explain why you are unable to identify pKb from your graph.


  1. A student titrated 25.00 mL an unknown acid solution with 0.1021 M sodium hydroxide solution and generated the titration curve provided on the next page. The raw data is available upon request. Using the titration curve, please answer the following questions


  1. What type of acid is this?


  1. monoprotic, diprotic, etc.


  1. strong, weak


  1. Clearly identify the equivalence point(s).


  1. Clearly identify the pKa value(s).


  1. Clearly explain how you identified these values.


  1. What was the concentration of the unknown acid solution?






  1. Determine the identity of the unknown, and explain how you came to that conclusion, from the following list of acids:

adipic acid, benzoic acid, citric acid, maleic acid, palmitic acid,


salicylic acid, or tartaric acid (yes – you may need to look up information on each acid).




























































































pH as a function of volume of base added































0.00 10.00 20.00 30.00 40.00 50.00 60.00  
        volume of base added (mL)          


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