User:Melissa Novy/Notebook/CHEM-572/2013/03/27

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==Entry title==
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==Objectives==
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* Insert content here...
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* Calculate the amount of silver-loaded clay necessary to achieve theoretical leaching of 2.5 μmol Ag<sup>+</sup> in 50 mL of solution.
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  '''MW Ag<sup>+</sup>: 107.87 g/mol'''
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  '''MW AgNO<sub>3</sub>: 169.87 g/mol'''
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  '''Given that 3.662 μmol Ag<sup>+</sup> was exchanged into 1.49711 g LMT, (3.662 μmol Ag<sup>+</sup>)/(1.49711 g LMT) = (2.5 μmol Ag<sup>+</sup>)/(x g LMT)'''
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  '''x = 1.02206 g LMT'''
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* Therefore, 2.5 μmol Ag<sup>+</sup> is present in 1.02206 g of 100AgLMT.  The corresponding control film must be 3 g PLA2002D with 1.02206 g LMT.
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PLA2002D + 33wt% LMT
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* Actual mass PLA2002D: 3.03753 g
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* Actual mass LMT: 1.02205 g

Revision as of 13:02, 2 April 2013

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Objectives

  • Calculate the amount of silver-loaded clay necessary to achieve theoretical leaching of 2.5 μmol Ag+ in 50 mL of solution.
  MW Ag+: 107.87 g/mol
  MW AgNO3: 169.87 g/mol
  Given that 3.662 μmol Ag+ was exchanged into 1.49711 g LMT, (3.662 μmol Ag+)/(1.49711 g LMT) = (2.5 μmol Ag+)/(x g LMT)
  x = 1.02206 g LMT
  • Therefore, 2.5 μmol Ag+ is present in 1.02206 g of 100AgLMT. The corresponding control film must be 3 g PLA2002D with 1.02206 g LMT.

PLA2002D + 33wt% LMT

  • Actual mass PLA2002D: 3.03753 g
  • Actual mass LMT: 1.02205 g



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