CHEM132TuesMar16

CHEM132TuesMar16 - Tuesday March 16 No CHEM132 SI on Wed....

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Tuesday March 16 No CHEM132 SI on Wed. March 17th Chapter 19 Ionic Equilib in Aq Soln today: buffer solutions - quantitatively, titrations Thursday: more titrations Tuesday March 23: ARIS due (19.1, 19.2 weak&strong bases, 19.2 weak&strong acids)
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3.50 M NH 4 Cl (aq) acidic, basic, neutral Cl is neutral – neglibible base NH4 is weak acid K a = 5.7 x 10 -10 , pH = ?? Ka =[NH3][H+] [NH4+] NH4+ NH3 + H+ I 3.5 0 0 C -x +x +x E 3.5-x ~3.5 x x
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NH 4 Cl / NH 3 buffer (NH 4 + K a = 5.7x10 -10 ) a.pH=pK a b.pH>pK a c.pH<pK a d.pH=7 e.pH<7 f.pH>7 What is pH of 100.0 mL of buffer: 0.50 M NH 4 3 0.50 M NH 4 3 ? (b) & (f)
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Determining the pH of a buffer 1. Account for any dilution or rxn with OH - or H + 1. Use K a or H-H equation to determine H + or pH. (assume negligible change to buffer parts)
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Two types of reactions Hydrolysis between weak acid (or weak base) & water to produce H + (or OH - )
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100. mL of
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CHEM132TuesMar16 - Tuesday March 16 No CHEM132 SI on Wed....

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