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AP Chemistry Chapter 17 Outline
1. Chapter 17 Additional Aspects of Aqueous Equilibria Chemistry, The Central Science , 11th edition Theodore L. Brown; H. Eugene LeMay, Jr.; and Bruce E. Bursten John D. Bookstaver St. Charles Community College Cottleville, MO
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5. The Common-Ion Effect Because HCl, a strong acid, is also present, the initial [H 3 O + ] is not 0, but rather 0.10 M . x 0.10 + x 0.10 0.20 − x 0.20 At Equilibrium + x + x − x Change 0 0.10 0.20 Initially [F − ], M [H 3 O + ], M [HF], M HF ( aq ) + H 2 O ( l ) H 3 O + ( aq ) + F − ( aq )
21. Calculating pH Changes in Buffers The 0.020 mol NaOH will react with 0.020 mol of the acetic acid: HC 2 H 3 O 2 ( aq ) + OH − ( aq ) C 2 H 3 O 2 − ( aq ) + H 2 O ( l ) 0.000 mol 0.320 mol 0.280 mol After reaction 0.020 mol 0.300 mol 0.300 mol Before reaction OH − C 2 H 3 O 2 − HC 2 H 3 O 2
22. Calculating pH Changes in Buffers Now use the Henderson – Hasselbalch equation to calculate the new pH: pH = 4.74 + 0.06 pH pH = 4.80 pH = 4.74 + log (0.320) (0.200)
![The Common-Ion Effect ,[object Object],[object Object],CH 3 COOH ( aq ) + H 2 O ( l ) H 3 O + ( aq ) + CH 3 COO − ( aq)](data:image/gif;base64,R0lGODlhAQABAIAAAAAAAP///yH5BAEAAAAALAAAAAABAAEAAAIBRAA7)