Chapter 16 Acids and Bases John D. Bookstaver St. Charles Community College Cottleville, MO Chemistry, The Central Science , 11th edition Theodore L. Brown, H. Eugene LeMay, Jr., and Bruce E. Bursten

Calculating K a from pH Now we can set up a table… 4.2 10 -3 4.2 10 -3 0.10 – 4.2 10 -3 = 0.0958 = 0.10 At Equilibrium + 4.2 10 -3 + 4.2 10 -3 – 4.2 10 -3 Change 0 0 0.10 Initially [HCOO – ], M [H 3 O + ], M [HCOOH], M

Calculating K a from pH = 1.8 10 -4 [4.2 10 -3 ] [4.2 10 -3 ] [0.10] K a =

Calculating pH from K a We next set up a table… We are assuming that x will be very small compared to 0.30 and can, therefore, be ignored. x x 0.30 – x 0.30 At Equilibrium +x +x -x Change 0 0 0.30 Initially [C 2 H 3 O 2 – ], M [H 3 O + ], M [C 2 H 3 O 2 ], M

pH of Basic Solutions Tabulate the data. x x 0.15 – x 0.15 At Equilibrium 0 0 0.15 Initially [OH – ], M [NH 4 + ], M [NH 3 ], M

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