Calculate the ph at the equivalence point for the

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10. Calculate the pH at the equivalence point for the following titration: 0.20 MHCl versus 0.20 Mmethylamine (CH3NH3; Kb= 4.4 × 10–4) (5 points)
11. A 25.0 mL solution of 0.100 MCH3COOH is titrated with a 0.200 MKOH solution. Calculate the pH after the following additions of the KOH solution: (a) 0.0 mL, (b) 5.0 mL, (c) 10.0 mL, (d) 12.5 mL, (e) 15.0 mL. (25 points)
(Reference: Chang 16.35)4Copyright © 2016 by Thomas Edison State University. All rights reserved.
12. Referring to the following table:IndicatorColor in AcidColor in BasepH Range*Thymol blueRedYellow1.2–2.8Bromophenol blueYellowBluish purple3.0–4.6Methyl orangeOrangeYellow3.1–4.4Methyl redRedYellow4.2–6.3Chlorophenol blueYellowRed4.8–6.4Bromothymol blueYellowBlue6.0–7.6Cresol redYellowRed7.2–8.8PhenolphthaleinColorlessReddish pink8.3–10.0*The pH range is defined as the range over which the indicator changes from the acid color to the base color.Specify which indicator or indicators you would use for the following titrations: (9 points)a.HCOOH versus NaOH
b.HCl versus KOHBromothymol bluec.HNO3versus CH3NH2
13. The pKaof butyric acid (HBut) is 4.7. Calculate Kbfor the butyrate ion (But). points)(5
5Copyright © 2016 by Thomas Edison State University. All rights reserved.
6Copyright © 2016 by Thomas Edison State University. All rights reserved.

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