Answered: 12) A 100.0 mL sample of 0.180 M HClO 4…

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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12) A 100.0 mL sample of 0.180 M HClO 4

is titrated with 0.270 M LiOH. Determine the pH of the solution

after the addition of 75.0 mL of LiOH.

13) A 100.0 mL sample of 0.20 M HF is titrated with 0.10 M KOH. Determine the pH of the solution before the

addition of any KOH. The K aof HF is 3.5 × 10-4.

14) A 100.0 mL sample of 0.10 M NH3 is titrated with 0.10 M HNO3. Determine the pH of the solution after the addition of 150.0 mL of HNO3. The Kb of NH3 is 1.8 × 10-5.

15) A 100.0 mL sample of 0.10 M NH3 is titrated with 0.10 M HNO3. Determine the pH of the solution after the addition of 200.0 mL of HNO3. The Kb of NH3 is 1.8 × 10-5.

16) A 100.0 mL sample of 0.10 M Ca(OH)2

is titrated with 0.10 M HBr. Determine the pH of the solution after

the addition of 200.0 mL HBr.

17) A 100.0 mL sample of 0.10 M Ca(OH)2

is titrated with 0.10 M HBr. Determine the pH of the solution after

the addition of 300.0 mL HBr.

18) A 100.0 mL sample of 0.20 M HF is titrated with 0.10 M KOH. Determine the pH of the solution after the

addition of 400.0 mL of KOH. The Ka

of HF is 3.5 × 10-4.

19) A 100.0 mL sample of 0.10 M NH3 is titrated with 0.10 M HNO3. Determine the pH of the solution after

the addition of 100.0 mL of HNO3. The Kb of NH3 is 1.8 × 10-5.

20) Calculate the percent ionization of nitrous acid in a solution that is 0.205 M in nitrous acid

and 0.295 M in potassium nitrite (

). The acid dissociation constant of nitrous acid is

21) Calculate the percent ionization of nitrous acid in a solution that is 0.169 M in nitrous acid. The acid dissociation constant of nitrous acid is 4.50 × 10-4.

22) What is the pH of a solution prepared by mixing 25.00 mL of 0.10 M CH3CO2H with 25.00 mL of 0.040 M CH3CO2Na? Assume that the volume of the solutions are additive and that

Ka= 1.8 × 10-5 for CH3 CO2H.

23) What is the pH of a solution prepared by mixing 50.00 mL of 0.10 M NH3 with 10.00 mL of 0.10 M NH4Cl? Assume that the volume of the solutions are additive and that Kb= 1.8 × 10-5 for NH3.

24) What is the pH of a solution prepared by mixing 100.00 mL of 0.020 M Ca(OH) 2 with 50.00 mL of 0.100 M NaOH? Assume that the volumes are additive.

25) What is the hydronium ion concentration in a solution prepared by mixing 50.00 mL of 0.10 M HCN with 50.00 mL of

NaCN? Assume that the volumes of the solutions are additive and that Ka=

26) You wish to prepare an HC2H3O2 buffer with a pH of 4.14. If the pKa of is 4.74, what ratio of C2H3O2-/HC2H3O2 must you use

28) A buffer solution is 0.100 M in both HC7

H5O2 and NaC7H5O2 and has a pH of 4.19. Which of the

following pH values would you expect from the addition of a small amount of a dilute solution of a strong base?

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