) 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.
) 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.
Chemistry: An Atoms First Approach
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Author:Steven S. Zumdahl, Susan A. Zumdahl
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Chapter14: Acid- Base Equilibria
Section: Chapter Questions
Problem 97AE: A student intends to titrate a solution of a weak monoprotic acid with a sodium hydroxide solution...
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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=4.9*10^-10 for HCN
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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