1. For each of the solutions in part 3, calculate an expected pH. The Ka for HC₂H3O2 is: 1.8 x 10⁹ and the Kb for NH3 is 1.76 x 105. Remember to account for the dilution factor. a. 10.0mL of 0.10 M HC₂H₂O₂ + 5.0mL of 0.10M HCI b. 10.0mL of 0.10M NH3 + 5.0mL of 0.10M NaOH c. 10.0mL of 0.10M HC₂H₂O₂ +10.0mL 0.10M NaC₂H₂O₂ d. 10.0mL of 0.10 M NH3 + 10.0mL of 0.10M NH.CI 2. Which solution(s) in question 1 would be considered a buffer solution? 3. Complete the calculation for K, from the earlier discussion of the amphoteric salt. Will this ion be acidic or basic? Predict the expected pH for the 0.050M solution. (1) H₂PO4 (aq) + H₂O → H₂O (aq) + HPO42(aq); K₁2 = 6.2 x 10-8 (2) H₂PO4 (aq) + H₂O → H₂PO4(aq) + OH(aq); Kb = = ??? Kw Kal 4. Similarly, the HPO4 ion is also amphoteric. The two possible reactions are: H₂O(aq) + PO4³(aq); Kas = 4.2 x 10-¹3 (1) HPO4 (aq) + H₂O) Kw = → H₂PO4 (aq) + OH(aq); Kb = = ??? K₂2 (2) HPO4 (aq) + H₂O Complete the calculation for Kb. Will this ion be acidic or basic? Predict the expected pH for the 0.050M solution.
1. For each of the solutions in part 3, calculate an expected pH. The Ka for HC₂H3O2 is: 1.8 x 10⁹ and the Kb for NH3 is 1.76 x 105. Remember to account for the dilution factor. a. 10.0mL of 0.10 M HC₂H₂O₂ + 5.0mL of 0.10M HCI b. 10.0mL of 0.10M NH3 + 5.0mL of 0.10M NaOH c. 10.0mL of 0.10M HC₂H₂O₂ +10.0mL 0.10M NaC₂H₂O₂ d. 10.0mL of 0.10 M NH3 + 10.0mL of 0.10M NH.CI 2. Which solution(s) in question 1 would be considered a buffer solution? 3. Complete the calculation for K, from the earlier discussion of the amphoteric salt. Will this ion be acidic or basic? Predict the expected pH for the 0.050M solution. (1) H₂PO4 (aq) + H₂O → H₂O (aq) + HPO42(aq); K₁2 = 6.2 x 10-8 (2) H₂PO4 (aq) + H₂O → H₂PO4(aq) + OH(aq); Kb = = ??? Kw Kal 4. Similarly, the HPO4 ion is also amphoteric. The two possible reactions are: H₂O(aq) + PO4³(aq); Kas = 4.2 x 10-¹3 (1) HPO4 (aq) + H₂O) Kw = → H₂PO4 (aq) + OH(aq); Kb = = ??? K₂2 (2) HPO4 (aq) + H₂O Complete the calculation for Kb. Will this ion be acidic or basic? Predict the expected pH for the 0.050M solution.
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Chapter16: Acid-base Equilibria
Section: Chapter Questions
Problem 16.125QP: A solution made up of 1.0 M NH3 and 0.50 M (NH4)2SO4 has a pH of 9.26. a Write the net ionic...
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Transcribed Image Text:1. For each of the solutions in part 3, calculate an expected pH. The Ka for HC₂H3O2 is: 1.8 x 10¹5
and the Kb for NH3 is 1.76 x 10. Remember to account for the dilution factor.
a. 10.0mL of 0.10 M HC₂H₂O2 + 5.0mL of 0.10M HCI
b. 10.0mL of 0.10M NH₂ + 5.0mL of 0.10M NaOH
c. 10.0mL of 0.10M HC₂H₂O₂ +10.0mL 0.10M NaC₂H₂O₂
d. 10.0mL of 0.10 M NH3 + 10.0mL of 0.10M NH₂CI
2. Which solution(s) in question 1 would be considered a buffer solution?
3. Complete the calculation for K, from the earlier discussion of the amphoteric salt. Will this ion
be acidic or basic? Predict the expected pH for the 0.050M solution.
(1) H₂PO4 (aq) + H₂O
→ H3O*(aq) + HPO42(aq); Ka2 = 6.2 x 10-8
(2) H₂PO4 (aq) + H₂O
→
Kw
H3PO4(aq) + OH(aq); Kb = ???
Kal
4. Similarly, the HPO4 ion is also amphoteric. The two possible reactions are:
(1) HPO4² (aq) + H₂O → H3O*(aq) + PO4³(aq); Kas = 4.2 x 10-¹3
(2) HPO4 (aq) + H₂O
Kw
→ H₂PO4 (aq) + OH(aq); Kb =
<= ???
K₁2
Complete the calculation for Kb. Will this ion be acidic or basic? Predict the expected pH for the
0.050M solution.
(OVER)
53
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