a) Consider: A4(aq) + 2 H3O*(aq) –→ H2A² (aq) + 2 H2O(1). This is the net ionic reaction that occurs between the beginning of the titration and to the equivalence point. (Type in 1st, 2nd, 3rd or 4th.) b) After point along the titration curve, the analyte is just starting to gain the 4th proton. (Type in A, B, C...) c) The point along the titration curve where concentrations of H2A²¯ and H3A¯ are equal is (Турe in A, B, С...) d) Molecules and ions: H4A, H3A', H2A²", HA3- or A4- Of the molecule and ions shown above, the molecule or ion that has the highest concentration when 36.0 mL of 0.15 M HCI has been added is (Do not use super- or subscripts. Write H3A¯ as H3A-.) For H4A: Ka1 = 2.5 x 102, Ka2 = 7.5 x 105, Ka3 = 9.2 x 10-9, and Ka4 = 4.3 x 10-13 e) The pH at midpoint 2 is (Report your pH va to two sig figs.) f) The value of Kp3 for A4 is . (Use two sig figs.) (Do not use superscripts, subscripts or carets! Write 1.2 x 103 as 1.2x10-3 or 1.2e-3.)

a) Consider: A4(aq) + 2 H3O*(aq) –→ H2A² (aq) + 2 H2O(1). This is the net ionic reaction that occurs between the beginning of the titration and to the equivalence point. (Type in 1st, 2nd, 3rd or 4th.) b) After point along the titration curve, the analyte is just starting to gain the 4th proton. (Type in A, B, C...) c) The point along the titration curve where concentrations of H2A²¯ and H3A¯ are equal is (Турe in A, B, С...) d) Molecules and ions: H4A, H3A', H2A²", HA3- or A4- Of the molecule and ions shown above, the molecule or ion that has the highest concentration when 36.0 mL of 0.15 M HCI has been added is (Do not use super- or subscripts. Write H3A¯ as H3A-.) For H4A: Ka1 = 2.5 x 102, Ka2 = 7.5 x 105, Ka3 = 9.2 x 10-9, and Ka4 = 4.3 x 10-13 e) The pH at midpoint 2 is (Report your pH va to two sig figs.) f) The value of Kp3 for A4 is . (Use two sig figs.) (Do not use superscripts, subscripts or carets! Write 1.2 x 103 as 1.2x10-3 or 1.2e-3.)

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...

See similar textbooks

Similar questions

What is the pH at 90.00 mL of titrant in the titration of 50.00 mL of 0.400 M B (a generic base with Kp = (4.45x10^-10)) with 0.200 M HNO3? Enter your answer in scientific notation with 3 sig figs. Do not include any units in your answer. Do not round any intermediate calculations. Note: Your answer is assumed to be reduced to the highest power possible. Your Answer: x10 Answer
3
Determine the pH at the point in the titration of 40.0 mL of 0.200 M H,NNH2 with 0.100 M HNO, after 80.0 mL of the strong acid has been added. The value of Kb for H,NNH, is 3.0 x 10-6.
2) Titration of 50.00 ml of 0.04715 M Na;C04 required 39.25 mL of potassium permanganate solution. Calculate the molar concentration of potassium permanganate. Mno, + H;C204→ Mn²+ + CO, + H20
The half‑equivalence point of a titration occurs half way to the equivalence point, where half of the analyte has reacted to form its conjugate, and the other half still remains unreacted. If 0.260 moles of a monoprotic weak acid (?a=1.4×10−5) is titrated with NaOH, what is the pH of the solution at the half‑equivalence point?
2. Which indicator could be used for the titration of 25.0 mL of 0.100 M propanoic acid (HC3H5O3, K₂ = 1.3E-5) with 0.100 M NaOH?
What is the pH of 3.00 L of a buffer made of (2.840x10^-1) M HBrO and (7.16x10^-1) M KBrO AFTER the addition of 250.00 mL of 0.800 M HNO3? Enter your answer in scientific notation with 3 sig figs. Do not include any units in your answer. Do not round any intermediate calculations. Note: Your answer is assumed to be reduced to the highest power possible. Your Answer: х10
The half‑equivalence point of a titration occurs half way to the equivalence point, where half of the analyte has reacted to form its conjugate, and the other half still remains unreacted. If 0.260 moles of a monoprotic weak acid (Ka=7.6×10−5) is titrated with NaOH, what is the pH of the solution at the half‑equivalence point?
Calculate the pH for each of the cases in the titration of 25.0 mL of 0.110 M pyridine, C₁H₁N(aq) with 0.110 M HBr(aq). The Kb of pyridine is 1.7 x 10-⁹. before addition of any HBr pH = after addition of 12.5 mL of HBr after addition of 16.0 mL of HBr after addition of 25.0 mL of HBr after addition of 35.0 mL of HBr 9.31 pH = pH = pH = pH = 5.23 4.63 Incorrect 11.65 Incorrect 1.33 Incorrect
the pKb values for the dibasic base B are pKb1 = 2.10 and pKb2 = 7.36. calculate the pH at all points in the titration of 50 mL of a .55 M B solution with 55 M HCI: before the addition of HCl, after the additon of 25 mL HCI, after addition of 50 mL HCl, after addition of 75 mL HCl, after addition of 75 mL HCl, after addition of 100 mL HCl
T Please don't provide the handwriting solution
The Kb of a base is 3.9 × 10−5. What is the pH at the half-equivalence point of the titration of this base with strong acid?