Phosphoric acid is a triprotic acid (Kal = 6.9 × 10-3, K22 = 6.2 × 10-8, and K3 = 4.8 × 10-13).= 4.8 x 10-13).To find the pH of a buffer composed of H, PO, (aq) and HPO (aq), which pKa value should be used in theHenderson-Hasselbalch equation?O pKal = 2.16pK22 = 7.21O pKa3 =12.32Calculate the pH of a buffer solution obtained by dissolving 18.0 g of KH, PO, (s) and 34.0 g of Na, HPO, (s) in water and then4.diluting to 1.00 L.pH =

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Answered: Phosphoric acid is a triprotic acid…

Chemistry: The Molecular Science

5th Edition

ISBN:9781285199047

Author:John W. Moore, Conrad L. Stanitski

Publisher:John W. Moore, Conrad L. Stanitski

Chapter15: Additional Aqueous Equilibria

Section: Chapter Questions

Problem 15.BCP

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Consider only the first dissociation constant of a 10-4 M solution of boric acid(H3BO3):a) develop the appropriate ionization fraction equations,b) draw a species distribution plot for H3BO3,c) develop the appropriate equations for the buffer capacity of H3BO3,d) plot the buffer capacity versus pH,e) develop the appropriate equations for the titration of H3BO3 with NaOH,f) plot pH versus equivalent fraction,g) at which pH is β a maximum? and,h) at which value of α0 and α1 is β a maximum?
Calculate the molar solubility of AgSCN (Ksp = 1.1 x 10-12) in a solution maintained at pH 9.00 and where the concentration of ammonia is 0.100 M. HSCN: pKa = 4.0 [Ag(NH3)2]+ : Kf1 = 2.04 x 103; Kf2 = 8.13 x 103
Sodium acetate buffers are used for purification and precipitation of nucleic acids, as well as for protein crystallization and staining gels used in protein electrophoresis. It is very popular in hematology, since there is some evidence that acetate-buffered infusions show improved stability. Acetate buffers are inexpensive and simple to prepare, and can be stored at room temperature. 27-29. Calculate the pH of the acetate buffer solution that contains 0.50M acetic acid (Kb=5.56x10-10) and 0.50M sodium acetate. 30-32. Calculate the change in pH that occurs when 0.010 mol NaOH(s) is added to 1.0L of the acetate buffer. 33-35. Compare the pH change with that when 0.010M of NaOH is added to 1.0L of pure water. 36-40. How can the pH of the buffered solution not increase even though a strong base, NaOH, is added? Explain using the ions present.
In the supersaturated solution Group of answer choices Q = Ksp Q < Ksp Q > Ksp Ka = Ksp Calculate the pH of a buffer solution prepared by mixing 25 mL 0.400 M butyric acid, HC4H7O2 and 35 mL of 0.200 M potassium butyrate, KC4H7O2. Ka of butyric acid is 2.76 x 10-6. Group of answer choices 5.40 3.60 6.30 4.50
A buffer was made by mixing 0.1926 moles of C 9H 7O 4H with 0.1960 moles of NaC 9H 7O 4 and diluting to exactly 1 liter. What will be the pH after addition of 10.00 mL of 0.3004 M CsOH to 50.00 mL of the buffer? K a(C 9H 7O 4H) = 3.000e-4. Note: only a portion of the original buffer is used in the second part of the problem.
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Titration of 50.00 mL of 0.04715 M Na2C2O4 required 39.25 mL of a potassium permanganate solution. 2MnO4- + 5C2O4-2 +16H+ -> 2Mn2+ + 10CO2(g) + 8H2O Calculate the molar concentration of the KMnO4 solution. Pls show step by step. What type of molecules will interfere in this analysis ?
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