Problem 4: Given: 1.0 M HOAC (K. = 1.8 x 10) 1.0 M NaOH stock solution...
Problem 5: Given: 1.0 M HOAc solution (K4 = 1.8 x 10-5). 1.0 M NaOAc solution Make 500 mL of 1.0 M HOAc/OAc- buffer with pH = 5.00
At the equivalence point of a titration of HOAc (acetic acid, pKa = 1.76 x 10-5) with NaOH, the species present of OAc" and H20. If the concentration of OAc at the equivalence point is 0.50 M, what is the pH of the solution? Remember that Kb x Ka = 10-14 and that the OAc will react with water as follows: OAC- + H20 --> HOÀc + OH- . 1 4.77 2. 10.23 3 5.68 4. 9.23
Acetic acid, HOAc, has a Ka = 1.73x10^-5. You need to prepare a buffer solution with a pH of 5.00 from a solution of 1M acetic acid (HOAc) and 1 M sodium acetate (NaOAc). How many mL of NaOAc should be added to the 30mL of HOAc solution to create the buffer? Using this buffer as an example, provide the reactions that allow the buffer to resist changes in pH upon addition of 1) NaOH and 2) HCl.
Consider the titration of 50 mL of 0.100 M acetic acid (CH3COOH, Ka = 1.8 x 10-5) with 0.200 M NaOH solution. Show all calculations for full credit. a) Write the titration reaction: b) Calculate the pH after 5.00 mL of NaOH: c) Calculate the pH after 12.5 mL of NaOH: d) Calculate the pH after 25 mL of NaOH:
A buffer is prepared by adding 150 mL of 1.0 M NaOH to 250 mL of 1.0 M NaH2PO4. How many moles of HCI must be added to this buffer solution to change the pH by 0.40 units? Assume the total volume remains unchanged at 400 mL. For H2PO4, K = 6.3 x 10-8 0.013 mol 0.25 mol (Your answer) 0.50 mol 0.057 mol (Correct answer) 0.031 mol
5. Calculate the grams of NaCH3COO required for 100.0 mL of 0.20 M CH3COOH solution to achieve a pH of 4.40. (Assume no volume change.) K = 1.8 x 10-5 6. What is the pH of 100.0 mL of buffer consisting of 0.20 M CH3COOH/0.20 M NaCH3COO after 10.0 mL of 0.20 M HC1 was added into the solution ? Kg = 1.8 x 10-5 7. The pH of a sodium acetate-acetic acid buffer is 4.80. Calculate the ratio of...
What is the pH of a solution (500 mL, 3.40 mM HOAc) in which 50 mL of 1.00 M HCl is added? What percentage of the HOAc is dissociated? What is the pH of a 3.40 mM of acetic acid, 500 mL in which 50 mL of 1.00 M NaOAc has been added? Ka HOAc is 1.8 x 10-5? What percentage of the acid is dissociated?
38. A buffer solution is 0.40 M N Kb for NH3 is 1.8 x 10 38. Abre olution is 0-40 M N11 and 0.60 NHộ an 0,60 M NHẠC. and 0.00 4) Calculate the ph for the buffer system kw Kakba PH- pka leo ENHI 1 1. XD INHA KA Ich PH 3 1.8x10-5 -5.56x10 10 P log (5,56x10") + log (0.40) H-9.15+ (-0.18) PH- 9.03 alculate the pH of the solution after adding 0.00600 moles of NaOH to 400.0...
What is the pH of a 0.25 M NaOAc solution? For HOAc Ka = 1.8 × 10^-5
. You have 45 mL of a 0.84 M solution of HCOOH (K 1.8 x 10-4). You titrate it with 0.51 M NaOH What is the pH at the half equivalence point (the point where you have added half the number of moles of base as you had acid)? (a) 2.08 (b) 2.51 (c) 2.77 (d) 3.30 (e) 3.74