38. A buffer solution is 0.40 M NH3 and 0.60 M NHACI. Kb for NH3 is 1.8 x 10-5 a) Calculate the pH for the buffer sy...
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...
I have already figured out part a. I need help with b and c. thank you. 38. A buffer solution is 0.40 M NH3 and 0.60 M NH4CI. Kb for NH3 is 1.8 x 10-5 a) Calculate the pH for the buffer system. pH = 7.08 b) Calculate the pH of the solution after adding 0.00600 moles of NaOH to 400.0 mL of the buffer. c) Calculate the pH of the solution after adding 0.050 moles of HCl to 600.0...
This is one question, please answer all parts! A buffer solution is 0.40 M NHs and 0.60 M NH4CI Kb for NHs is 1.8x 10 a) Calculate the pH for the buffer system b) Calculate the pH of the solution after adding 0.00600 moles of NaOH to 400.0 mL of the buffer c) Calculate the pH of the solution after adding 0.050 moles of HCl to 600.0 mL of the buffer
3) Kb for NH3 1.8 x 10-5 a) Calculate the pH of a buffer solution that is 0.100 M NH3 and 0.120 M NHANO3. b) What is the pH after 60.0 mL of 0.010 M HCl is added to 90.0 mL of the buffer solution in 2(a). Assume the change in volume is additive. c) What is the pH after 60.0 mL of 0.010 M Ca(OH)2 is added to 90.0 mL of the buffer solution in 2(a). Assume the change...
4. Calculate the pH of a buffer solution made by adding 500 mL of 0.40 M HCl to 750 mL of 0.80 M NHs. For NH3, Kb-1.8 x 10-5. A) pH-9.95 B) pH -9.72 C)pH -9.55D) pH 9.25 E) pH-8.99
2. What is the pH of a buffer containing 0.050 M NH3 and 0.050 M NHACI? 3. What is meant by buffer capacity? 4. Sketch a pH titration curve for the addition of 0.10 M HCl to 25.0 mL of a 0.10 M NH3 solution and indicate the "buffer zone". 4. Sketch a pH titration curve for the addition of 0.10 M HCl to 25.0 mL of a 0.10 M NHz solution and indicate the "buffer zone".
A 75.0-mL volume of 0.200 M NH3 (Kb=1.8×10−5) is titrated with 0.500 M HNO3. Calculate the pH after the addition of 27.0 mL of HNO3. Express your answer numerically. A 52.0-mL volume of 0.35 MM CH3COOH (Ka=1.8×10−5Ka=1.8×10−5) is titrated with 0.40 M NaOH. Calculate the pH after the addition of 15.0 mL of NaOH. and Imagine that you are in chemistry lab and need to make 1.00 LL of a solution with a pH of 2.80. You have in front...
Titrations Part A A 75.0-mL volume of 0.200 M NH3 (Kb=1.8×10−5) is titrated with 0.500 M HNO3. Calculate the pH after the addition of 19.0 mL of HNO3. Express your answer numerically. Part B A 52.0-mL volume of 0.35 M CH3COOH (Ka=1.8×10−5) is titrated with 0.40 M NaOH. Calculate the pH after the addition of 23.0 mL of NaOH. Express your answer numerically.
A 75.0-mL volume of 0.200 M NH3 (Kb=1.8×10-5) is titrated with 0.500 M HNO3. Calculate the pH after the addition of 11.0mL of HNO3.A 52.0-mL volume of 0.35 M CH3COOH (Ka=1.8×10-5) is titrated with 0.40 M NaOH. Calculate the pH after the addition of 31.0mL of NaOH.
a) Calculate the pH of a buffer system that contains o.200 M of NH3(aq) and o.200 M of NH4Cl(aq). The Kb of NH3(aq) is 18 x 10-5. Consult Textbook Numerical Answer pH b) Calculate the change in pH when 6.00 mL of 100 M HCl is added to 100.0 mL of the buffer solution. Numerical Answer: c) Calculate the change in pH when 6.00 mL of o.100 M NaOH is added to 100.0 mL of the buffer solution. Numerical Answer: