Here Ph will not change but as we know, Buffer solution as a solution whose ph doesnot change by adding small quantity of acid or base.
In part b, bases is added so ph will remain same as the part a
In part c, acid is added so here also ph remain same.
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 0.6...
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 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.
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...
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
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
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...
28. A 0.50 L buffer solution is 0.20 M in HF and 0.40 M in NaF. The Ka for HF is 1.5 x 10* Show all work for full credit. (a) Calculate the pH of the solution after the addition of 0.025 moles of solid KOH. (3 pts) (b) Calculate the pH of the solution after the addition of 0.050 moles of HCl. (3 pts)
We have 500.0 mL of a buffer solution that is 0.636 M in NH3 and 0.345 M in NH4Cl. We add 500.0 mL of a solution 0.249 M in HCl. The final volume is 1.0000 L. The Kb value for NH3 is 1.8 x 10-5. What is the pH of the final solution?
1) Calculate the pH of a 0.026 M solution of NH4NO3. Kb of NH3= 1.8x10^-5. include both the dissociation and hydrolysis equations in the set up 2)calculate the pH of a 75 ml buffer solution containing 0.20 M of citric acid(C6H8O7, Ka= 3.2x10^-7) and 0.30 M sodium citrate. and what is the pH after adding 3.0 mlbof 1.5 M HCl to the buffer solution in that question? 3) what is the pH of 20.00 ml of 0.40 M nitrous acid(...
1)A 10.0 mL sample of 0.25 M NH3(aq) is titrated with 0.20 M HCl(aq) (adding HCl to NH3). Determine which region on the titration curve the mixture produced is in, and the pH of the mixture at each volume of added acid.Kb of NH3 is 1.8 × 10−5.Henderson–Hasselbalch equation:Part a):1) After adding 10 mL of the HCl solution, the mixture is [ Select ] ["at", "before", "after"] the equivalence point on the titration curve.2) The pH of the solution after...
Consider titration of 20.0 mL of 0.100 M NH3 with 0.200 M HCl solution. Calculate the pH after the addition of the following volumes of HCl solution. The Kb of NH3 = 1.8 x 10^5 a. 0.00 mL b. 6.00 mL c. 10.00 mL d. 20.00 mL