pH LI Calculate the pH of the following solutions: Solution (a) 0.10 M CH3COOH 12.9 (b)...
If 100mL of 0.10M CH3COOH (Ka=1.8x10-5) is titrated with 0.10 M NaOH. Calculate the pH value for the following solution. A. 75.0 mL of NaOH is added B. 100.0 mL of NaOH is added C. Suggest an indicator for this titration
What is the pH of a solution prepared by mixing 25.00 mL of 0.10 M CH3COOH with 25.00 mL of 0.050 M CH3COONa? Assume that the volume of the solutions are additive and that Ka = 1.8 x 10-5 for CH3COOH.
1) What is the pH of a solution in which 25 mL of 0.10 M NaOH is added to 15 mL of 0.10 M HCl? 2) If you add 2.50 mL of 0.150 M HCl to 100 mL of a buffer consisting of 0.100 M CH3COOH and 0.200 M CH3COONa, what will be the change in pH? (Ka of CH3COOH is 1.8x10^-5)
Calculate the pH of the following solutions: a) Calculate the pH of the solution obtained by mixing 20.00 mL of 1.00 M HCl with water until a volume of 2000 mL. b) Calculate the pH by mixing 5.00 mmol of HNO3 with 5.00 mmol of KOH, in a total volume of 1000 mL of solution c) Calculate the pH by mixing 5.00 mmol of C6H5COOH with 3.00 mmol NaOH, and bring up to volume 300 mL. d) Calculate the pH...
i need help with finding the ph of an aq solution. im confused 9,10,12,13,14, &15. on 10 I caluclated 14 and 12 the closest answer i got was 2.67, but i was exact. If its not a big inconvience can you show me how? thank you 9. Calculate the pH of a 0.65 M NH3 solution if Kb for NH3 is 1.8x10-5. a) 2.47. b) 4.93. c) 11.53. d) 12.68. 10. The pH of a 0.2 M aqueous solution of...
1. What volume of 0.10 M NaOH is needed to neutralize 100 mL of 0.050 M HCl? 2a. When 100 mL of 0.01 M NaOH solution is mixed with 100 mL of 0.01 M of HNO3 solution, what is the concentration of H+ and the pH in the resulting mixture? 2b. When 100 mL of 0.01 M NaOH solution is mixed with 100 mL of 0.02 M of HCl solution, what is the concentration of H+ and the pH in...
2. Calculate the pH at the following point in the titration of 20.00 mL of0.500 M CH3COOH with 0.500 M NaOH. CH3COOH has a Ka = 1.8x10-5. (2.5 pts) a. pH before the addition of any NaOH. Include balanced chemical equation. b. pH after the addition of 8.00 mL of 0.500 M NaOH. Include balanced chemical equation. c. pH after the addition of 10.00 mL of 0.500 M NaOH. Include balanced chemical equation. d. pH after the addition of 20.00...
What is the pH of the resulting solution if 30.00 mL of 0.10 M acetic acid is added to 30.00 mL of 0.10 M NaOH? Ka = 1.8x10-5 for CH3CO2H.
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(...
Part Calculate the pH of a solution prepared by mixing 15.0 mL of 0.10 M NaOH and 30.0 mL of 0.10 M benzoic acid solution. (Benzoic acid is monoprotic; its dissociation constant is 6.5x10.) IVO AQ R O a ? Submit Request Answer