Question 15 Spoints Save Answer A chemist trates 75.0 mL of 0.10 M HNO2 Ka 4.510*)...
please help, and show steps if possible A chemist titrates 75.0 mL of 0.10 M HN3 (Ka = 2.5x10-5) with a 0.10 M KOH solution. Calculate the pH in the flask after 50.00 mL of the KOH solution is added. Enter your answer WITH TWO DECIMAL PLACES, or it will be marked incorrect! Which of the following acids would be the best to use to prepare a buffer with a pH of 5.45? C5H505COOH Ka = 4.0x10-6 CH3COOH Ka =...
An analytical chemist is titrating 91.8 mL of a 0.4200 M solution of nitrous acid (HNO2) with a 0.9300 M solution of KOH. The pK, of nitrous acid is 3.35. Calculate the pH of the acid solution after the chemist has added 24.9 mL of the KOH solution to it. Note for advanced students: you may assume the final volume equals the initial volume of the solution plus the volume of KOH solution added. Round your answer to 2 decimal...
A chemist performs a titration experiment on a 35 mL sample of 0.10 M CH3NH3+ (Ka = 2.27 x 10−11) with 0.10 M NaOH. Determine the pH of solution after 25 mL of NaOH is added to the solution.
You have 75.0 mL of 0.150 M HNO2 (Ka = 4.50 x 10-4) to which you add 50.0 mL of 0.150 M NaOH. What will be the resulting pH of the solution?
a) A 41.0 mL sample of 0.194 M HNO2 is titrated with 0.220 M KOH. (Ka for HNO2 is 4.57×10−4.) Determine the pH at the equivalence point for the titration of HNO2 and KOH. b) A 50.0-mL sample of 0.200 M sodium hydroxide is titrated with 0.200 M nitric acid. Calculate the pH of the solution, after you add a total of 56.7 mL 0.200 M HNO3.
1.A 25.00 ml smaple of 0.523 M nitrous acid, HNO2, solution is titrated with a 0.213 M NaOH. For HNO2, Ka = 4.0 X 10^-4 a) What is the pH before any NaOH is added? b) Write the reaction that takes place as KOH solution is added to the HNO2 solution. c) write the reaction that determines the pH at the equivialnce point. -What is the pH at the equivilance point -what is the pH at the 1/2 equivilance point...
25. 50.00 mL of 0.10 M CH3COOH (Ka = 1.8 x 10") is titrated with a 0.10 M KOH solution. After 75.00 mL of the KOH solution is added, the pH in the titration flask will be A) 9.31 B) 9.18 C) 9.52 D) 11.63 E) 12.30
24. 50.00 mL of 0.10 M CH3COOH (Ka = 1.8 x 10-5) is titrated with a 0.10 M KOH solution. After 50.00 mL of the KOH solution is added, the pH in the titration flask will be A) 4.28 B) 8.72 C) 9.41 D) 11.24 E) 12.08 [Kb = 5.6 x 10-10 for acetate ion] 0.0025 - 0.25 .
Consider a titration of 250 mL 0.15 M acetic acid (Ka = 1.8 x10-5) with 0.10 M KOH. What is the pH of the acetic acid solution (ie: before the titration has begun?) What is the pH after adding 25 mL of 0.10 M KOH? What is the volume of base needed to reach the equivalence point? Is the pH at equivalence point acidic, basic, or exactly neutral? What is the pH after 500 mL of KOH has been added?
An analytical chemist is titrating 239.5 mL of a 0.2900 M solution of aniline (CHNH, with a 0.3800 M solution of HNO3. The p K of aniline is 9.37. Calculate the pH of the base solution after the chemist has added 107.9 mL of the HNO2 solution to it. Note for advanced students: you may assume the final volume equals the initial volume of the solution plus the volume of HNO2 solution added. Round your answer to 2 decimal places....