Determine the pH during the titration of 60.4 mL of 0.442 M formic acid (Ka = 1.8×10-4) by 0.442 M KOH at the following points.   At the equivalence point  (e) After the addition of 90.6 mL of KOH

Calculate the pH at the equivalence point in titrating 0.090 M solutions of each of the following with 0.064 M NaOH. (a) hydrochloric acid (HCI) pH = (b) hypolodous acid (HIO), K₂ = 2.3e-11 pH = (c) phenol (HC6H5O), Ka 1.3e-10 PH

Calculating the pH of a weak base titrated with a strong acid An analytical chemist is titrating 104.1 mL of a 0.1200M solution of propylamine (C,H,NH,) with a 0.2600M solution of HNO3. The p K, of propylamine is 3.46. Calculate the pH of the base solution after the chemist has added 53.1 mL of the HNO, solution to it. Note for advanced students: you may assume the final volume eguals the initial volume of the solution plus the volume of HNO, solution added. Round your answer to 2 decimal places. pH = Explanation Check O 2021 McGraw-Hill Education. All Rights Reserved. Terms of Use Privacy | Accessibility APR 23 MacBook Air O00 000 F4

Calculate the pH during the titration of 30.00 mL of 0.1000 M KOH with 0.1000 M HBr solution after the following additions of acid: (a) 8.00 mL pH = (b) 29.20 mL pH = (c) 35.00 mL pH =

Calculate pH for a weak base/strong acid titration. Determine the pH during the titration of 35.9 mL of 0.286 M methylamine (CH3NH₂, Kp = 4.2x10-4) by 0.286 M HCIO4 at the following points. (a) Before the addition of any HCIO4 (b) After the addition of 13.2 mL of HCIO4 (c) At the titration midpoint (d) At the equivalence point (e) After adding 54.9 mL of HCIO4

Find the pH of the reaction mixture after the addition of the given volume (see below for your assignment) of 0.25M hydrochloric acid to a 20.0 mL sample of .15M potassium fluoride (Ka for HF =7.2 x 10^-4) 13.5 mL HCl added Weak base, strong acid pH curve Titration, post equivalence point

Calculate the pH at the equivalence point for the titration of 0.100 M methylamine (CH, NH,) with 0.100 M HCI. The K, of methylamine is 5.0 × 10-4. pH =

Calculate the pH of a buffer that is 0.208 M lactic acid, HC3H5O3, and 0.208 M sodium lactate, NaC3H5O3 if 9.474 mL of 4.192 M NaOH is added. The total volume is 1.00 L. The Ka for lactic acid is 1.4*10-4.

When titrating a 25 mL solution of 0.20M CH3COOH with 0.10M KOH, you realize you forgot to add an indicator initially. You've added 10 mL of KOH to the flask of acid. Ka of CH3COOH = 1.8 x 10^-5 1) Calculate the pH at this point 2) What color would your solution be if you add 40 mL KOH more. And a few drops of clorophenol blue indicator at this point. Why?

Calculate the pH during the titration of 30.00 mL of 0.1000 M KOH with 0.1000 M HBr solution after the following additions of acid:    (a) 4.00 mL    pH =       (b) 29.50 mL    pH =       (c) 35.00 mL    pH =