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- When 40.00 mL of a weak monoprotic acid solution is titrated with 0.100-M NaOH, the equivalence point is reached when 35.00 mL base has been added. After 20.00 mL NaOH solution has been added, the titration mixture has a pH of 5.75. Calculate the ionization constant of the acid.When a diprotic acid. H2A. is titrated with NaOH, the protons on the diprotic acid are generally removed one at a time, resulting in a pH curve that has the following generic shape: a. Notice that the plot has essentially two titration curves. If the first equivalence point occurs at 100.0 mL NaOH added, what volume of NaOH added corresponds to the second equivalence point? b. For the following volumes of NaOH added, list the major species present after the OH reacts completely. i. 0 mL NaOH added ii. between 0 and 100.0 mL NaOH added iii. 100.0 mL NaOH added iv. between 100.0 and 200.0 mL NaOH added v. 200.0 mL NaOH added vi. after 200.0 mL NaOH added c. If die pH at 50.0 mL NaOH added is 4.0 and the pH at 150.0 mL NaOH added is 8.0, determine the values Ka and Ka. for the diprotic acid. d.A 50.0-mL sample of NaHSO3 is titrated with 22.94 mL of 0.238 M KOH. (a) Write a balanced net ionic equation for the reaction. (b) What is [HSO3-] before the titration? (c) Find [HSO3-], [SO32-], [OH-], [K+], and [Na+] at the equivalence point. (d) What is the pH at the equivalence point?
- Question 16 of 20 Determine the pH at the point in the titration of 40.0 mL of 0.200 M H2NNH2 with 0.100 M HNO3 after 80.0 mL of the strong acid has been added. The value of Kb for H,NNH, is 3.0 x 106, 9- 1 4 NEXT > Nse the table below to determine the moles of reactant and product ater the reaction of the acid and base. H2NNH2(aq) H*(aq) H2NNH3*(aq) Before (mol) Change (mol) After (mol) 5 RESET 0.100 + x 0.100 - x 0.100 0.200 +x 0.200 + x 0.200 - ) 1.00 x 103 -1.00 x 10-3 2.00 x 10 3 -2.00 x 10-3 6.00 x 103 -6.00 x 103 7.00 x 103 -7.00 x 103 8.00 x 103 -8.00 x 10 3 ↑#6 Calculate the pH during the titration of 40.00 mL of 0.1000 M HCl with 0.1000 M NaOH solution after the following additions of base: (a) 23.00 mL pH = (b) 39.40 mL pH = (c) 54.00 mL pH =1. Calculate the pH changes during the titration of 0.100 M HCl with 50.00 mL of 0.0500 M KOH when the following volumes of the titrant is added: (a) The volume of the titrant required to reach the equivalence point (b) Select five (5) different volumes of the titrant before the equivalence point. (c) At equivalence point (d) Select five (5) different volumes of the titrant after the equivalence point (e) Plot the titration curve using MS Excel Spreadsheet (f) Plot the 1st order and 2nd order titration curve
- Consider the titration of 100.0 mL of 0.100 M H2NNH2 (Kb = 3.0 ✕ 10-6) by 0.200 M HNO3. Calculate the pH of the resulting solution after the following volumes of HNO3 have been added. (a) 0.0 mL (b) 20.0 mL (c) 25 ml (d)40 ml (e) 55.0 mL (f) 65.0 mLWhat is the pH of a buffer prepared by adding 0.506 mol of the weak acid HA to 0.305 mol of NaA in 2.00 L of solution? The dissociation constant Ka of HA is 5.66 × 10-7. Express the pH numerically to three decimal places. • View Available Hint(s) pH : = 6.027 Submit Previous Answers Correct Important: If you use this answer in later parts, use the full unrounded value in your calculations. Since both the acid and base exist in the same volume, we can skip the concentration calculations and use the number of moles in the Henderson-Hasselbalch equation to calculate the pH. The answer will be the same. Part B What is the pH after 0.150 mol of HCl is added to the buffer from Part A? Assume no volume change on the addition of the acid. Express the pH numerically to three decimal places. • View Available Hint(s) ? pH =Question 4 a) Determine the pH of 0.10 M NAOH solution. b) Find out the pH of a 0.002 M acetic acid solution if it is 2.3% ionised at this dilution. c) A chemistry student desires to prepare one litre of a solution buffered at pH 9.00. How many grams of ammonium chloride haye to be added to one litre of 0.20 M NH3 to makesuch a buffer. pKb value of ammonia is 4.75 in the equation. NH3 + H20 = NH + OH
- Question 7 of 14 Submit Determine the pH at the point in the titration of 40.0 mL of 0.200 M H2NNH2 with 0.100 M HNO3 after 10.0 mL of the strong acid has been added. The value of Kb for H2NNH2 is 3.0 × 10 6. 4 NEXT > Use the table below to determine the moles of reactant and product after the reaction of the acid and base. H2NNH:(aq) H(aq) H.NNH (aq) Before (mol) Change (mol) After (mol) 5 RESET 0.100 0.200 + x 0.200 - x +x 0.200 0.100 - x 1.00 x 10-3 -1.00 x 10-3 2.00 x 103 -2.00 x 10 6.00 x 103 -6.00 x 103 0.100 + x 7.00 x 10-3 -7.00 x 10-3 8.00 x 103 -8.00 x 103 4:50 PM 4/15/2021 68 e to search Ins 近Question 10 Which of the following statements about buffered solu- tions are true? Select all that apply. A Buffer solutions resist changes in the concentration of hyd roxide ions. A buffer solution may be made up of a strong acid and one of its salts. C Buffer solutions will not change very much if a small amou nt of strong acid is added to it. Buffer solutions will not change pH very much if a small a mount of weak base is added to it.The p?a of hypochlorous acid is 7.530 . A 58.0 mL solution of 0.130 M sodium hypochlorite ( NaOCl ) is titrated with 0.299 M HCl . Calculate the pH of the solution after the addition of 9.78 mL of 0.299 M HCl . (please type answer not write by hend)