After 2 mL NaOH has been added:
pH = 3.15, [H3O+] = 10-3.15 = 7.08*10-4 M, [OH-] = 10-14/10-3.15 = 1.41*10-11 M, pOH = 14-pH = 10.85
After 26 mL (1 mL before equivalence point) NaOH has been added:
pH = 6.1, [H3O+] = 10-6.1 = 7.94*10-7 M, [OH-] = 10-14/10-6.1 = 1.26*10-8 M, pOH = 14-pH = 7.9
After 27 mL (equivalence point) NaOH has been added:
pH = 8.88, [H3O+] = 10-8.88 = 1.32*10-9 M, [OH-] = 10-14/10-8.88 = 7.586*10-6 M, pOH = 14-pH = 5.2
Use the acetic acid titration curve to determine the listed pH values and then perform the...
Concentration of HCl is 0.09655 M. Concentration of NaOH is 0.100 M. a) What is the pH at equivalence point? b) Moles of HCl at equivalence point? c) Moles of NaOH at equivalence point? d) Volume of NaOH at equivalence point? 1.15 Volume NaOH added (mL) pH Moles of NaOH added 0.89 0.89 0.00010 0.89 0.00020 0.90 0.00030 0.91 0.00040 0.93 0.00050 0.94 0.00060 0.96 0.00070 0.98 0.00080 1.01 0.00090 1.03 0.00100 1.06 0.00110 1.08 0.00120 1.11 0.00130 0.00140 1.19...
Concentration of HCI is 0.09655 M. Concentration of NaOH is 0.100 M. a) What is the pH at equivalence point? b) Moles of HCl at equivalence point? c) Moles of NaOH at equivalence point? d) Volume of NaOH at equivalence point? Volume NaOH added (mL) pH Moles of NaOH added 0.89 0.89 0.00010 0.89 0.00020 0.90 0.00030 0.91 0.00040 0.93 0.00050 0.94 0.00060 0.96 0.00070 0.98 0.00080 1.01 0.00090 1.03 0.00100 1.06 0.00110 LOS 0.00120 1.11 0.00130 1.15 0.00140 1.19...
Volume NaOH added Moles of NaOH added pH (mL) 0 2.89 0 3.18 0.00010 0,00020 3.18 0.00030 3 3.42 3.56 4 0.00040 0.00050 5 3.67 Concentration of NaOH-0.1 M Concentration of HCHO-0.1 M 6 3.73 0,00060 0,00070 7 3.89 0,00080 8 3.99 9 4.07 0.00090 What is the pH at equivalence point? What is the volume of NaOH at equivalence point? a) 10 4.14 0.00100 b) Moles of NaOH at the equivalence point? Moles of HC:H0 at equivalence point? 11...
1.Draw the pH titration curve for the titration of 35 mL of 0.150 M acetic acid with 0.200 M NaOH. Include the pH values and NaOH volume requested below on your pH titration curve. Also, put on the curve the species that dictates the pH at the requested pH values. For acetic acid, K = 1.8 x 10%. 1) the initial pH 2) the pH after 15.0 mL of NaOH have been added 3) the volume of NaOH at the...
Determine the pH during the titration of 29.5 mL of 0.324 M acetic acid (Ka = 1.8×10-5) by 0.414 M NaOH at the following points. (a) Before the addition of any NaOH ________ (b) After the addition of 5.70 mL of NaOH _______ (c) At the half-equivalence point (the titration midpoint) _______ (d) At the equivalence point _______ (e) After the addition of 34.6 mL of NaOH ________
Calculate pH for a weak acid/strong base titration. Determine the pH during the titration of 67.3 mL of 0.419 M hypochlorous acid (K-3.5x10-) by 0.419 M NaOH at the following points. (a) Before the addition of any NaOH (b) After the addition of 15.0 mL of NaOH (c) At the half-equivalence point (the titration midpoint) (d) At the equivalence point (e) After the addition of 101 mL of NaOH
Question 3: Draw the titration curve (pH versus mL of NaOH added) that would be obtained from the titration of 30 mL of a 0.10 M solution of an unknown triprotic acid, H3A (Kat = 1.26 x 10-3; Ka2 = 5.6 x 10-6, Ka3 = 3.32 x 10-10) with 0.10 M NaOH. Indicate the volume needed to reach the first second, and third equivalence points and the pH at the half equivalence points for the three titration regions.
What is the shape of the titration curve (plot of pH vs. mL of added base) for titration of a weak acid by a strong base? In a titration, 10 mL of 0.10 M HF was titrated with 0.20 M KOH. Calculate the pH of the resulting solution after the addition of the following volumes of base: 0 mL, 2.5 mL, 5.0 mL, and 6.0mL. What volume of base is needed to reach the equivalence point? What species is present...
I'm not sure how to solve this! Any help is appreciated! 1.Draw the pH titration curve for the titration of 35 mL of 0.150 M acetic acid with 0.200 m Include the pH values and NaOH volume requested below on your pH titration curve. Al curve the species that dictates the pH at the requested pH values. For acetic acid, Ka = 1.885 in your pH titration curve. Also, put on the 1) the initial pH 2) the pH after...
This is incorrect. What are the titration points for this titration curve? The pH values, respectively at 0 mL is 9.16, at 10 mL pH is 5.56, at 20 mL pH is 4.98, at the equivalence point the pH is 3.24, at one half equivalence point the pH is 5.23, at 40 mL the pH is 1.87, at 50 mL the pH is 1.60. Use your calculations to make a sketch of the titration curve. Label Titration curve : y...