[Review Topics]Calculate the pH at the halfway point and at the equivalence point for each of the following titrations.a 100.0 mL of 0.30M HC,H,O2 (K. = 6.4 x 10) titrated by 0.10 M NaOH%3DpH at the halfway point=%3DpH at the equivalence pointb. 100.0 ml. of 0.30 M C2H; NH, (K, = 5.6 x 10) titrated by 0.50 M HNO,%3DpH at the halfway point =pH at the equivalence pointc. 100.0 mL of 0.80 M HCl titrated by 0.25 M NaOHpH at the halfway point=pH at the equivalence point%3D

a) 100 mL of 0.10 M HC7H5O2 (Ka = 6.4 X10-5) titrated by 0.10 M NaOH Solution : a) At…

Lalculate the pH at the halfway point and at the equivalence point for each of the following titrations a. 100.0 ml. of 0.30 M HC;H,O2 (K. = 6.4 x 10) titrated by 0.10 M NaOH pH at the halfway point pH at the equivalence point %3D b. 100.0 mL of 0.30 M C2H5 NH2 (K = 5.6 x 10 10) titrated by 0.50 M HNO3 %3D pH at the halfway point pH at the equivalence point !3! c. 100.0 mL of 0.80 M HCl titrated by 0.25 M NAOH pH at the halfway point pH at the equivalence point !!

Lalculate the pH at the halfway point and at the equivalence point for each of the following titrations a. 100.0 ml. of 0.30 M HC;H,O2 (K. = 6.4 x 10) titrated by 0.10 M NaOH pH at the halfway point pH at the equivalence point %3D b. 100.0 mL of 0.30 M C2H5 NH2 (K = 5.6 x 10 10) titrated by 0.50 M HNO3 %3D pH at the halfway point pH at the equivalence point !3! c. 100.0 mL of 0.80 M HCl titrated by 0.25 M NAOH pH at the halfway point pH at the equivalence point !!

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

See similar textbooks

Similar questions

Which is the best indicator for the equivalence point during the titration of KOH solution with HCIO. Indicator A. Acid Range Color yellow pH Range 10.1-12.2 Basic Range Color red B. 8.3-9.9 red colorless C. yellow 6.3-7.3 purple D. гed 4.2-6.2 yellow yellow E. red 2.1-4.4
What do you call the stage of the titration in which the number of moles of the titrant is stoichiometrically less than the number of moles of the analyte? pre-equivalence equivalence end stage post-equivalenc
C)
For the titration of a strong acid with a strong base, which statement below is FALSE? O Past the equivalence point, the pH is due to diluted excess strong basest the equivalence point, the pH is due to diluted excess strong base O Between V =0 mL and the equivalence point, the pH is due to diluted unreacted strong acid. O At V = 0 mL titrant added, the pH is due to initial concentration of strong acid. O The indicator changes color at the end point due to excess acid. At the equivalence point, the pH is due to the auto-ionization of water.
10. Calculate the pH at equivalence point and find the indicators for the following titrations: a 25 mL of 0.5 M HI with 0.1 M KOH b. 25 mL 0.1 M CH;NH, with 0.1 M HCI c. 25 mL of 0.1 M CH;COOH with 0.1 M HCI
11. A 35.0 mL sample of 0.100 M acetic acid is titrated with a 0.150 M NaOH solution. The Ka of acetic acid 1.80 * 10-5. Calculate the pH at the following points of the titration: A) 9.00 mL of the base is added to the acid B) 1/2 equivalence point C) Equivalence point
A 75.0 mL sample of 0.100M NH3 is titrated with 0.100 M HCI. What is the most likely pH of the resulting solution after the addition of 100.0 mL of HCl to the NH3? Kp, NH3 = 1.8x10-5 O the pH would be exactly 1 O the pH is = 7.545 O the pH = 5.277 O pH = 1.845
In the titration curve below, which species would NOT be in solution at Point B? 14 Unknown Solution K2A %3D 13 12 pH 11 10 9. 8. D 6. 4 --O E 3 F 1 25 50. 75 100. mL of 1.00 M HCI added O CI- O H2A O K+ O A2- O HA
A 50.0 mL aliquot of a 0.00100M solution of acetic acid (K, = 1.8 x 10-5) is titrated with 0.00993M NaOH. Use the Indicator Table below to decide which of the indicators listed would most accurately signal the equivalence point for this titration. Properties of Several Indicators Write the letter corresponding to your choice of indicator in the box
Help me with both parts of number 4
Please don't provide handwriting solution
Consider the titration of a 25.0-mL sample of 0.115 M CH3COOH with 0.100 M КОН. Ka CH3COOH = 1.8x10-5 O The pH at the equivalence point is 0. O The pH at the equivalence point is neutral. O The pH at the equivalence point is = 14 since one electrolyte is a strong electrolyte. %3D O The pH at the equivalence point is > 7.