Study 3: Titration of a Weak Acid, pKa = 5, with a Strong Base 10.00 mL of 0.100 M HX with 0.100 M NaOH e) Find the (H+) and pH of the acid before addition of the NaOH. (use Ka) f) Determined the volume of NaOH needed to reach the equivalence point, Ve. g) Find the [H+] and pH at the equivalence point, Ve

Study 3: Titration of a Weak Acid, pKa = 5, with a Strong Base 10.00 mL of 0.100 M HX with 0.100 M NaOH e) Find the (H+) and pH of the acid before addition of the NaOH. (use Ka) f) Determined the volume of NaOH needed to reach the equivalence point, Ve. g) Find the [H+] and pH at the equivalence point, Ve

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

0.434-g sample of an unknown monoprotic acid was titrated with 0.120 M KOH and the resulting titration curve is shown here. Find pKa hi, i found the molar mass 0.434g/4.2x10-3 but dont know how to find pKa thank you!
3
Q3
Consider the titration of a 60.0 mL of 0.295 M weak acid HA (Ka = 4.2 x 10-6) with 0.400 M КОН. After 30.0 mL of KOH have been added, identify the primary species left in the solution. A) HA and A В) НА C) HA and OH D)A E)A and OH"
Consider the titration of 50.0 mL of 0.100 M acetic acid with 0.0900 M NaOH. For acetic acid, Ka = 1.8 x 10-5. %3D a) What is the initial pH? (Be able to write the reaction responsible for the initial pH!) b) Determine whether the pH at the equivalence point is >, <, or = 7.00. (Be able to write BOTH the titration reaction & the reaction that is responsible for the pH at the equivalence point!)
book bus ng over 4 The following titration curve depicts the titration of a weak base with a strong acid. Which of the labeled points is the equivalence point. P H 12 10 8 6 s 2 0 3 ** 5 O II only OV only O IV only O I only III only I 18 10 [[ 15 IV 23 **** ++ 25 IL NaOH 111 20 35 40 45 50
What's the ph after adding a) 20ml of base b) 25ml of base Im having trouble with the excess base concept. Thank u
QUESTION 1 Calculate the pH after addition of 24.38 mL of 0.1148 M HCIO4 to 25.00 mL of 0.1989 M CH3CH2NH2. Kы(CH3CH2NH2) = 6.400e- 4. Key Concept: Titration of a weak base by a strong acid. Up to just before the equivalence point, the Henderson-Hasselbach equation can be used to determine pH. Although this is not the normal form it works quite nicely: pH = pKa - log(nb/na) Strategy Calculate initial mol of base, calculate mole of acid added →nb = initial mol of base minus mol acid added; na = mol of acid added.;
None
Part 1: A 42.50-mL sample of 0.0527 M HF (Ka = 6.6 10-4) was titrated with a 0.0600-M KOH solution. What would be the equivalence point of this titration? Part 2: (This is the follow-up question of part 1) What would be the pH of the titree solution at the equivalence point? Please solve part 2