4. Describe the pH changes as large or small in the vicinity of the: Tiratien of l.of a a. equivalence point Ek A pll b. half-equivalence point 5. Refer to the figure to answer the questions a & b. a. What is the pk, of the unknown acid? b. What is the K, of the unknown acid? 6. Two unknown, weak, monoprotic acids of equal concentration were titrated separately with NaOH. Upon evaluation, the titration curves revealed that the pk, of Acid 1 is 8.1 and the pk, of Acid 2 is 5.8. so 100 150 200 afeseM NaOl added Which acid is the stronger acid?

4. Describe the pH changes as large or small in the vicinity of the: Tiratien of l.of a a. equivalence point Ek A pll b. half-equivalence point 5. Refer to the figure to answer the questions a & b. a. What is the pk, of the unknown acid? b. What is the K, of the unknown acid? 6. Two unknown, weak, monoprotic acids of equal concentration were titrated separately with NaOH. Upon evaluation, the titration curves revealed that the pk, of Acid 1 is 8.1 and the pk, of Acid 2 is 5.8. so 100 150 200 afeseM NaOl added Which acid is the stronger acid?

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...

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Concept explainers

Acid Base Titration

An acid-base titration is the method of quantitative analysis for determining the concentration of an acid and base by exactly neutralizing it with a standard solution of base or acid having known concentration.

Question

4. Describe the pH changes as large or small in the vicinity of the:
Titration of 10 ml. of an
a. equivalence point
pll
b. half-equivalence point
5. Refer to the figure to answer the questions a & b.
a. What is the pk, of the unknown acid?
b. What is the K, of the unknown acid?
6. Two unknown, weak, monoprotic acids of equal concentration were
titrated separately with NaOH. Upon evaluation, the titration curves
revealed that the pk, of Acid 1 is 8.1 and the pk, of Acid 2 is 5.8.
• s0 100 150
200
al. ef00M NuOl added
Which acid is the stronger acid?

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5 Please answer all questions. Thanks
Give detailed Solution..no need handwritten answer (don't use Ai for answering this)
pH 14 12 10 8 6. 4 2- 0 0 10 20 30 Volume of NaOH (mL) 40 550
At each stage of the titration: A. Determine the amount (mol) of weak acid, weak base, and strong acid present. B. Determine the total volume of the combined solutions. C. Determine [H;O*] or [OH], whichever predominates, using the total volume and the nature of the solution: weak base, buffer, weak acid, or strong acid. D. Calculate pH. Determine the pH during the titration of 37.3 mL of 0.336 M methylamine (CH3NH2, K, = 4.2x10-4) by 0.336 M HI at the following points. (Assume the titration is done at 25 °C.) Note that state symbols are not shown for species in this problem. (a) Before the addition of any HI 12.067 (b) After the addition of 16.2 mL of HI 10.74 (c) At the titration midpoint 10.62 (d) At the equivalence point (e) After adding 56.0 mL of HI
Solve 16. 8
Look up the formula of the following compounds often found in buffers:a. acetic acidb. sodium acetatec. phosphoric acidd. monopotassium phosphate (also known as potassium dihydrogen phosphate)e. dipotassium phosphate
Which of the following statements is TRUE if a pH indicator was NOT added before titration? a. The concentration of the analyte will be lower than the actual. b. Equivalence point could not be determined c. Endpoint can be observed. d. The concentration of the analyte will be higher than the actual.
Calculate the pH during the titration of 20.00 mL of0.1 M NaOH with 0.100 M HCl after theaddition of the following volumes of reagent:a. 0.00 mLb. 10.00 mLc. 15.00 mLd. 20.00 mLe. 24.5 mLf. 25.00 mLg. 30 mLh. 35 mL