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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2. Calculate the volume of the salt preparation of 200 ml of the following buffer solutions. S BUFFER DESIRED NUMBER pH 5 Tale 6 7 8 210 6.90 7.18 9.45 8.25 0.1M SOLUTIONS TOT NaH₂PO4/Na₂HPO4 NaH₂PO4/Na₂HPO4 NH4CI/NH3 NH4CI/NH3 pka to be used in the 6.80 6.80 9.30 9.30 VOLUME OF SALT (ml)
New 27/8/2021. A buffer of acetic acid and sodium acetate (pH = 5.2) is prepared by mixing the calculated quantities of two acid/base pair and adjust to the desired pH with pH meter by adding Select one: a. Any weak base b. Any weak acid c. Acetic acid or sodium acetate O d. Strong acid or strong base
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O D. 8.70 x 10-13 M 38. Determine the pH of 0.42 M for formic acid, HCOOH solution. The value of pKa for HCOOH is 3.75. * O A. 0.38 Ов. 206 C. 5.32 D. 11.94 orminc the pH of a buffer solution containing 0.2 mole of NH.Cl and
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
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Solve 16. 8
A. Preparation of reagents Standard HCI solution Compute for the volume of concentrated HCI needed to prepare 500 mL of 0.1000 M HCI solution. Prepare the solution accurately. • NaCl solution Compute for the weight of NaCl needed to prepare 250 mL of 0.05 M NaCI solution. Prepare the solution accurately. B. Correction factor for indicator Determine the indicator correction by titrating approximetely 100 ml of 0.05 NaCl and 3 drops of indicator. Boil briefly, cool, and then complete the titration. Determine the volume of HCI that react with the indicator. You may do one to two replicates for this part
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
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