QUESTION 42 Buffer preparation: A 6.90 g sample of sodium nitrite (NaNO2. 68.995) was dissolved in about 100 mL of water. To this was added 500 ml of 0.200 M nitrous acid (HNO₂. pkg = 3.34) and the total volume was brought to 1.00 L by adding distilled water. (hint calculate the molarites of the two buffer components first) Addition of a strong base to the buffer: To the entire solution of this buffer solution was added 0.056 mol KOH (s). There is no detetable change in volume as a result of this additoin The pH of the buffer +KOH solution is Write down your work to upload in the following "File Response" question.

QUESTION 42 Buffer preparation: A 6.90 g sample of sodium nitrite (NaNO2. 68.995) was dissolved in about 100 mL of water. To this was added 500 ml of 0.200 M nitrous acid (HNO₂. pkg = 3.34) and the total volume was brought to 1.00 L by adding distilled water. (hint calculate the molarites of the two buffer components first) Addition of a strong base to the buffer: To the entire solution of this buffer solution was added 0.056 mol KOH (s). There is no detetable change in volume as a result of this additoin The pH of the buffer +KOH solution is Write down your work to upload in the following "File Response" question.

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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Question 6
1. What would be the pH of buffer containing 137ml of 3.50M boric acid and 228ml of 1.90M lithium borate. The pKa of buffer system is 13.80. solved answer pH= 13.76 2. What would be the pH of the buffer from question 1, after adding 84.5ml of 0.71 M KOH (strong base) to buffer? ??
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You are given 60 mL of 0.50 M phosphate buffer, pH = 6.83, to test. The starting composition of the buffer, both in terms of the concentration and the molar quantity of the two major phosphate species, is: Concentration of HPO42−: 0.304 M Molar quantity of HPO42−: 18.2 mmol Concentration of H2PO4−: 0.196 M Molar quantity of H2PO4−: 11.8 mmol You add 1.7 mL of 1.00 M HCl to the buffer. Calculate the molar quantity of H3O+ added as HCl, and the final molar quantity of HPO42− and H2PO4− at equilibrium. H3O+ = HPO42− = H2PO4− = What is the new HPO42−/H2PO4− ratio, and the new pH of the solution? The pKa of H2PO4− is 6.64. Use the Henderson-Hasselbalch equation to calculate the new pH. Now take a fresh 60 mL of the 0.50 M pH 6.83 buffer and add 3.7 mL of 1.00 M NaOH. Using steps similar to those above, calculate the new pH of the solution.
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A student prepared 100.0 mL of a buffer in the lab that contains 0.300 M of a weak acid, HA, and 0.200 M of its conjugate base, NaA. The student then added 1.0x10 moles of NaOH to the buffer. a) Write down your student name and number b) Write down how the student calculated the final moles of A and HA after adding the NaOH: moles A finl =2.0x102 mole - 1.0x10-3mole moles HA na = 3.0x102mole +1.0x10-3mole c) There is an error in their formula. Identify the error d) Calculate the correct final moles of A and HA
A buffer solution contains 0.201 M CH3NH3 Br and 0.486 M CH3NH2 (methylamine). Determine the pH change when 0.115 mol HBr is added to 1.00 L of the buffer. (Assume Kb (CH3NH₂) = 4.2 × 10-4.) pH after addition change = Submit Answer - pH before addition = pH Retry Entire Group 9 more group attempts remaining D
#9 plz