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3) into a 1.000 liter volumetric flask, and suddenly realize that you don’t have all the reagents you expected to have. Looking around, you find a large carboy of 1.00 M Na2CO3. How much of this Na2CO3 solution should you add to your volumetric flask such that when it is diluted with water to the 1 liter calibration mark, the pH is 6.00 ? You may treat sulfuric acid as if it has completely dissociated (acting as a “strong acid"). Suppose you wanted to make a pH=6.0 buffer. You pipette 50 ml of 1.00 M H2SO4

3) into a 1.000 liter volumetric flask, and suddenly realize that you don’t have all the reagents you expected to have. Looking around, you find a large carboy of 1.00 M Na2CO3. How much of this Na2CO3 solution should you add to your volumetric flask such that when it is diluted with water to the 1 liter calibration mark, the pH is 6.00 ? You may treat sulfuric acid as if it has completely dissociated (acting as a “strong acid"). Suppose you wanted to make a pH=6.0 buffer. You pipette 50 ml of 1.00 M H2SO4

Chemistry
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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Do you have any ideas on 4a)????
TI O Aa v f) What is the predominant speciation (e.g., protonated or deprotonated) for each of the acids and bases in your system? You should not need to so a calculation for this. Explain your reasoning. 3) into a 1.000 liter volumetric flask, and suddenly realize that you don’t have all the reagents you expected to have. Looking around, you find a large carboy of 1.00 M N22CO3. How much of this Na2CO3 solution should you add to your volumetric flask such that when it is diluted with water to the 1 liter calibration mark, the pH is 6.00 ? You may treat sulfuric acid as if it has completely dissociated (acting as a "strong acid"). Suppose you wanted to make a pH=6.0 buffer. You pipette 50 ml of 1.00 M H2SO4 4) A volumetric flask contains 0.12 mole NaHCO3, 0.17 mole Na3PO4, and 0.030 mole sodium formate. You want to have a pH of 8.00 after dilution, but you recognize that the solution as is will not give you the correct pH. You have on hand 1.00 M NAOH and 1.00 M HCL. 4а) volume should Which reagent (NAOH or HCl) should you add to the volumetric flask, and what you add, such that after this addition and filling the volumetric to the calibration line, the pH is 8.00? 山T四0@ 22 étv W
Transcribed Image Text:TI O Aa v f) What is the predominant speciation (e.g., protonated or deprotonated) for each of the acids and bases in your system? You should not need to so a calculation for this. Explain your reasoning. 3) into a 1.000 liter volumetric flask, and suddenly realize that you don’t have all the reagents you expected to have. Looking around, you find a large carboy of 1.00 M N22CO3. How much of this Na2CO3 solution should you add to your volumetric flask such that when it is diluted with water to the 1 liter calibration mark, the pH is 6.00 ? You may treat sulfuric acid as if it has completely dissociated (acting as a "strong acid"). Suppose you wanted to make a pH=6.0 buffer. You pipette 50 ml of 1.00 M H2SO4 4) A volumetric flask contains 0.12 mole NaHCO3, 0.17 mole Na3PO4, and 0.030 mole sodium formate. You want to have a pH of 8.00 after dilution, but you recognize that the solution as is will not give you the correct pH. You have on hand 1.00 M NAOH and 1.00 M HCL. 4а) volume should Which reagent (NAOH or HCl) should you add to the volumetric flask, and what you add, such that after this addition and filling the volumetric to the calibration line, the pH is 8.00? 山T四0@ 22 étv W
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