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, yêu 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, yêu 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

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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Any ideas on #3??

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, ysu 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
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 HCI.
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