Example: A solution buffered at pH 3.90 is needed for a reaction.Would formic acid and its salt, sodium formate, make a good choicefor this buffer? If so what would be a good salt, and how much ofeach should be used?pH = pKa + 1Where does ±1 come from?For formic acid, K, = 1.8 x 10 -4, thereforetion Let's extend the problem to find out how to make 0.500 liters of thisbuffer containing 0.250 mol HCOOH. How many grams ofNaCHOO are required? (molar mass = 68.02 g/mol)

Given: A solution buffered at pH 3.90 is required for a reaction. ka of formic acid is 1.8 x 10-4

Example: A solution buffered at pH 3.90 is needed for a reaction. Would formic acid and its salt, sodium formate, make a good choice for this buffer? If so what would be a good salt, and how much of each should be used? pH = pKa + 1 Where does ±1 come from?

Example: A solution buffered at pH 3.90 is needed for a reaction. Would formic acid and its salt, sodium formate, make a good choice for this buffer? If so what would be a good salt, and how much of each should be used? pH = pKa + 1 Where does ±1 come from?

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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Example: A solution buffered at pH 3.90 is needed for a reaction.
Would formic acid and its salt, sodium formate, make a good choice
for this buffer? If so what would be a good salt, and how much of
each should be used?
pH = pKa + 1
Where does ±1 come from?
For formic acid, K, = 1.8 x 10 -4, therefore
tion

Let's extend the problem to find out how to make 0.500 liters of this
buffer containing 0.250 mol HCOOH. How many grams of
NaCHOO are required? (molar mass = 68.02 g/mol)

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