Your goal is to make a buffer with a pH of 4.75 from acetic acid and sodium acetate. Assume the pKa for acetic acid is 4.74. What is the volume of 1 M sodium acetate added to make your buffer? Report your answer to the tenths place. To do this, we use the Henderson-Hasselbach Equation pH = pkA + log (base/acid) where pkA = 4.74 for acetic acid, pH = target pH and [base] /[acid] = x/(1-x) since we don't know the concentration of the base, we will call it x the acid is just 1-x, assuming the two add up to 100% solve for x, and then you know the mL of base and acid to add.
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Chemical equilibrium and ionic equilibrium are two major concepts in chemistry. Ionic equilibrium deals with the equilibrium involved in an ionization process while chemical equilibrium deals with the equilibrium during a chemical change. Ionic equilibrium is established between the ions and unionized species in a system. Understanding the concept of ionic equilibrium is very important to answer the questions related to certain chemical reactions in chemistry.
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To do this, we use the Henderson-Hasselbach Equation
pH = pkA + log (base/acid)
where pkA = 4.74 for acetic acid,
pH = target pH
and [base] /[acid] = x/(1-x)
since we don't know the concentration of the base, we will call it x
the acid is just 1-x, assuming the two add up to 100%
solve for x, and then you know the mL of base and acid to add.
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