A 25.31 ml solution of a weak acid, 0.211M, is titrated with 0.338M. The ka of the acid is 1.3 x 10^-7. Calculate the pH after these volumes of NaOH have been added. Round all answers to two decimal places a. 0.00ml added (a) b. 3.16ml added c. at the equivalence point d. 15.96ml
A 25.31 ml solution of a weak acid, 0.211M, is titrated with 0.338M. The ka of the acid is 1.3 x 10^-7. Calculate the pH after these volumes of NaOH have been added. Round all answers to two decimal places a. 0.00ml added (a) b. 3.16ml added c. at the equivalence point d. 15.96ml
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Chapter1: Chemical Foundations
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Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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A 25.31 ml solution of a weak acid, 0.211M, is titrated with 0.338M. The ka of the acid is 1.3 x 10^-7. Calculate the pH after these volumes of NaOH have been added.
Round all answers to two decimal places
a. 0.00ml added (a)
b. 3.16ml added
c. at the equivalence point
d. 15.96ml
Expert Solution
Step 1
Henderson-Hasselbach equation shows the relationship between pH of a solution, the acid dissociation constant and the concentration of acidic ions and the neutral molecule in solution. It is represented as:
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