Phosphoric acid (H3PO4) is a triprotic acid with pKa values of 2.12, 7.21, and 12.32. It is a useful buffer solution for pH values near the pKa values. You have a 0.100 M solution of phosphate buffer with a pH of 2.50. How many mL of 0.500 M NaOH solution must be added to 1.00 L of this buffer solution to convert it to a buffer at pH 7.70? Answer in mL

Phosphoric acid (H3PO4) is a triprotic acid with pKa values of 2.12, 7.21, and 12.32. It is a useful buffer solution for pH values near the pKa values. You have a 0.100 M solution of phosphate buffer with a pH of 2.50. How many mL of 0.500 M NaOH solution must be added to 1.00 L of this buffer solution to convert it to a buffer at pH 7.70? Answer in mL

Principles of Modern Chemistry

8th Edition

ISBN:9781305079113

Author:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Publisher:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Chapter15: Acid–base Equilibria

Section: Chapter Questions

Problem 49P

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Question

Phosphoric acid (H3PO4) is a triprotic
acid with pKa values of 2.12, 7.21, and
12.32. It is a useful buffer solution for
pH values near the pKa values. You
have a 0.100 M solution of phosphate
buffer with a pH of 2.50. How many
mL of 0.500 M NaOH solution must be
added to 1.00 L of this buffer solution
to convert it to a buffer at pH 7.70?
Answer in mL

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Step 1: Concept of Molarity

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Step 2: Dissociation reaction of phosphoric acid

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Step 3: Calculation of initial composition of buffer solution

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Step 4: Second dissociation reaction

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Step 5: Calculation of final concentrations

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Step 6: Calculating the moles of hydroxide ions

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Step 7: Calculation of volume of NaOH required

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