A chemist titrates 180.0 mL of a 0.1821 M hydrocyanic acid (HCN) solution with 0.8669 M NAOH solution at 25 °C. Calculate the pH at equivalence. The pK of hydrocyanic acid is 9.21. Round your answer to 2 decimal places. Note for advanced students: you may assume the total volume of the solution equals the initial volume plus the volume of NAOH solution added. dh pH %3D
A chemist titrates 180.0 mL of a 0.1821 M hydrocyanic acid (HCN) solution with 0.8669 M NAOH solution at 25 °C. Calculate the pH at equivalence. The pK of hydrocyanic acid is 9.21. Round your answer to 2 decimal places. Note for advanced students: you may assume the total volume of the solution equals the initial volume plus the volume of NAOH solution added. dh pH %3D
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Chapter16: Acid-base Equilibria
Section: Chapter Questions
Problem 16.149QP: A solution of weak base is titrated to the equivalence point with a strong acid. Which one of the...
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![A chemist titrates 180.0 mL of a 0.1821 M hydrocyanic acid (HCN) solution with 0.8669 M NAOH solution at 25 °C. Calculate the pH at equivalence. The
pK of hydrocyanic acid is 9.21.
Round your answer to 2 decimal places.
Note for advanced students: you may assume the total volume of the solution equals the initial volume plus the volume of NAOH solution added.
pH = 1
Explanation
Check
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Transcribed Image Text:A chemist titrates 180.0 mL of a 0.1821 M hydrocyanic acid (HCN) solution with 0.8669 M NAOH solution at 25 °C. Calculate the pH at equivalence. The
pK of hydrocyanic acid is 9.21.
Round your answer to 2 decimal places.
Note for advanced students: you may assume the total volume of the solution equals the initial volume plus the volume of NAOH solution added.
pH = 1
Explanation
Check
2021 McGraw-Hill Educa
Reserved. Terms of Use
Privacy
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