Calculate the pH during the titration of 20.0 mL of 0.500 M formic acid ( Ka =
Question:
Calculate the pH during the titration of 20.0 mL of 0.500 M formic acid ( Ka = 1.8 × 10-4) with 0.500 M NaOH. Calculate the pH after 0, 10.0, 20.0, and 30.0 mL of NaOH have been added, and sketch the titration curve.
Strategy
First, write the chemical equation for the titration and calculate the equivalence point. We will use an sRfc table to determine which species are present after adding titrant. Once we know which species are present, we will determine whether the system contains a strong acid or base, a weak acid or base, a buffer, or just water (including spectator ions). We already know how to calculate the pH of each of these systems.
Step by Step Answer:
Write the chemical equation to calculate the equivalence point before beginning to calculate the pH of the solution If we know the equivalence point we can estimate the pH and determine whether the re...View the full answer
Chemistry Principles And Practice
ISBN: 9780534420123
3rd Edition
Authors: Daniel L. Reger, Scott R. Goode, David W. Ball
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