1. 75.0 mL of 0.130 M acetic acid (HC₂H₂O₂) solution is titrated with 0.210 M Ba(OH)₂. (K, for HC₂H₂O₂ = 1.8 x 105). a. What is the pH after 8.00 mL of the base has been added? b. How many mL of the base are required to reach equivalence? c. What is the pH at the equivalence point?

1. 75.0 mL of 0.130 M acetic acid (HC₂H₂O₂) solution is titrated with 0.210 M Ba(OH)₂. (K, for HC₂H₂O₂ = 1.8 x 105). a. What is the pH after 8.00 mL of the base has been added? b. How many mL of the base are required to reach equivalence? c. What is the pH at the equivalence point?

Chemistry

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Chapter1: Chemical Foundations

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Acid Base Titration

An acid-base titration is the method of quantitative analysis for determining the concentration of an acid and base by exactly neutralizing it with a standard solution of base or acid having known concentration.

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use ICE table if needed
C
1. 75.0 mL of 0.130 M acetic acid (HC₂H₂O₂) solution is
titrated with 0.210 M Ba(OH)₂. (K for HC₂H₂O₂ = 1.8 x
10-5).
a. What is the pH after 8.00 mL of the base has been
added?
b. How many mL of the base are required to reach
equivalence?
c. What is the pH at the equivalence point?
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Step 3: Determine required Volume of Base to reach equivalence

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