Consider the titration of a 24.8 mL sample of 0.140 moll-1 LiOH with 0.145 molL-1 HNO3. Determine the initial pH, volume of added acid required to reach the equivalence point, pH at 6.8 mL of added acid, and pH at equivalence point.

Consider the titration of a 24.8 mL sample of 0.140 moll-1 LiOH with 0.145 molL-1 HNO3. Determine the initial pH, volume of added acid required to reach the equivalence point, pH at 6.8 mL of added acid, and pH at equivalence point.

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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Concept explainers

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.

Question

Consider the titration of a 24.8 mL sample of 0.140 molL-1 LiOH with 0.145 molL-1 HNO3. Determine the initial pH, volume of added acid required to reach the equivalence point, pH at 6.8 mL of
added acid, and pH at equivalence point.

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Step 1: Determine the pH of the solution and volume of HNO3 at equivalence point from the given data:

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Step 2: Calculation for initial pH of the solution:

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Step 3: Calculation for volume of HNO3 at equivalence point:

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Step 4: Calculation for pH after add 6.8 mL of HNO3 and at equivalence point:

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