1) A 50.0 mL solution of 0.107 M KOH is titrated with 0.214 M HCI. Calculate the pH of the solution after adding each of the given amounts of HCI. a) 0.00 mL b) 7.00 mL c) 12.5 mL d) 19.0 mL e) 24.0 mL f) 25.0 mL

1) A 50.0 mL solution of 0.107 M KOH is titrated with 0.214 M HCI. Calculate the pH of the solution after adding each of the given amounts of HCI. a) 0.00 mL b) 7.00 mL c) 12.5 mL d) 19.0 mL e) 24.0 mL f) 25.0 mL

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

1) A 50.0 mL solution of 0.107 M KOH is titrated with 0.214 M HCI. Calculate the pH of the solution
after adding each of the given amounts of HCI.
a) 0.00 mL
b) 7.00 mL
c) 12.5 mL
d) 19.0 mL
e) 24.0 mL
f) 25.0 mL

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Step 1: Determine the pH of the solution after add each of the given amounts of HCl:

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Step 2: a. Calculation for pH of the solution at 0.00 mL of HCl:

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Step 3: b. Calculation for pH of the solution afer add 7.00 mL of HCl:

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Step 4: c. Calculation for pH of the solution afer add 12.5 mL of HCl:

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Step 5: d. Calculation for pH of the solution afer add 19.0 mL of HCl:

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Step 6: e. Calculation for pH of the solution afer add 24.0 mL of HCl:

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Step 7: f. Calculation for pH of the solution afer add 25.0 mL of HCl:

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