1. A 40.00 mL sample of 0.250 MKOH is titrated with 0.200 MHI using phenol red as the indicator (pH range 6.4-8.2). Calculate the pH for the following points in the titration. Hint: first calculate the mol of KOH remaining Total L of HI added 0.00 0.0250 0.0500 0.1000 mol of HI added 0.00 mol of OH- remaining mol of excess H+ [OH-]remaining, M [H+] excess, M pH POH

1. A 40.00 mL sample of 0.250 MKOH is titrated with 0.200 MHI using phenol red as the indicator (pH range 6.4-8.2). Calculate the pH for the following points in the titration. Hint: first calculate the mol of KOH remaining Total L of HI added 0.00 0.0250 0.0500 0.1000 mol of HI added 0.00 mol of OH- remaining mol of excess H+ [OH-]remaining, M [H+] excess, M pH POH

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.

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Exercises:
1. A 40.00 mL sample of 0.250 M KOH is titrated with 0.200 MHI using phenol red as the
indicator (pH range 6.4 - 8.2). Calculate the pH for the following points in the titration.
Hint: first calculate the mol of KOH remaining
Total L of
HI added
0.00
0.0250
0.0500
0.1000
mol of HI
added
0.00
mol of OH-
remaining
mol of excess H+
[OH-]remaining, M
[H+] excess, M
pH
POH

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Step 1: General Formulas in Titrations

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Step 2: pH calculation when 0.00 L HI is added

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Step 3: pH calculation when 0.025 L HI is added

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Step 4: pH calculation when 0.0500 L HI is added

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Step 5: pH calculation when 0.100 L HI is added

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