5.00 mL of a 0.30 M HCl solution is titrated with 0.35 M NaOH. What is the pH of the solution after 40.00 mL of the NaOH has been added? 50.00 mL of 0.10 M HNO2 is titrated with a 0.10 M KOH solution. After 25.00 mL of the KOH solution is added, what will be the pH in the titration flask ? Calculate the pH at the equivalence point for the titration of 0.100 M HCl with 25.00 mL of 100 M NH3

Chemistry
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ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
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Chapter1: Chemical Foundations
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Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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  1. 35.00 mL of a 0.30 M HCl solution is titrated with 0.35 M NaOH. What is the pH of the solution after 40.00 mL of the NaOH has been added? 
  2. 50.00 mL of 0.10 M HNO2 is titrated with a 0.10 M KOH solution. After 25.00 mL of the KOH solution is added, what will be the pH in the titration flask ?
  3. Calculate the pH at the equivalence point for the titration of 0.100 M HCl with 25.00 mL of 100 M NH3 .
  4.  
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