During the titration of 50.0mL of 0.1098M HCl using a standardized 0.0750M NaOH solution, what would be the pH of the solution (round off to 2 decimal points) after the addition of: a.) 0.00mL NaOH total volume? b.) 50.0mLNaOHtotalvolume? c.) 75.0mL NaOH total volume? d.) 100.mLNaOHtotalvolume?
During the titration of 50.0mL of 0.1098M HCl using a standardized 0.0750M NaOH solution, what would be the pH of the solution (round off to 2 decimal points) after the addition of: a.) 0.00mL NaOH total volume? b.) 50.0mLNaOHtotalvolume? c.) 75.0mL NaOH total volume? d.) 100.mLNaOHtotalvolume?
Chemistry by OpenStax (2015-05-04)
1st Edition
ISBN:9781938168390
Author:Klaus Theopold, Richard H Langley, Paul Flowers, William R. Robinson, Mark Blaser
Publisher:Klaus Theopold, Richard H Langley, Paul Flowers, William R. Robinson, Mark Blaser
Chapter14: Acid-base Equilibria
Section: Chapter Questions
Problem 100E: What mass of NH4Cl must be added to 0.750 L of a 0.100-M solution of NH3 to give a buffer solution...
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During the titration of 50.0mL of 0.1098M HCl using a standardized 0.0750M NaOH solution, what would be the pH of the solution (round off to 2 decimal points) after the addition of:
a.) 0.00mL NaOH total volume?
b.) 50.0mLNaOHtotalvolume?
c.) 75.0mL NaOH total volume?
d.) 100.mLNaOHtotalvolume?
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