Consider the titration of 250.0 mL of 0.150 M HNO3 by 0.55 M NaOH. 1) Calculate the pH after 50.0 mL of NaOH has been added. 2) What volume of NaOH must be added so that the pH = 7.00?
Consider the titration of 250.0 mL of 0.150 M HNO3 by 0.55 M NaOH. 1) Calculate the pH after 50.0 mL of NaOH has been added. 2) What volume of NaOH must be added so that the pH = 7.00?
Chemistry: Principles and Reactions
8th Edition
ISBN:9781305079373
Author:William L. Masterton, Cecile N. Hurley
Publisher:William L. Masterton, Cecile N. Hurley
Chapter14: Equilibria In Acid-base Solutions
Section: Chapter Questions
Problem 70QAP: Consider the titration of HF (K a=6.7104) with NaOH. What is the pH when a third of the acid has...
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Step 1: Defining pH
VIEWStep 2: Calculation for moles of nitric acid and NaOH used!
VIEWStep 3: Finding out the remaining concentration of nitric acid!
VIEWStep 4: Calculation for pH after addition of 50.0 mL NaOH
VIEWStep 5: Calculation for volume of NaOH required to reach the equivalence point!
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