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For an acid-base titration, the moles of the acid should be equal the moles of the base. 30 mL of aliquot of a 0.23N HCl is placed in an Erlenmeyer flask and 2 drops of phenolphthalein was added. It was titrated and had an intial reading of 15.8 The normality of the solution is found to be 0.52N. (a) How much of the NaOH solution is used for the titration? (b) What is the final reading on the buret?

For an acid-base titration, the moles of the acid should be equal the moles of the base. 30 mL of aliquot of a 0.23N HCl is placed in an Erlenmeyer flask and 2 drops of phenolphthalein was added. It was titrated and had an intial reading of 15.8 The normality of the solution is found to be 0.52N. (a) How much of the NaOH solution is used for the titration? (b) What is the final reading on the buret?

Chemistry: Principles and Practice
Chemistry: Principles and Practice
3rd Edition
ISBN:9780534420123
Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer
Publisher:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer
Chapter18: Electrochemistry
Section: Chapter Questions
Problem 18.103QE
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For an acid-base titration, the moles of the acid should be equal the moles of the base. 30 mL of aliquot of a 0.23N HCl is placed in an Erlenmeyer flask and 2 drops of phenolphthalein was added. It was titrated and had an intial reading of 15.8 The normality of the solution is found to be 0.52N. (a) How much of the NaOH solution is used for the titration? (b) What is the final reading on the buret?

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