42.A buffer is prepared using acetic acid, CH3COOH, (a weak acid, pKa = 4.75) and sodium acetate, CH3COONa (which provides acetate ions, the conjugate base), according to the following proportions: Volume of CH3COOH(aq): 139.0 mLConcentration of CH3COOH(aq): 1.103 M Volume of CH3COONa(aq): 127.0 mLConcentration of CH3COONa(aq): 1.259 M Calculate the pH of this buffer after the addition of 20.00 mL of 3.00 M sodium hydroxide, NaOH, a strong base. 4.38 5.90 4.69 4.81 5.12

Using Henderson - Hasselbalch equation to calculate pH of a buffer Adding strong base will reacts…

Answered: Calculate the pH of this buffer after…

Calculate the pH of this buffer after the addition of 20.00 mL of 3.00 M sodium hydroxide, NaOH, a strong base. 4.38 5.90 4.69 4.81 5.12

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

Chapter16: Reactions Between Acids And Bases

Section: Chapter Questions

Problem 16.102QE

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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.

Question

42.

A buffer is prepared using acetic acid, CH₃COOH, (a weak acid, pK_a = 4.75) and sodium acetate, CH₃COONa (which provides acetate ions, the conjugate base), according to the following proportions:

Volume of CH₃COOH_(aq): 139.0 mL

Concentration of CH₃COOH_(aq): 1.103 M

Volume of CH₃COONa_(aq): 127.0 mL

Concentration of CH₃COONa_(aq): 1.259 M

Calculate the pH of this buffer after the addition of 20.00 mL of 3.00 M sodium hydroxide, NaOH, a strong base.

		4.38
		5.90
		4.69
		4.81
		5.12

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