a) Calculate how much water in mL must be added to dilute 75.0 mL 0.010 M HNO3 to a solution with pH = 3.0. b) Calculate how many grams of CH3CH2COOH must be dissolved in 350.0 mL of water for the solution to have a pH 2.85 at 25oC. = Ka(CH3CH2COOH)=1,35 . 10^-5 ?

a) Calculate how much water in mL must be added to dilute 75.0 mL 0.010 M HNO3 to a solution with pH = 3.0. b) Calculate how many grams of CH3CH2COOH must be dissolved in 350.0 mL of water for the solution to have a pH 2.85 at 25oC. = Ka(CH3CH2COOH)=1,35 . 10^-5 ?

Chemistry: Principles and Reactions

8th Edition

ISBN:9781305079373

Author:William L. Masterton, Cecile N. Hurley

Publisher:William L. Masterton, Cecile N. Hurley

Chapter13: Acids And Bases

Section: Chapter Questions

Problem 108QAP

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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

Any 1 of the following questions

a) Calculate how much water in mL must be
added to dilute 75.0 mL 0.010 M HNO3 to a
solution with pH = 3.0.
b) Calculate how many grams of
CH3CH2COOH must be dissolved in 350.0
mL of water for the solution to have a pH
2.85 at 25oC.
=
Ka(CH3CH2COOH)=1,35 . 10^-5
?

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