The pH of a white vinegar solution is 2.57. This vinegar is an aqueous solution of acetic acid with a density of 1.09 g/mL. What is the mass percentage of acetic acid in the solution? K. (acetic acid) = 1.8 x 10 5 Mass percentage = %

The pH of a white vinegar solution is 2.57. This vinegar is an aqueous solution of acetic acid with a density of 1.09 g/mL. What is the mass percentage of acetic acid in the solution? K. (acetic acid) = 1.8 x 10 5 Mass percentage = %

Chemistry: Principles and Reactions

8th Edition

ISBN:9781305079373

Author:William L. Masterton, Cecile N. Hurley

Publisher:William L. Masterton, Cecile N. Hurley

Chapter10: Solutions

Section: Chapter Questions

Problem 65QAP: Twenty-five milliliters of a solution (d=1.107g/mL)containing 15.25% by mass of sulfuric acid is...

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Concept explainers

Ionic Equilibrium

Chemical equilibrium and ionic equilibrium are two major concepts in chemistry. Ionic equilibrium deals with the equilibrium involved in an ionization process while chemical equilibrium deals with the equilibrium during a chemical change. Ionic equilibrium is established between the ions and unionized species in a system. Understanding the concept of ionic equilibrium is very important to answer the questions related to certain chemical reactions in chemistry.

Arrhenius Acid

Arrhenius acid act as a good electrolyte as it dissociates to its respective ions in the aqueous solutions. Keeping it similar to the general acid properties, Arrhenius acid also neutralizes bases and turns litmus paper into red.

Bronsted Lowry Base In Inorganic Chemistry

Bronsted-Lowry base in inorganic chemistry is any chemical substance that can accept a proton from the other chemical substance it is reacting with.

Question

The pH of a white vinegar solution is 2.57. This vinegar is an aqueous solution of acetic
acid with a density of 1.09 g/mL. What is the mass percentage of acetic acid in the
solution?
K. (acetic acid) = 1.8 x
Mass percentage =
%

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