   Chapter 12, Problem 12.66QP General Chemistry - Standalone boo...

11th Edition
Steven D. Gammon + 7 others
ISBN: 9781305580343

Solutions

Chapter
Section General Chemistry - Standalone boo...

11th Edition
Steven D. Gammon + 7 others
ISBN: 9781305580343
Textbook Problem

A beverage contains tartaric acid, H2C4H4O6, a substance obtained from grapes during wine making. If the beverage is 0.265 M tartaric acid, what is the molal concentration? The density of the solution is 1.016 g/mL.

Interpretation Introduction

Interpretation:

Molal concentration of aqueous tartaric acid has to be calculated.

Concept Introduction:

Molality is one of the many parameters that is used to express concentration of a solution.  It is expressed as,

Molality = number of moles of solutemass of solvent in kg

Molarity is one of the many parameters that is used to express concentration of a solution.  It is expressed as,

Molarity = number of moles of solutevolume of solution in L

Explanation

Aqueous solution of tartaric acid in grapes is used in wine making. To determine the molal concentration of aqueous tartaric acid we need to know the volume of the solution.  Volume of the solution is equivalent to mass of the solution divided by density of the solution since density = massvolume .  Mass of the solution is equivalent to sum of the mass of solute tartaric acid and mass of the solvent water.  Hence we first need to calculate the mass of the solution.

Given:

The molar concentration of aqueous solution of tartaric acid is 0.265 M .

no. of moles of tartaric acid = mass of tartaric acidmolar mass of tartaric acid

mass of tartaric acid in 0.265 M aqueous solution  = no. of moles of tartaric acid × molar mass of tartaric acid = 0.265 mol × 150.087 g/mol = 39.77 g

Considering one liter of solution,

Mass of the solution = density of solution × volume of solution                                  = 1

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