   Chapter 15, Problem 100AP ### Introductory Chemistry: A Foundati...

9th Edition
Steven S. Zumdahl + 1 other
ISBN: 9781337399425

#### Solutions

Chapter
Section ### Introductory Chemistry: A Foundati...

9th Edition
Steven S. Zumdahl + 1 other
ISBN: 9781337399425
Textbook Problem
1 views

# The concentration of a solution of HCl is 33. 1 % by mass, and its density was measured to be 1.147 g/mL. How many milliliters of the HCl solution are required to obtain 10.0 g of HCI?

Interpretation Introduction

Interpretation:

The milliliters of HCl solution required to obtain 10.0g of HCl is to be calculated.

Concept Introduction:

Solution is composed of solute and solvent particles. Solute particles are always present in lower amount as compared to amount of the solvent in the solution. The atomic mass of an element is defined as the sum of number of protons and number of neutrons. Molar mass of an element is determined from atomic mass of an element.

The molarity is calculated by the formula,

Molarity=NumberofmolesofsoluteVolumeofsolutionL.

Explanation

The mass, mass percent and density of HCl is given to be 10.0g, 33.1% and 1.147g/mL respectively.

The mass of solution needed to get 10.0g of HCl is calculated by the formula,

Massofsolution=MassofHCl×100MasspercentofHCl        (1)

Substitute the values of mass and mass percent of HCl in the equation (1).

Massofsolution=10g×10033

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