   Chapter 15, Problem 101AP ### 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

# An experiment calls for 1.00 g of silver nitrate, but all that is available in the laboratory is a 0.50% solution of AgNO3. Assuming the density of the silver nitrate solution to be very nearly that of water because it is so dilute, determine how many mililiters of the solution should be used.

Interpretation Introduction

Interpretation:

The milliliters of the solution that should be used are 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 of AgNO3 and mass percent of AgNO3 solution is given to be 1.00g and 0.50% respectively.

The mass of AgNO3 solution is calculated by the formula,

Massofsolution=MassofAgNO3×100MasspercentofAgNO3        (1)

Substitute the values of mass and mass percent of AgNO3 in the equation (1).

Massofsolution=1.00g×1000.50=200g

Thus, the mass of solution is 200g

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