   Chapter 15, Problem 93AP ### 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
113 views

# 93. Calculate the mass of AgCl formed, and the concentration of silver ion remaining in solution, when 10.0 g of solid AgNO3is added to 50. mL of 1.0 × 10 - 2 M NaC1 solution. Assume there is no volume change upon addition of the solid.

Interpretation Introduction

Interpretation:

The mass of AgCl formed and the concentration of silver ion remaining in the solution is to be calculated.

Concept Introduction:

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 number of moles is calculated by the formula,

Moles=MassgMolarmass

Molarity is used to find out the concentration of solution.

The molarity is calculated by the formula,

Molarity=NumberofmolesofsoluteVolumeofsolutionL.

Explanation

The volume and molarity of NaCl solution is given to be 50.mL and 1.0×102M respectively.

The conversion of units of 50.mL into L is done as,

50.mL=50.1000L=0.05L

The balanced chemical equation of sodium chloride and silver nitrate is shown below.

NaClaq+AgNO3sAgCls+NaNO3aq

The concentration of remaining silver ions is to be calculated. It indicates that NaCl behaves as a limiting reactant in the above reaction.

The number of moles of NaCl is calculated by the formula,

NumberofMoles=Volume×Molarity        (1)

Substitute the values of molarity and volume of NaCl solution in the equation (1).

NumberofMoles=0.05L×1.0×102M=0.05×102moles=0.0005moles

The equation exhibits that one equivalent of sodium chloride combines with one equivalent of silver nitrate to form one equivalent of silver chloride. It means for every 0.0005moles of sodium chloride, same moles of silver nitrate are consumed to produce 0.0005moles of silver chloride.

The molar mass of AgCl is 143.32g/mol.

The mass of AgCl is calculated by the formula,

Massg=Moles×Molarmass        (2)

Substitute the values of moles and molar mass of AgCl in the equation (2).

Massg=0.0005moles×143.32g/mol=0.0717g

Therefore, the mass of AgCl formed is 0

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