   # What mass of solid AgBr is produced when 100.0 mL of 0.150 M AgNO 3 is added to 20.0 mL of 1.00 M NaBr? ### Chemistry: An Atoms First Approach

2nd Edition
Steven S. Zumdahl + 1 other
Publisher: Cengage Learning
ISBN: 9781305079243

#### Solutions

Chapter
Section ### Chemistry: An Atoms First Approach

2nd Edition
Steven S. Zumdahl + 1 other
Publisher: Cengage Learning
ISBN: 9781305079243
Chapter 6, Problem 61E
Textbook Problem
125 views

## What mass of solid AgBr is produced when 100.0 mL of 0.150 M AgNO3 is added to 20.0 mL of 1.00 M NaBr?

Interpretation Introduction

Interpretation: The produced mass of solid AgBr should be calculated.

Concept Introduction:

Precipitation reaction:

The precipitate will be formed when two soluble salt solutions combined together is called as a precipitation reaction. The amount precipitate will formed by the reaction is deepened on the mole amount of reactant.

Formula:

Mass=Number of mole (mol) ×Molecularweight(g)Limited mole(mol)......(1)

### Explanation of Solution

Explanation

Volume of AgNO3 =0.1L

Molarity of AgNO3 =0.15M

Volume of NaBr =0.02L

Molarity of   NaBr =1.00M

The volume and molarity of NaBr and AgNO3 are recorded as shown above.

Calculate the mole of AgNO3 solution as follows,

Mole=volume×molarityL

Mole of AgNO3 solution = 0.1(L)×0.150(M)1(L)

= 0.015 mole

The values of volume and molarity of AgNO3 solution are plugging in above formula to get mole of AgNO3 The mole of AgNO3 solution is 0.015 mole .

Calculate the moles of NaBr solution as follows,

Mole=volume×molarityL

Mole of NaBr solution = 0

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