Introductory Chemistry (5th Edition)

Published by Pearson
ISBN 10: 032191029X
ISBN 13: 978-0-32191-029-5

Chapter 13 - Solutions - Exercises - Problems - Page 480: 53


1.6x$10^2$ g

Work Step by Step

Since 1 L AgNO3 contains = 1000 mL AgNO3. So 4.8 L AgNO3 contains = 4800 mL AgNO3 4800 mL of AgNO3 solution contains 4800mL of silver. Hence Mass of solution = Volume of solution x density of solution Density of solution = 1.01 g/mL. Mass of 4800 mL of silver solution =4800mL x 1.01g/mL= 4848g silver. Mass percent is the number of grams of solute per 100g of solution. A solution with a concentration of 3.4% silver per 100 g of solution. Hence 4848g of solution are present. This gives: = (3.4g silver/100 g solution)x 4848g solution = 1.6x$10^2$ g AgNO3.
Update this answer!

You can help us out by revising, improving and updating this answer.

Update this answer

After you claim an answer you’ll have 24 hours to send in a draft. An editor will review the submission and either publish your submission or provide feedback.