Introductory Chemistry (5th Edition)

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

Chapter 13 - Solutions - Exercises - Problems: 53

Answer

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.
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