What is the boiling point when 11.89 g of K3PO4 (formula mass = 212.30 g/mol) is dissolved in 165.83 g H2O? The boiling point elevation constant is 0.5100 (°C*kg)/mol. Assume any salt is completely ionic!
What is the boiling point when 11.89 g of K3PO4 (formula mass = 212.30 g/mol) is dissolved in 165.83 g H2O? The boiling point elevation constant is 0.5100 (°C*kg)/mol. Assume any salt is completely ionic!
Chemistry: The Molecular Science
5th Edition
ISBN:9781285199047
Author:John W. Moore, Conrad L. Stanitski
Publisher:John W. Moore, Conrad L. Stanitski
Chapter13: The Chemistry Of Solutes And Solutions
Section13.7: Colligative Properties Of Solutions
Problem 13.15E
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What is the boiling point when 11.89 g of K3PO4 (formula mass = 212.30 g/mol) is dissolved in 165.83 g H2O? The boiling point elevation constant is 0.5100 (°C*kg)/mol. Assume any salt is completely ionic!
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