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A 3.87 g sample of a hydrate of MnCl2 was heated to drive off the water. The anhydrous powder weighed 2.46 g. Determine the amount of water lost and calculate the number of moles of water there are to every one mole of the hydrate.

A 3.87 g sample of a hydrate of MnCl2 was heated to drive off the water. The anhydrous powder weighed 2.46 g. Determine the amount of water lost and calculate the number of moles of water there are to every one mole of the hydrate.

Chemistry: Principles and Practice
Chemistry: Principles and Practice
3rd Edition
ISBN:9780534420123
Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer
Publisher:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer
Chapter4: Chemical Reactions In Solution
Section: Chapter Questions
Problem 4.117QE
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1. A certain hydrate salt that has molar mass 474 g/mole consists of 45.6 % water. Calculate the number of water moles there are to every one mole of the salt. omaunt = 45.6x4nTg/mol of woter 100 = M0.144 g/ml molor mas s of water= 18,9mol number of water molas = loil44g/mol =12 18 gmol 2. A 3.87 g sample of a hydrate of MnCl2 was heated to drive off the water. The anhydrous powder weighed 2.46 g. Determine the amount of water lost and calculate the number of moles of water there are to every one mole of the hydrate.
Transcribed Image Text:1. A certain hydrate salt that has molar mass 474 g/mole consists of 45.6 % water. Calculate the number of water moles there are to every one mole of the salt. omaunt = 45.6x4nTg/mol of woter 100 = M0.144 g/ml molor mas s of water= 18,9mol number of water molas = loil44g/mol =12 18 gmol 2. A 3.87 g sample of a hydrate of MnCl2 was heated to drive off the water. The anhydrous powder weighed 2.46 g. Determine the amount of water lost and calculate the number of moles of water there are to every one mole of the hydrate.
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