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A certain liquid X has a normal boiling point of 95.40 °C and a boiling point elevation constant K, =0.75 °C·kg•mol 1 . A solution is prepared by dissolving some zinc chloride (ZnCl,) in 400. g of X. This solution boils at 96.5 °C. Calculate the mass of ZnCl, that was dissolved. Round your answer to 2 significant digits. alo Ar g x10

A certain liquid X has a normal boiling point of 95.40 °C and a boiling point elevation constant K, =0.75 °C·kg•mol 1 . A solution is prepared by dissolving some zinc chloride (ZnCl,) in 400. g of X. This solution boils at 96.5 °C. Calculate the mass of ZnCl, that was dissolved. Round your answer to 2 significant digits. alo Ar g x10

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Chemistry
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ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
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- 1 A certain liquid X has a normal boiling point of 95.40 °C and a boiling point elevation constant K,=0.75 °C•kg•mol A solution is prepared by dissolving some zinc chloride (ZNCI,) in 400. g of X. This solution boils at 96.5 °C. Calculate the mass of ZnCl, that was dissolved. Round your answer to 2 significant digits. olo Ar x10 ?
Transcribed Image Text:- 1 A certain liquid X has a normal boiling point of 95.40 °C and a boiling point elevation constant K,=0.75 °C•kg•mol A solution is prepared by dissolving some zinc chloride (ZNCI,) in 400. g of X. This solution boils at 96.5 °C. Calculate the mass of ZnCl, that was dissolved. Round your answer to 2 significant digits. olo Ar x10 ?
Expert Solution
Step 1

Given, 

Normal boiling point of X liquid, Tb = 95.40 °C 

Boiling point of solution, Tb' = 96.5 °C 

Elevation of boiling point, ∆Tb = Tb' - Tb

                                                       = (96.5 - 95.40)

                                                       = 1.1 °C 

Weight of liquid X, W1 = 400 g 

Kb = 0.75 °C.kg.mol-1

Molar mass of ZnCl2 , M2 = 136.286 g/mol

 

 

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