- 1A certain liquid X has a normal freezing point of –1.00 °C and a freezing point depression constant K,=2.88 °C·kg•mol *.A solution is prepared by dissolving some zinc chloride (ZnCl,) in 350. g of X. This solution freezes at -2.1 °C. Calculatethe mass of ZNC1, that was dissolved.Be sure your answer is rounded to the correct number of significiant digits.alo18.2 gArх10

Given: Normal freezing point of X=-1.00oC Freezing point depression constantKf=2.88oCKgmol-1 Mass…

1 A certain liquid X has a normal freezing point of –1.00 °C and a freezing point depression constant K=2.88 °C•kg•mol A solution is prepared by dissolving some zinc chloride (ZNC1,) in 350. g of X. This solution freezes at -2.1 °C. Calculate the mass of ZnCl, that was dissolved.

1 A certain liquid X has a normal freezing point of –1.00 °C and a freezing point depression constant K=2.88 °C•kg•mol A solution is prepared by dissolving some zinc chloride (ZNC1,) in 350. g of X. This solution freezes at -2.1 °C. Calculate the mass of ZnCl, that was dissolved.

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

Section: Chapter Questions

Problem 27QRT: Refer to Figure 13.10 ( Sec. 13-4b) to answer these questions. (a) Does a saturated solution occur...

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Question

- 1
A certain liquid X has a normal freezing point of –1.00 °C and a freezing point depression constant K,=2.88 °C·kg•mol *.
A solution is prepared by dissolving some zinc chloride (ZnCl,) in 350. g of X. This solution freezes at -2.1 °C. Calculate
the mass of ZNC1, that was dissolved.
Be sure your answer is rounded to the correct number of significiant digits.
alo
18.2 g
Ar
х10

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