a) Patients who have a zinc deficiency can take tablets consisting of a hydrated zinc sulfate, ZnSO4.xH₂O, to treat this problem. A pharmacist heated a 5.073g sample of hydrated zinc sulfate. After heating, the mass of the remaining anhydrous zinc sulfate was 2.848g. Use this information to determine the value of x in this hydrated salt. b) In a second experiment to verify the value of x, the pharmacist reacted a 7.579g sample of the hydrated zinc sulfate with a small excess of powdered magnesium. This should reduce all of the Zn²+ ions to Zn(s): ZnSO4.xH₂O + Mg → Zn + MgSO4 + xH₂O The solid zinc product was dried and weighed, and was found to have a mass of 1.630g. Use this information to obtain the moles and molar mass of the ZnSO4.xH₂O in the sample and hence find the value of x. You must show all of your working out. Make sure you use accurate values of molar and atomic masses. c) You should find that the values of x obtained by the two experiments do not exactly agree. Give three suggestions to explain this, based on the experimental procedures.
a) Patients who have a zinc deficiency can take tablets consisting of a hydrated zinc sulfate, ZnSO4.xH₂O, to treat this problem. A pharmacist heated a 5.073g sample of hydrated zinc sulfate. After heating, the mass of the remaining anhydrous zinc sulfate was 2.848g. Use this information to determine the value of x in this hydrated salt. b) In a second experiment to verify the value of x, the pharmacist reacted a 7.579g sample of the hydrated zinc sulfate with a small excess of powdered magnesium. This should reduce all of the Zn²+ ions to Zn(s): ZnSO4.xH₂O + Mg → Zn + MgSO4 + xH₂O The solid zinc product was dried and weighed, and was found to have a mass of 1.630g. Use this information to obtain the moles and molar mass of the ZnSO4.xH₂O in the sample and hence find the value of x. You must show all of your working out. Make sure you use accurate values of molar and atomic masses. c) You should find that the values of x obtained by the two experiments do not exactly agree. Give three suggestions to explain this, based on the experimental procedures.
Chemistry for Engineering Students
4th Edition
ISBN:9781337398909
Author:Lawrence S. Brown, Tom Holme
Publisher:Lawrence S. Brown, Tom Holme
Chapter3: Molecules, Moles, And Chemical Equations
Section: Chapter Questions
Problem 3.112PAE: 3.112 In one experiment, the burning of 0.614 g of sulfur produced 1.246 g of sulfur dioxide as its...
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Transcribed Image Text:Question 4
a) Patients who have a zinc deficiency can take tablets consisting of a hydrated zinc sulfate,
ZnSO4.xH₂O, to treat this problem. A pharmacist heated a 5.073g sample of hydrated zinc sulfate.
After heating, the mass of the remaining anhydrous zinc sulfate was 2.848g. Use this
information to determine the value of x in this hydrated salt.
b) In a second experiment to verify the value of x, the pharmacist reacted a 7.579g sample of the
hydrated zinc sulfate with a small excess of powdered magnesium. This should reduce all of the
Zn²+ ions to Zn(s):
ZnSO4.xH₂O + Mg → Zn + MgSO4 + xH₂0
The solid zinc product was dried and weighed, and was found to have a mass of 1.630g. Use this
information to obtain the moles and molar mass of the ZnSO4.xH₂O in the sample and hence find
the value of x. You must show all of your working out. Make sure you use accurate values of
molar and atomic masses.
c) You should find that the values of x obtained by the two experiments do not exactly agree.
Give three suggestions to explain this, based on the experimental procedures.
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