Q2/ The aluminum content of an alloy is determined gravimetrically by precipi- tating it with 8-hydroxyquinoline (oxine) to give Al(C,H,ON)3. If a 1.021-g sample yielded 0.1862 g of precipitate. what is the percent aluminum in the alloy?

Q2/ The aluminum content of an alloy is determined gravimetrically by precipi- tating it with 8-hydroxyquinoline (oxine) to give Al(C,H,ON)3. If a 1.021-g sample yielded 0.1862 g of precipitate. what is the percent aluminum in the alloy?

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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Question

icel Chiemistry
nalytical Chemistry
Sheet No. 2
What weight of pyrite ore (impure FeS,) must be taken for analysis so that the
BASO, precipitate weight obtained will be equal to one-half that of the percent S
in the sample? NAr
Q2/
The aluminum content of an alloy is determined gravimetrically by precipi-
tating it with 8-hydroxyquinoline (oxine) to give Al(C,H,ON). If a 1.021-g
sample yielded 0.1862 g of precipitate. what is the percent aluminum in the
alloy?
Q3/
A mixture containing only BaO and CaO weighs 2.00 g. The oxides are con-
verted to the corresponding mixed sulfates, which weigh 4.00 g. Calculate the
percent Ba and Ca in the original mixture.
04/ A sample of 0.676g of an unknown compound containing barium jons
excess of NazSO4. If the mass
(Ba) is dissolved in water and treated with
the original unknown compound?

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Please don't provide handwriting solution
Jack was asked to determine iron (55.845 g/mol) content in dietary supplement. He tookfew random tablets and ground them into fine powder. Next, he weighed 3.116 g of thefine powder. Sample was dissolved and iron was precipitated as Fe(OH)3 (106.867 g/mol).The precipitate was then ignited to a constant weight of 0.355 g as Fe2O3 (159.69 g/mol).Report the iron content in dietary supplement as % w/w FeSO4·7H2O (278.01 g/mol).
A powder contains FeSO4⋅7H2OFeSO4⋅7H2O (molar mass=278.01 g/mol),(molar mass=278.01 g/mol), among other components. A 2.880 g2.880 g sample of the powder was dissolved in HNO3HNO3 and heated to convert all iron to Fe3+.Fe3+. The addition of NH3NH3 precipitated Fe2O3⋅?H2O,Fe2O3⋅xH2O, which was subsequently ignited to produce 0.406 g Fe2O3.0.406 g Fe2O3. What was the mass of FeSO4⋅7H2OFeSO4⋅7H2O in the 2.880 g2.880 g sample?
Number 3.