We want to determine the purity of alum sample bought in a local pharmacy inMiagao. A Chem 28 student determined the purity gravimetrically of a sample of alum,K2SO4:Al2(SO4)3-24H2O. A 1.5879-g sample was dissolved and the aluminum precipitatedas Al(OH)3. The precipitate was collected by filtration, washed, and ignited to give aproduct Al,03 weighing 0.1572 g. Show your calculation to determine the purity of thealum sample.

Mass of sample = 1.5879 gm Mass of Al2O3 = 0.1572 gm Molar mass of potash alum = 474.4 gm/mole…

Answered: We want to determine the purity of alum…

Chemistry for Engineering Students

4th Edition

ISBN:9781337398909

Author:Lawrence S. Brown, Tom Holme

Publisher:Lawrence S. Brown, Tom Holme

Chapter4: Stoichiometry

Section: Chapter Questions

Problem 4.98PAE

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please help me The aluminum in a 1.200g sample of impure ammonium aluminum sulfate was precipitatedwith aqueous ammonia as the hydrous Al2O3 · XH2O. The precipitate was filtered and ignitedat 100°C to give anhydrous Al2O3, which weighed 0.2001 g. Express the result of this analysisin terms of % Al.
The aluminum in a 1.200-g sample of impure ammonium aluminum sulfate was precipitated with aqueous ammonia as the hydrous Al2O3.xH2O. The precipitate was filtered and ignited at to give anhydrous Al2O3, which weighed 0.2001 g. Express the result of this analysis in terms of %NH4Al(So4)2 %Al2O3 %Al
Malic acid (C4H6O5) is a dicarboxylic acid that naturally occurs in the production of bignay wine. Maria was tasked to find out the acid content in a 200.0 mL wine sample by titrating it with a standardized solution of KOH. He was able to establish the working concentration of the KOH solution by using 39.12 mL of it to titrate a primary standard of KHP that weighed 3.021 g. The grams and %w/w of Malic acid present in the 200.0 mL wine sample were then determined by titrating a 20.00 mL aliquot using 48.95 mL of the standardized KOH solution. C4H6O5 (aq) + 2KOH (aq) ↔ K2C4H4O5 (aq) + 2H2O (l) Assume the density of the wine sample is 1.000 g/mL MM of KHP = 204.22 g/mol MM of C4H6O5 = 134.0874 g/mol ? What is the molar concentration of the prepared KOH solution?…
Malic acid (C4H6O5) is a dicarboxylic acid that naturally occurs in the production of bignay wine. Maria was tasked to find out the acid content in a 200.0 mL wine sample by titrating it with a standardized solution of KOH. He was able to establish the working concentration of the KOH solution by using 39.12 mL of it to titrate a primary standard of KHP that weighed 3.021 g. The grams and %w/w of Malic acid present in the 200.0 mL wine sample were then determined by titrating a 20.00 mL aliquot using 48.95 mL of the standardized KOH solution. C4H6O5 (aq) + 2KOH (aq) ↔ K2C4H4O5 (aq) + 2H2O (l) Assume the density of the wine sample is 1.000 g/mL MM of KHP = 204.22 g/mol MM of C4H6O5 = 134.0874 g/mol What is the molar concentration of the prepared KOH solution?…
One way in which the useful metal copper is produced is by dissolving the mineral azurite, which contains copper(I) carbonate, in concentrated sulfuric acid The sulfuric acid reacts with the copper(I) carbonate to produce a blue solution of copper(I) sulfate. Scrap iron is then added to this solution, and pure copper metal precipitates out because of the following chemical reaction: Fe(s) + CuSO4(aq) -> Cu(s) + FeSO4(aq) Suppose an industrial quality-control cherist analyzes a sample from a copper processing plant in the following way. He adds powdered iron to a 300. mL copper(I) sulfate sample from the plant until no more copper will precipitate. He then washes, dries, and weighs the precipitate, and finds that it has a mass of 75. mg Calculate the oriqinal concentration of copper(I) sulfate in the sample. Round your answer to 2 significant digits.
An unknown sample containing a mixture of NaCl and Na2CO3 was analyzed to determine the % composition of each compound. In the analysis for Na2CO3 (soda ash), the following data were obtained mass of unknown - 0.4436 g conc. of HCl used - 0.25 N initial volume - 0.5 mL final volume - 20.0 mL (MW soda ash) 106.12) 1.) What method was used to determine the concentration of HCl? 2.) What is the net volume of HCl used in the titration? 3.) What is % Na2CO3 in the given sample? NOTE: Round off your answer to a whole number (2 sig fig)
3. A solution was prepared by dissolving 413 mg of K3Fe(CN)6 (329.2 g/mol) in sufficient water to give 500.0 mL. A. What is the molar analytical concentration of K3Fe(CN)6? B.What is the the molar concentration of K+( potassium ion)? C. What is the weight/volume percentage of K3Fe(CN)6? D.
1. Calculate the equivalent weight of KMnO₄ in the following reaction: MnO₄⁻ + CN⁻ + H₂O ⟶ MnO₂ (s) + CNO⁻ + OH⁻) 2. Calculate the normality and molarity of a 15.0% (by weight) H₂SO₄ solution with a specific gravity of 1.090. * 3. To what volume should 100 mL of the above solution be diluted to prepare 1.50 N solution?
In the standardization of HCl using pure anhydrous sodium carbonate as the primarystandard for methyl orange as an indicator, 1.0 mL HCl was found to be equivalent to 0.05gof sodium carbonate (MW =106). The normality of HCl is:
A quantitative analysis for ethanol, C2H6O, can be accomplished by a redox back titration.Ethanol is oxidized to acetic acid, C2H4O2, using excess dichromate, Cr2O72–, which is reduced toCr3+. The excess dichromate is titrated with Fe2+, giving Cr3+ and Fe3+ as products. In a typicalanalysis, a 5.00-mL sample of a brandy is diluted to 500 mL in a volumetric flask. A 10.00-mLsample is taken and the ethanol is removed by distillation and collected in 50.00 mL of anacidified solution of 0.0200 M K2Cr2O7. A back titration of the unreacted Cr2O72–requires 21.48mL of 0.1014 M Fe2+. Calculate the %w/v ethanol in the brandy
To determine the percentage of bromide in a mixture containing a soluble bromide salt, the procedure from Experiment 10 is used except the bromide is precipitated with aqueous lead (II) nitrate, Pb(NO3)2, forming PbBr2(s). Initially, a 0.7893 g sample of an unknown bromide salt is dissolved in water. Excess Pb(NO3)2 is added to the solution to quantitatively precipitate the bromide from the solution. The resulting mixture is filtered through a piece of filter paper weighing 1.3587 g. After several days of drying, the filter paper and precipitate weighed 1.8257 g. Calculate the percent bromide in the original sample. Pb(NO3)2 Mw = 331.2 g/mol PbBr2 Mw = 367.0 g/mol
To determine the amount of magnetite, Fe3O4 in an impure ore, a 1.5419 g sample is dissolved in concentrated HCl to obtain a mixture of Fe2 + and Fe3 +. After HNO3 is added to oxidize Fe2 + to Fe3 + and diluted with water, Fe3 + is precipitated as Fe (OH) 3 by adding NH3. 0.8525 g of pure Fe2O3 is obtained by filtering, rinsing and burning the precipitate. Calculate the percentage of Fe3O4% in the sample. (Fe = 55,847g / mol, O = 15,999g / mol)

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