See the attached file Copper(II) sulfate pentahydrateMass of empty crucible11.88Mass of crucible plus hydrate12.37Mass of hydrate takenAppearance of hydrateBlue Boluratien, Selt.Theoretical mass of H20 lost expected on heating hydrateMass of crucible + anhydrous CuSO4 after heating12:304Mass of anhydrous CuSO4(mass of crucible + anhydrous/CUSO4 after heating – mass of empty crucible)Mass of water lost from hydrate crystals 0.07,(mass of hydrate taken – mass of anhydrous CuS04)% error in mass water loss from hydrate% of water lossAppearance of CuSO4 after heatingWhi ty/ clya,Appearance of CuSO4 on adding waterBlue.

Answered: Image /qna-images/answer/cb074bf3-26e4-4347-bf0e-5012e6f43f86.jpg

Copper(II) sulfate pentahydrate Mass of empty crucible |1.88, Mass of crucible plus hydrate 12.3 • 494 Goluration. Selt. Mass of hydrate taken Appearance of hydrate Blue Theoretical mass of H20 lost expected on heating hydrate Mass of crucible + anhydrous CuSO4 after heating. 12:30 Mass of anhydrous CuSO4. (mass of crucible + anhydrous/CUSO4 after heating – mass of empty crucible) 0:42 0•07% Mass of water lost from hydrate crystals (mass of hydrate taken – mass of anhydrous CuS04) % error in mass water loss from hydrate % of water loss Appearance of CuSO4 after heating hi ty I cluar Appearance of CUSO4 on adding water Blue.

Copper(II) sulfate pentahydrate Mass of empty crucible |1.88, Mass of crucible plus hydrate 12.3 • 494 Goluration. Selt. Mass of hydrate taken Appearance of hydrate Blue Theoretical mass of H20 lost expected on heating hydrate Mass of crucible + anhydrous CuSO4 after heating. 12:30 Mass of anhydrous CuSO4. (mass of crucible + anhydrous/CUSO4 after heating – mass of empty crucible) 0:42 0•07% Mass of water lost from hydrate crystals (mass of hydrate taken – mass of anhydrous CuS04) % error in mass water loss from hydrate % of water loss Appearance of CuSO4 after heating hi ty I cluar Appearance of CUSO4 on adding water Blue.

Fundamentals Of Analytical Chemistry

9th Edition

ISBN:9781285640686

Author:Skoog

Publisher:Skoog

Chapter7: Statistical Data Treatment And Evaluation

Section: Chapter Questions

Problem 7.12QAP

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Similar questions

At elevated temperature NaHCO3 is quantitatively converted to Na2CO3. By calcining 0.3592 g of an antacid tablet containing NaHCO3, 0.2362 g of Na2CO3 was obtained. Calculate the percentage purity of the tablet (such as % w/w NaHCO3) It would be appreciated if you could write each step to the answer.
A sample of ferrous oxide has actual formula Fe93O1.00. In this sample what fraction of metal ions are Fe2+ions? What type of nonstoichiometric defect is present in this sample?
How do you convert 18.8 CP2/TM3 to YY2/ZW3? Use the folowing inequalities: 1CP=2.104 BX, *Bx=4 YY, 1TM=7.1088DD, 1DD=4.966ZW. When writing out the answer leave out the units.
You have two distinct gaseous compounds made from element X and element Y. The mass percents are as follows: Compound I: 30.43% X, 69.57% Y Compound II: 63.64% X, 36.36% Y In their natural standard states, element X and element Y exist as gases. (Monatomic? Diatomic? Triatomic? That is for you to determine.) When you react gas X with gas Y to make the products, you get the following data (all at the same pressure and temperature): 1 volume gas X + 2 volumes gas Y 2 volumes compound I 2 volumes gas X + 1 volume gas Y 2 volumes compound II Assume the simplest possible formulas for reactants and products in the chemical equations above. Then, determine the relative atomic masses of element X and element Y.
You have two distinct gaseous compounds made from element X and element Y. The mass percents are as follows: Compound I: 30.43% X, 69.57% Y Compound II: 63.64% X, 36.36% Y In their natural standard states, element X and element Y exist as gases. (Monatomic? Diatomic? Triatomic? That is for you to determine.) When you react gas X with gas Y to make the products, you get the following data (all at the same pressure and temperature): 1. volume gas X + 2 volumes gas Y2 volumes compound I 2. volumes gas X + 1 volume gas Y2 volumes compound II Assume the simplest possible formulas for reactants and products in the chemical equations above. Then, determine the relative atomic masses of element X and element Y.
You have two distinct gaseous compounds made from element X and element Y.The mass percents are as follows: Compound I: 30.43% X, 69.57% Y Compound II: 63.64% X, 36.36% Y In their natural standard states, element X and element Y exist as gases. (Monatomic? Diatomic? Triatomic? That is for you to determine.) When you react "gas X" with "gas Y" to make the products, you get the following data (all at the same pressure and temperature): 1 volume "gas X" + 2 volumes "gas Y" → 2 volumes compound I 2 volumes "gas X" + 1 volume "gas Y" → 2 volumes compound II Assume the simplest possible formulas for reactants and products in the chemical equations above. Then, determine the relative atomic masses of element X and element Y.
Using grammatically correct English sentences, describethe relationship between the number 6.022 * 1023 and thegram.
It is estimated that uranium is relatively common in earth's curst, occuring in amounts of 4g/metric ton. A metric ton is 1000 kg. At this concentration, what mass of uranium is present in 1.0 mg of the earth's curst? (The answer is suppose to be 4X10-9 grams)
2.48g of hydrated copper(ii)chloride (CuCl2.xH2O) were heated to constant mass. 1.96g of anhydrous copper(ii)chloride were obtained. determine the value of x in CuCl2.xH2O.(AO2)
Assuming that the percent of uncertainty in the calculated molar mass is the same as the percent of uncertainty in the temperature change, calculate the uncertainty in the molar mass. Could the chemist unequivocally state that the substance is cocaine? For example, is the uncertainty small enough to distinguish cocaine from codeine (C18H21NO3, molar mass = 299.36 g/mol)?
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Q11 Ans: 60.38 kJ/mol

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