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8. Magnesium oxide is not very soluble in water, and is dif tult to titrate directly. I ts purity can be det ermined by use of a 'back titration'method. A 4.06 g sample of impure magnesium oxide was completely dissolved in 100 cm³ of hydrochl oric acid, of concentration 2.0 mol dm (in excess). The excess acid required 1 9.7 cm³ of sodium hydroxide (0.20 mol dm) for neutralization. This second ti tration is called a 'back titration', and is used to determine the unreacted acid. Calculate the mass of magnesium oxide that reacted with the initial hydrochlo ric acid, hence the % purity of the magnesium oxide.

8. Magnesium oxide is not very soluble in water, and is dif tult to titrate directly. I ts purity can be det ermined by use of a 'back titration'method. A 4.06 g sample of impure magnesium oxide was completely dissolved in 100 cm³ of hydrochl oric acid, of concentration 2.0 mol dm (in excess). The excess acid required 1 9.7 cm³ of sodium hydroxide (0.20 mol dm) for neutralization. This second ti tration is called a 'back titration', and is used to determine the unreacted acid. Calculate the mass of magnesium oxide that reacted with the initial hydrochlo ric acid, hence the % purity of the magnesium oxide.

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Chemistry
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ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
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11:32 am ( More CHM101 ASSIG... hown in the following balanced equation: NH, (ag) + HNO,(ag) - NH, N0, (ag) In an experiment, 404.2 g of ammonium nitrate is produced when 112.5 g of amm onia and excess nitric acid are combined. Determine the percent yield of the produ ct. 7. An iron supplement is used to treat anaemia and 50 mg of Fe2+ is required per tablet. If the iron compound used in the tablet is Feso4.7H20, what mass of thi s compound would be required per tablet to provide the desired amount of Fe2 +? 8. Magnesium oxide is not very soluble in water, and is dif tult to titrate directly. I ts purity can be determined by use of a 'back titration'method. A 4.06 g sample of impure magnesium oxide was completely dissolved in 100 cm3 of hydrochl oric acid, of concentration 2.0 mol dm3 (in excess). The excess acid required 1 9.7 cm3 of sodium hydroxide (0.20 mol dm3) for neutralization. This second ti tration is called a 'back titration', and is used to determine the unreacted acid. magnesium oxide that reacted with the initial hydrochlo Calculate the mass ric acid, hence the % purity of the magnesium oxide. The reaction equations are: M90 (s) + HCI (ag)- MgC, (aq) + H,O) NaOH (ag) + HCI (ag) - NaCI (ng) + HO0) 9. Assign the oxidation numbers of each element given bold in the following che mical species: HCI, NH3, NO3- , K2Cr207, Hg2Cl2, HgCl2 Al(OH)3, NazPO4 10. Aniline, a starting material for urethane plastic foams, consists of C, H, and N. Combustion of such compounds yields CO2, H20, and N2 as products. If the co mbustion of 9.71 g of aniline yields 6.63 g H,0 and 1.46 g N,, determine the e mpirical formula of aniline and the molecular formula, if the molar mass of an iline is 93 g/mol. 11.Calculate the percentage of Cl in Al(CIO,)3- 12.A 60kg woman has 1.13kg of heamoglobin (64,456 g/mol) in her blood. How many molecules of heamoglobin are in her blood? 13.A solution of Na,CO3 (105.99 g/mol) is obtained by dissolving 0.10599 g of N a,CO, into in a 1000.00 mL volumetric flask. 2|Pagel Q Edit Fit screen Search Save as
Transcribed Image Text:11:32 am ( More CHM101 ASSIG... hown in the following balanced equation: NH, (ag) + HNO,(ag) - NH, N0, (ag) In an experiment, 404.2 g of ammonium nitrate is produced when 112.5 g of amm onia and excess nitric acid are combined. Determine the percent yield of the produ ct. 7. An iron supplement is used to treat anaemia and 50 mg of Fe2+ is required per tablet. If the iron compound used in the tablet is Feso4.7H20, what mass of thi s compound would be required per tablet to provide the desired amount of Fe2 +? 8. Magnesium oxide is not very soluble in water, and is dif tult to titrate directly. I ts purity can be determined by use of a 'back titration'method. A 4.06 g sample of impure magnesium oxide was completely dissolved in 100 cm3 of hydrochl oric acid, of concentration 2.0 mol dm3 (in excess). The excess acid required 1 9.7 cm3 of sodium hydroxide (0.20 mol dm3) for neutralization. This second ti tration is called a 'back titration', and is used to determine the unreacted acid. magnesium oxide that reacted with the initial hydrochlo Calculate the mass ric acid, hence the % purity of the magnesium oxide. The reaction equations are: M90 (s) + HCI (ag)- MgC, (aq) + H,O) NaOH (ag) + HCI (ag) - NaCI (ng) + HO0) 9. Assign the oxidation numbers of each element given bold in the following che mical species: HCI, NH3, NO3- , K2Cr207, Hg2Cl2, HgCl2 Al(OH)3, NazPO4 10. Aniline, a starting material for urethane plastic foams, consists of C, H, and N. Combustion of such compounds yields CO2, H20, and N2 as products. If the co mbustion of 9.71 g of aniline yields 6.63 g H,0 and 1.46 g N,, determine the e mpirical formula of aniline and the molecular formula, if the molar mass of an iline is 93 g/mol. 11.Calculate the percentage of Cl in Al(CIO,)3- 12.A 60kg woman has 1.13kg of heamoglobin (64,456 g/mol) in her blood. How many molecules of heamoglobin are in her blood? 13.A solution of Na,CO3 (105.99 g/mol) is obtained by dissolving 0.10599 g of N a,CO, into in a 1000.00 mL volumetric flask. 2|Pagel Q Edit Fit screen Search Save as
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