7. The tetraethyl lead, Pb(C2H5)4 in a 25.00 mL sample of gasoline was shaken with 15.00 mL of 0.02095 M I2. The reaction is Pb(C2H5)4 + I2 → Pb(C2H5)3I + C2H$I After the reaction was complete, the unused I2 was titrated with 6.09 mL of 0.03465 M NazS2O3. I2 + 2NA2S2O3 2Nal + NazS4Os Calculate the weight in milligrams of Pb(C2HS)4 (323.4 g/mol) in each milliliter of the gasoline. [ 8.100 5.400 2.700 10.80 ] mg/mL

7. The tetraethyl lead, Pb(C2H5)4 in a 25.00 mL sample of gasoline was shaken with 15.00 mL of 0.02095 M I2. The reaction is Pb(C2H5)4 + I2 → Pb(C2H5)3I + C2H$I After the reaction was complete, the unused I2 was titrated with 6.09 mL of 0.03465 M NazS2O3. I2 + 2NA2S2O3 2Nal + NazS4Os Calculate the weight in milligrams of Pb(C2HS)4 (323.4 g/mol) in each milliliter of the gasoline. [ 8.100 5.400 2.700 10.80 ] mg/mL

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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6
A 57.0 mLmL sample of a 0.108 MM potassium sulfate solution is mixed with 37.0 mLmL of a 0.106 MM lead(II)(II) acetate solution and the following precipitation reaction occurs: K2SO4(aq)+Pb(C2H3O2)2(aq)→2KC2H3O2(aq)+PbSO4(s). Find the theoretical yield and percent yield.
It is desired to prepare 600 mL of 0.250 normal Ca(OH)2 for use in the reaction:2 HCl + Ca(OH)2 CaCl2 + 2 H2OHow many grams of Ca(OH)2 are needed?
1. The following reaction occurs in your lab: You have 225.0 mL of 0.345 M Na3PO4. How many grams of precipitate can are made? Balanced Rxn: 3 CaCl2 (aq) + 2 Na3PO4 (aq) → 6 NaCl (aq) + Ca3(PO4)2 (s) - 2. How many mL of a 0.220 M solution of KOH will be required to titrate 38.00 mL of a 0.0566 M solution of H3PO4? Balanced Rxn: H3PO4 (aq) + 2KOH (aq) → K2HPO4 (aq) + 2H2O (1)
4. Calculate the calculate the mass of precipitate formed from 5.0 g of strontium chloride. Li3PO4(aq) → Sr3(PO4)2(S) + LiCl(aq) _SrCl₂(aq) + 5. What mass of aluminum hydroxide in needed to neutralize 5.00 g of hydrochloric acid? Al(OH)3(s) + _HCl(aq) → ___AlCl3(aq) + _H₂O(1) 195
A 65.0 mL sample of a 0.110 M potassium sulfate solution is mixed with 36.5 mL of a 0.114 M lead(II) acetate solution and the following precipitation reaction occurs: K2SO4(aq)+Pb(C2H3O2)2(aq)→2KC2H3O2(aq)+PbSO4(s) The solid PbSO4 is collected, dried, and found to have a mass of 1.01 g . Determine the limiting reactant, the theoretical yield, and the percent yield.
Barium can be analyzed by precipitating it as BaSO4BaSO4 and weighing the precipitate. When a 0.265 gg sample of a barium compound was treated with excess H2SO4H2SO4 8.50×10−2 gg of BaSO4BaSO4 formed. What is the percentage of barium in the compound?
Consider the neutralization reaction 2HNO3(aq) + Ba(OH)2(aq) yields to 2H2O(L) + Ba(NO3)2(aq) A 0.100 L sample of an unknow HNO3 solution required 49.3 mL of 0.100 M Ba(OH)2 for complete neutralization. What is the concentration of the HNO3 solution?
Many chemical compounds contain impurities. Crude potassium carbonate (K2CO3) obtained from the chemical supplier is assayed for purity in the following way: 8.450 g of crude potassium carbonate is weighed out into a flask and dissolved in water. The final volume was completed to 0.500 L with distilled water. 20.00 mL sample is taken from this solution and placed in a flask. Potassium carbonate is then titrated to the equivalence point with 17.80 mL of 0.2050 M HCl solution. What is the percent purity of potassium carbonate in this sample? K2CO3 + HCl  KCl + H2O + CO2
A 2.1182.118 g sample of a solid mixture containing only potassium carbonate (MM=138.2058 g/molMM=138.2058 g/mol) and potassium bicarbonate (MM=100.1154 g/molMM=100.1154 g/mol) is dissolved in distilled water. A volume of 30.1030.10 mL of a 0.7570.757 M HCl standard solution is required to titrate the mixture to a bromocresol green end point. Calculate the weight percent of potassium carbonate and potassium bicarbonate in the mixture.
Barium (Ba) can be analyzed in solutions by forming BaSo4 (s) precipitate. Ba 2+ + SO4 2- = BaSo4 (s) When a 1.0 g sample of a barium compound was treated with H2So4, it formed 0.605 g of BaSo4 (s) percipitate. a) What is the percent by weight of barium (Ba 2+) in the barium compound? b) What is the identity of the sample barium compound?
You mix 29.0 mL of 0.312 M FeCl3 with 38.5 mL of 0.446 M NaOH. What mass of Fe(OH)3 (in grams) will precipitate from this reaction mixture? Mass= g One of the reactants (FeCl3 or NaOH) is present in a stoichiometric excess. What is the molar concentration of the excess reactant remaining in solution after Fe(OH)3 has been precipitated? Assume the volumes are additive. Concentration = M