11. A 101.3-mg sample of an organic compound known to contain Cl is burned in pure O2 and the combustion gases collected in absorbent tubes. The tube used to trap CO2 increases in mass by 167.6 mg, and the tube for trapping H2O shows a 13.7-mg increase. A second sample of 121.8 mg is treated with concentrated HNO3 producing Cl2, which subsequently reacts with Ag*, forming 262.7 mg of AgCl. (MM of C = 12.01 g/mol , O = 16.00 g/mol, CI = 35.45 g/mol, H = 1.008 g/mol, AgCl = 143.32 g/mol). Determine the: %3D

11. A 101.3-mg sample of an organic compound known to contain Cl is burned in pure O2 and the combustion gases collected in absorbent tubes. The tube used to trap CO2 increases in mass by 167.6 mg, and the tube for trapping H2O shows a 13.7-mg increase. A second sample of 121.8 mg is treated with concentrated HNO3 producing Cl2, which subsequently reacts with Ag*, forming 262.7 mg of AgCl. (MM of C = 12.01 g/mol , O = 16.00 g/mol, CI = 35.45 g/mol, H = 1.008 g/mol, AgCl = 143.32 g/mol). Determine the: %3D

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...

See similar textbooks

Similar questions

2. In one gravimetric analysis, the aluminum in a 1.2g sample of impure NHAI(SO4)2 was precipitate as hydrous ALO3.XH2O. The precipitate was filtered and ignited at 1000 °C to give anhydrous Al2O3 which weighed 0.1798g. Calculate the % Al inthe sample. 3. A sample of 0.4500g impure potassium chloride was dissolved in water treated with excess silver nitrate solution. 0.8402 g of silver chloride was precipitated. What is the percentage of potassium chloride in the sample?
A 4.912-g sample of a petroleum product was burnedin a tube furnace, and the SO2produced was collectedin 3% H2O2.Reaction:SO2(g)+H2O2→H2SO4A 25.00-mL portion of 0.00873 M NaOH was introducedinto the solution of H2SO4, following whichthe excess base was back-titrated with 15.17 mL of0.01102 M HCl. Calculate the sulfur concentrationin the sample in parts per million.
The digestion of a 0.1432 g sample of a compound containing phosphorous in a mixture of HNO3 and H2SO, resulted in the formation of CO2, H2O and H3PO4 Addition of ammonium molybdate yielded a solid having the composition (NH)3PO, 12M0O3 (MW=1876.3 g/mol). This precipitate was filtered washed, and dissolved in 50 00 mL of 0.2000 M NaOH: (NH,)3PO4-12MO03(s)+ 26OH (aq) HPO,2 (aq) +12M00,2 (aq) +14H2O(1) + 3NH3(g) After the solution was boiled to remove NH3, the excess NaOH was titrated with 14.71mL of 0.1741 M HCI to a phenolphthalein end point (back titration). Calculate the percentage of phosphorous in the solid sample. 6.19% 10.6% O 27.6% O0 238% O 19.5
A 0.2985 g sample of an antibiotic powder was dissolved in HCl and the solution diluted to 100.0 mL. A 20.00 ml aliquot was transferred to a flask and followed by 25.00 ml of 0.01886 M KBRO3. An excess of KBr was added to form Br2, and the flask was stoppered. After 10 min, during which time the Br2 brominated the sulfanilamide, an excess of KI was added. The liberated iodine titrated with 12.88 ml of 0.1235 M sodium thiosulfate. Calculate the percent sulfanilamide (NH2C,H4SO2NH2) in the powder. Bro, + 5Br + 6H* 3Br, + 3H,0 NH2 NH2 Br. Br + 2B12 + 2H++ 2Br SO,NH2 SO,NH2 sulfanilamide Br, + 51 2Br + 12 excess 2 + 25,0,- 25,0,2 + 21- - MM: NH2C6H4SO2NH2 = 172.21 KBRO3 = 167.00 KBr 119.00
The concentration of ammonia in a cleaning product was determined by back titration.Firstly, 10.00 cm3 of the cleaning product was pipetted into a large conical flask,containing 250.00cm3 of 0.50 mol/l HCl to give Solution A.Following a period of reaction and shaking, 50.00cm3 of Solution A was removed anddiluted to 250 cm3 with water in a volumetric flask to give Solution B.20 cm3 samples of Solution B were titrated against 0.05 mol/l Na2CO3 solution, givingan average titre of 12.45 cm3. i) Write equations for the reactions that have taken place.ii) Determine the concentration of NH3 in the original cleaning product in mol/l,g/l, ppm, and % w/v.
(4) Assume that the change in concentration of N₂O4 is small enough to be neglected in the following problem. (a) Calculate the equilibrium concentration of both species in 1.00 L of a solution prepared from 0.129 mol of N₂O4 with chloroform as the solvent. N₂04 (9) 2 NO₂ (g) Kc = 1.07 x 10-5 in chloroform (b) Show that the change is small enough to be neglected.
1. (a) Write the chemical equation indicating the stepwise displacement of coordinated H20 by NH3 for the following reaction. [Ni(H20)6]?* + XNH3 -> [Ni(H2O)6-x (NH3)x]"(aq) + X2H2O (b) The log Kn values for the reaction are given in the table below. Comment on the trend. Log K1 K2 K3 K4 Ks K6 2.8 2.24 1.73 1.19 0.75 0.03
Caustic potash that has been exposed to air is found on analysis to contain 90.00% KOH, 2.38% K2CO3 and 7.62% H2O. What weight of residue will be obtained if 1.00 g of this sample is added to 46.00 mL of 1.00 N HCl and the resulting solution, after neutralization with 1.070N KOH is evaporated to dryness?
A 0.512 g sample of a commercial phosphate detergent was ignited at a red heat to destroy the organic matter. The residue was taken up in hot HCl, which converted the P to H3PO4. The phosphate was precipitated as MgNH4PO4.6H2O by addition of Mg2+ followed by aqueous NH3. After being filtered and washed the precipitate was converted to Mg2P2O7 by ignition at 1000 0C and the residue weighed 0.1151g. (a) What is the Gravimetric Factor to convert Mg2P2O7 to P? (b) Calculate the percent P in the sample could you type it out please
A 10.00mL sample of alcoholic ethyl acetate was diluted to 100.00 mL. 20.00 mL was aliquoted and mixed with 40.00 mL of 0.04672 M KOH. The resulting mixture was heated for 2 hours. CH3COOC2H5 + OH- → CH3COO- + C2H5OH After cooling, the excess OH was back titrated with 3.41 mL of 0.05042 M H2SO4. Answer the following: Calculate the number of moles of OH- that reacted with ethyl acetate. Calculate the number of moles of ethyl acetate in the 20.00 mL solution. What is the mass of ethyl acetate (FW=88.11 g/mol) in the original 10.00 mL sample?
Name: 11. A student is instructed to determine the concentration of a solution of CoCl2 based on absorption of light (spectrometric/colorimetric method). The student is provided with a 0.10 M solution of CoCl₂ with which to prepare standard solutions with concentrations of 0.020 M, 0.040 M, 0.060 M and 0.080 M. (a) Describe the procedure for diluting the 0.10 M solutions to a concentration of 0.020 M using distilled water, a 100 mL volumetric flask, and a pipet or buret. Include specific amounts where appropriate. Percent Transmittance The student takes the 0.10 M solution and determines the percent transmittance and the absorbance at various wavelengths. The two graphs below represent the data. 100 Absorbance 50 60 40 20 Absorbance 360 0.60 0.20 360 0.30 0.20 0.10 440 480 Wavelength (nm) 0.020 Wavelength (nm) (b) Identify the optimum wavelength for the analysis. The student measures the absorbance of the 0.020 M, 0.040 M, 0.060 M, 0.080 M and 0.10 M solutions. The data are plotted…
A. For each pair of compounds, fill in the appropriate information needed to distinguish them. Compound that will Positive Differentiating Chemical test sign/s of reaction Compound A Compound B react (А/B) COH Dissolution and (1) rapid bubbling (effervescence) (2) ОН OH NH2 H2N. HO. (3) (4) B Formation of O¯ Na O Na (5) white (6) precipitate Br (7) (8) (9)