2. The hydrogen sulfide in a 50.0 g sample of crude petroleum was removed by distillation and collected in a solution of CdCl2. The precipitated CdS was then filtered, washed, and ignited to CdSO4. Calculate the percentage of H₂S in the sample if 0.1080 g of CdSO4 was recovered.

2. The hydrogen sulfide in a 50.0 g sample of crude petroleum was removed by distillation and collected in a solution of CdCl2. The precipitated CdS was then filtered, washed, and ignited to CdSO4. Calculate the percentage of H₂S in the sample if 0.1080 g of CdSO4 was recovered.

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

A 0.4550-g solid mixture containing CaCl2 is dissolved in water and treated with an excess of Pb(NO3)2, resulting in the precipitation of 0.6168 g of PbCl2. What percent of sample is CaCl2?
A chemist needs to determine the concentration of a solution of nitric acid, HNO3. She puts 905 mL of the acid in a flask along with a few drops of indicator. She then slowly adds 0.200 mol L Ba(OH)2 to the flask until the solution turns pink, indicating the equivalence point of the titration. She notes that 225 mL of Ba(OH)2 was needed to reach the equivalence point. Solution map In this titration, the concentration of base is known and can be used to calculate the unknown acid concentration: concentration of base → moles of base → moles of acid → concentration of acid Part A How many moles of Ba(OH)2 are present in 225 mL of 0.200 mol L-1 Ba(OH)2? Express your answer numerically in moles. • View Available Hint(s) Vo AEO ? mol Ba(OH)2 Submit
On the first phase, which is prepared by dissolving some bromine (Br2) in 10 mL of carbon sulfur at constant pressure and 25 ° C, 20 mL of water is added at the same temperature. After waiting for the well-shaken mixture to come to equilibrium, the carbon sulfur and water phases are completely separated and the bromine amounts are determined. It has been experimentally determined that there is 1.29 g of bromine in the carbon sulfur phase and 0.0064 g of bromine in the water phase. a) Partition coefficient of bromine between carbon sulfur and water phases ......................determined as. b) If 2.2 g of bromine were dissolved in carbon sulfide initially at the same pressure and temperature, the mass of bromine passing into the water phase ...................... ...... ..................... (MBr: 79,904 g / mol) Note: enter only required numerical values and units in the spaces in the question.
A chemistry student needs to standardize a fresh solution of sodium hydroxide. She carefully weighs out 13.mg of oxalic acid H2C2O4, a diprotic acid that can be purchased inexpensively in high purity, and dissolves it in 250.mL of distilled water. The student then titrates the oxalic acid solution with her sodium hydroxide solution. When the titration reaches the equivalence point, the student finds she has used 11.9mL of sodium hydroxide solution. Calculate the molarity of the student's sodium hydroxide solution. Round your answer to 2 significant digits.
0.753-g sample of a chlorocarbon compound was analyzed by burning it in oxygen and collecting the evolved gases in a solution of NaOH. After neutralizing, the sample was treated with 25.74 mL of a 0.264 M AgNO3 solution. This precipitated the chloride (Cl-) out as AgCl and left an excess of AgNO3. The excess AgNO3 was titrated with 0.1 M KSCN and required 16.47 mL to reach the endpoint in a Volhard titration. Calculate the % w/w Cl– (35.45 g/mol) in the sample. Provide your answer to 2 places after the decimal point and without units. Reactions: Cl– + Ag+ → AgCl(s) Reaction 1 Ag+ + SCN– → AgSCN(s) Reaction 2 HINT: This is an example of a back-titration. Steps to success: First, calculate the TOTAL amount (in moles) of Ag+ added from the volume and molarity of the silver nitrate solution. Second, determine the EXCESS amount of Ag+ from the reaction with thiocyanate (Reaction 2 above). Third, calculate the…
6. In an experiment, the molecular formula for calcium hydroxide was determined to be Ca(OH)2. In this experiment, 0.050 g of Ca (s) was added to 150. mL of DI water. After adding 10 drops of 0.1% thymol blue indicator, the solution was titrated with 0.30 M HCl. a. Write the balanced equation for the net ionic reaction that occurred during the titration. b. Calculate the volume of 0.30 M HCl required to reach the end point of the titration. C. If the initial reading of HCl in the burette was 25.60 mL, what was the final reading of HCl in the burette at the end point of the titration?
Write the balanced equation for the reaction of aqueous Pb(ClO3)2Pb(ClO3)2 with aqueous NaI.NaI. Include phases. chemical equation: What mass of precipitate will form if 1.50 L1.50 L of highly concentrated Pb(ClO3)2Pb(ClO3)2 is mixed with 0.500 L 0.300 M NaI0.500 L 0.300 M NaI? Assume the reaction goes to completion.
3. What is the percentage of sulfur in a sample of 2 gm of coal that gave a precipitate of 0.084 g of barium sulfate? Note that the atomic weight of sulfur is 32 gm / mole and the molecular weight of the Baso precipitate is 233.4 g / mole.
100.0 mL of 0.60 M aqueous Pb(NO3)2 is mixed with excess aqueous KI. What mass of precipitate is formed?
A 150.0 mL solution of 3.011 M strontium nitrate is mixed with 210.0 mL of a 3.176 M sodium fluoride solution. Calculate the mass of the resulting strontium fluoride precipitate. mass: Assuming complete precipitation, calculate the final concentration of each ion. Ksp values can be found in the table of solubility product constants. [Na] = [NO₂] = [SP²+] = [F] = M M M M
In a titration lab determining the salt content of potato chips, silver nitrate, potassium chromate, and calcium carbonate were used. Explain the purpose of each chemical.
100.0 cm3 of a 1.234 mol.dm-3 solution of nickel(II) nitrate was added to 150.0 cm3 of a 1.178 mol.dm-3 solution of sodium carbonate. Calculate the concentration of nitrate ions in the solution at the completion of the reaction.