A 4.955-g sample of a petroleum product was burned in a tube furnace, and the SO₂ produced was collected in 3% H₂O2. Reaction: SO2(g) + H₂O2 → H₂SO4 A 27.00-mL portion of 0.00816 M NaOH was introduced into the solution of H₂SO4, following which the excess base was back-titrated with 15.45 mL of 0.01173 M HCl. Calculate the sulfur concentration in the sample in parts per million. ppm Concentration =

A 4.955-g sample of a petroleum product was burned in a tube furnace, and the SO₂ produced was collected in 3% H₂O2. Reaction: SO2(g) + H₂O2 → H₂SO4 A 27.00-mL portion of 0.00816 M NaOH was introduced into the solution of H₂SO4, following which the excess base was back-titrated with 15.45 mL of 0.01173 M HCl. Calculate the sulfur concentration in the sample in parts per million. ppm Concentration =

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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The concentration of SO42– ions in a 45.0 mL sample of seawater is determined by adding a solution of BaCl2 and precipitating the SO42– as BaSO4. After the precipitate is filtered from the solution, it is dried and weighed. If the mass of BaSO4 recovered is 0.315 g, what is the sulfate concentration of the seawater sample? Express your answer in mmol/L.
6.) One way to determine the amount of nitrogen in a sample is through a method called Kjeldahl Method. In this method, the nitrogen in the sample is converted first to ammonium ions (N ? NH4+). The ammonium ions are then converted to ammonia by making the solution basic with the use of sodium hydroxide (NH4+ ? NH3). The ammonia produced is reacted with hydrochloric acid (NH3 +HCl ? NH4Cl). The unreacted hydrochloric acid is then titrated with standard sodium hydroxide solution. Using the method outlined, a 1-mL fish sample was analyzed. The liberated ammonia was collected in 100 mL of 0.0503 M HCl. The unreacted HCl then required 28.3 mL of 0.124 M NaOH for titration. Calculate the nitrogen in the sample as mg N/mL.
The following solutions are needed to be prepared for the titration procedure:1. 20 mL of 2 M HCl2. 20 mL of 0.05 M KOH1.0867 grams of Fe(OH)n was mixed with the 20mL of 2 M HCl that is initially prepared. This solution was diluted to 200 mL and was labeled as solution A. 20.0 mL aliquot of solutionA was taken and titrated with 20.0 mL of 0.05 M KOH. From this data, determine for the value of n.
1. (а) The solubility product of a sparingly soluble salt, XF2, was determined by titration and found to be 2.9 x 101º M. The procedure involved the following steps: (i) A saturated solution of the salt XF2 was prepared. (ii) 25.00 mL of this solution was titrated against a standardized 0.005 M HCl solution. Determine the titre value obtained in the experiment.
Oxalic acid dihydrate (H2C2O4 2H2O) can be used to standardize NaOH solution through acid-base titration. To determine the molarity of an unknown NaOH solution, a student weighed out 0.56 g of solid oxalic acid dihydrate and dissolved the solid in 32.8 mL of DI water. The resulting solution was used in a titration with the unknown NaOH solution (3 drops of phenolphthalein was used as an indicator). The balanced chemical equation is given below. If the student used 25.71 mL of the unknown NaOH solution in the titration, what is the molarity of the NaOH solution? Keep the correct number of significant figures. H2C2O4 (aq) + 2NaOH (aq) --> Na2C2O4 (aq) + 2H2O (l)
Standardising a base solution by titration.
A 185.0 mL sample of 1.200 M Pb(NO3)2 is mixed with 99.50 mL of 1.500 M NaCl and the PbCl2 precipitate is filtered from the solution. Then 200.0 mL of 3.000 M NaBr is added to the remaining solution, and the PbBr2 precipitate is also collected and dried. What is the mass (in grams) of the PbBr2 precipitate, assuming the yield in each precipitation step is 100%?
The percentage of CaCO3 in a sample of finely powdered limestone was determined. In the laboratory, the sample was dissolved in HCl then heated to expel CO2. The remaining HCl was then titrated with NaOH. Which is the main analyte in the sample? NaOH HCl CO2 CaCO3
A 0.917-g sample of canned tuna was analyzed by the Kjeldahl method. A volume of 20.59 mL of 0.1249 M HCl was required to titrate the liberated ammonia. Calculate the percentage of nitrogen in the sample.
A 20.00-mL sample of aqueous oxalic acid, H2C2O4, was titrated with a 0.09113-M solution of potassium permanganate, KMnO4. A volume of 23.24 mL was required to reach the endpoint. What is the molarity of oxalic acid?
You have been provided with a 2.08 x 10-2 L sample of lithium hydroxide (LiOH) of unknown concentration. You perform a titration with 2.19 M nitric acid (HNO3), and find that 24.6 mL are required to reach the equivalence point (as determined using a coloured indicator). What is the concentration of the lithium hydroxide solution in mol L-1?
A dried sample of commercial salt was prepared by a coning and quartering. A 0.837-g sample of the salt was dissolved and diluted to 250.0 mL in a volumetric flask. Repeat 10.00-mL aliquots of this solution were titrated with a 0.057 M silver nitrate solution, requiring 9.07 mL to reach equivalence. Calculate the mass (g) of NaCl in the original sample.