A 5.351 g solid sample containing only KNO₂ (FW = 85.104 g/mol) and KNO3 (FW = 101.103 g/mol) is dissolved in 500.0 mL of water. A 50.00 mL aliquot of the solution is treated with 48.00 mL of 0.1171 M Ce** in strong acid to oxidize the nitrite (NO₂) ion and form the nitrate (NO3) ion. After 5 minutes, the excess Ce4+ is back-titrated with 33.57 mL of 0.04141 M Fe²+. Calculate the mass percent of KNO₂ in the solid.

A 5.351 g solid sample containing only KNO₂ (FW = 85.104 g/mol) and KNO3 (FW = 101.103 g/mol) is dissolved in 500.0 mL of water. A 50.00 mL aliquot of the solution is treated with 48.00 mL of 0.1171 M Ce** in strong acid to oxidize the nitrite (NO₂) ion and form the nitrate (NO3) ion. After 5 minutes, the excess Ce4+ is back-titrated with 33.57 mL of 0.04141 M Fe²+. Calculate the mass percent of KNO₂ in the solid.

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 50.0 ml solution contains only Na2SO4 (MW 142.04 g/mole). If 40.0 ml of 0.25 M BaCl2 is needed to precipitate all the SO42- as BaSO4, what mass of Na2SO4 was in the original solution? What is the concentration of Cl- in the final solution?
Tungsten trioxide (WO,) has a rich yellow color and is often used as a pigment in ceramics and paints. To test a ceramic vase for its WO, content, a 10.15 g sample of the vase was ground and reduced with Pb(Hg) to convert any WO, to W³+. The resulting W3+ was transferred to 500.0 mL of 1.00 M HCI. A 100.00 mL aliquot of the HCl solution required 14.78 mL of 0.08271 M potassium permanganate (KMNO,) to reach the purple endpoint. A blank required 0.26 mL. Balance the redox reaction. redox reaction: MnO, + W3+ Mn2+ + WO3+ Determine the percent WO, in the ceramic sample. percent WO3: %
1. A sample (0.212g) of an unknown acid was dissolved in water and analyzed by titrating with 0.1760 M NaOH. A volume of 15.48 mL of NaOH was required to completely neutralize the acid. Calculate the molar mass of the acid in g/mol.
3. A 4.912-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 25.00-mL portion of 0.00873 M NaOH was introduced into the solution of H₂SO4, following which the excess base was back-titrated with 15.17 mL of 0.01102 M HCI. Calculate the sulfur concentration in the sample in parts per million.
A certain rust remover containing phosphoric acid has a density of 1.685 g/mL. Titration of a 59.3 mL sample of the rust remover requires 640 mL of 1.86 M NaOH to completely react with the acid to form sodium phosphate. What is the mass percent H3PO4 (98.0 g/mol) in the rust remover? Oa, 19.8% Ob. 14.6% Oc. 69.7% Od.85.1% Oe. 39.1%
2. A supplement was tested for iron content in a laboratory. First, a random sample of 10 tablets weighing a total of 13.7421 g was turned into fine powder. A scoop of this powder weighing 2.7544 g was then dissolved and precipitated as Fe(OH)3 which was then rinsed and ignited to a constant weight as Fe₂O3 (159.69 g/mol). The recorded constant weight of Fe₂O3 is 0.2629 g. a. What is the %Fe (55.85 g/mol) content of the supplement? b. What is the iron content of the supplement reported as g FeSO4.7H₂O (277.908 g/mol) per tablet?
solution after precipitation is complete. 68. The drawings below represent aqueous solutions. Solution A is 2.00 L of a 2.00-M aqueous solution of copper(II) nitrate. Solution B is 2.00 L of a 3.00-M aqueous solution of potas- sium hydroxide. (0) suiro Cu²+ ebro NO3 БО K+ OH™ A B a. Draw a picture of the solution made by mixing solutions A and B together after the precipitation reaction takes place. Make sure this picture shows the correct relative volume compared to solutions A and B, and the correct relative number of ions, along with the correct relative amount of solid formed. b. Determine the concentrations (in M) of all ions left in solution (from part a) and the mass of solid formed.
Consider the neutralization reaction 2 HNO3(aq) + Ba(OH)2(aq). 2 H2O(l) + Ba(NO3)2(aq) A 0.105 L sample of an unknown HNO3 solution required 42.5 mL of 0.250 M Ba(OH)2 for complete neutralization. Wha the concentration of the HNO3 solution? concentration: .098
A 0.205 g sample of a monoprotic acid was dissolved in 25 mL of water. The acid solution was titrated to its endpoint with 28.1 mL of 0.0788 M NaOH solution. What is the molar mass of the acid?
Jack was asked to determine iron (55.845 g/mol) content in dietary supplement. He tookfew random tablets and ground them into fine powder. Next, he weighed 3.116 g of thefine powder. Sample was dissolved and iron was precipitated as Fe(OH)3 (106.867 g/mol).The precipitate was then ignited to a constant weight of 0.355 g as Fe2O3 (159.69 g/mol).Report the iron content in dietary supplement as % w/w FeSO4·7H2O (278.01 g/mol).
What mass (in g) of silver chloride (MM = 142.32 g/mol) is formed from the reaction of 157.4 mL of a 0.101 M silver acetate solution with 48 mL of 0.109 M magnesium chloride solution?
What mass of Na3PO4 is required to produce 500.0 mL of solution that is 0.750 M in sodium ions? The molar mass of Na3PO4 is 163.94 g/mol and that of Na+ is 22.99 g/mol.