was acidified and analyzed using excess iodine ion. Then I−3 is titrated with 0.320M Na2S2O3. If the titre volume is 28.25mL, calculate the % of NaNO2 in the sample. (MM of NaNO2= 68.9953 g/mol). Hint: the stoich ratio between NaNO2 and HNO2 is just 1:1. 2HNO2 + 3H+ → 2NO + 2H2O + I−3 S2O3−2 + I−3 → I− + S4O6−2

was acidified and analyzed using excess iodine ion. Then I−3 is titrated with 0.320M Na2S2O3. If the titre volume is 28.25mL, calculate the % of NaNO2 in the sample. (MM of NaNO2= 68.9953 g/mol). Hint: the stoich ratio between NaNO2 and HNO2 is just 1:1. 2HNO2 + 3H+ → 2NO + 2H2O + I−3 S2O3−2 + I−3 → I− + S4O6−2

Principles of Modern Chemistry

8th Edition

ISBN:9781305079113

Author:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Publisher:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Chapter11: Solutions

Section: Chapter Questions

Problem 26P

See similar textbooks

Similar questions

For the determination of basic species in 0.1878 g Talcid sample; 20 mL of 0.1009 M HCl solution was added to the sample and the necessary procedures were carried out and titrated with 0.1097 M NaOH solution. Since 10.2 mL of base solution is consumed at the end of the titration, which of the following is the% base amount in CaCO3? (CaCO3: 100,087 g / mol) A. 23.96B. 55.1C. 45.1D. 42.1
During the titration of an HClO4 solution with 0.10320 M NaOH, a student, Lovely became distracted and overshot the endpoint. A fellow student Ashley suggested that he should record the present volume of NaOH added and titrate the excess with a standard acid solution. If the original sample volume was 25.000 mL, the volume of NaOH added was 28.060 mL. It took 3.4700 mL of 0.10940 M HCl to back-titrate the NaOH and calculate the molar concentration of the original HClO4
During the titration of an HClO4solution with 0.10320M NaOH, a CHEM 3A student,Juan becamedistracted and overshot the endpoint. A fellow student Pedrosuggested that he should record the present volume of NaOH added and titrate the excess with a standard acid solution. If the original sample volume was 25.000mL, the volume of NaOH added was 28.060mL. It took 3.4700 mL of 0.10940 M HCl to back-titrate the NaOH andcalculate the molar concentration of the original HClO4solution.
A 0.4126-g sample of primary-standard Na2CO3 was treated with 40.00 mL of dilute perchloric acid. The solution was boiled to remove CO2, following which the excess HClO4 was back - titrated with 9.20 mL of dilute NaOH. In a separate experiment, it was established that 26.93 mL of the HClO4 neutralized the NaOH in a 25.00-mL portion. Calculate the molarities of the HClO4 and NaOH.
Calculate the concentration of Na2S2O3 if it requires 25.00 mL of the titrant to react with 0.02500g of KIO3. (molar mass of KIO3 = 214 g/mol)
Calculate the molar concentration of H3O+ ions and the pH of the following solutions: (a) 25.0 cm3 of 0.144 M HCI(aq) was added to 25.0 cm3 of 0.125 M NaOH(aq), (b) 25.0 cm3 of 0.15 M HCI(aq) was added to 35.0 cm3 of 0.15 M KOH(aq), (c) 21.2 cm3 of 0.22 M HNO3(aq) was added to 10.0 cm3 of 0.30M NaOH(aq).
A pure organic compound has the formula C4H8SOx. A sample of a compound wasdecomposed; the sulfur was converted to sulfate and titrated in a modified version of theadsorption indicator procedure. From the following data, determine the correct formula forthe compound.Given: weight of sample = 12.64 mgBa(ClO4)2 needed for titration = 10.60 mL of 0.0100 M Ba(ClO4)2
You are given a solution of HCOOH (formic acid) with an approximate concentration of 0.20 M and you will titrate this with a 0.1105 MM NaOH. If you add 20.00 mL of HCOOH to the beaker before titrating, approximately what volume of NaOH will be required to reach the end point?
KHP is a monoprotic acid which provides one H+ ion. How would your results be affected if a diprotic acid (such as sulfuric acid, H2SO4) was used which provides two H+ ions? Calculate the molarity of the NaOH solution if 16.00 mL of NaOH was titrated against 14.00 mL of 1.25 M H2SO4. Do not include units with your answer.
The tartaric acid, H2C4H4O6 (150.087 g/mol ) in 100.0 mL wine sample was determined using 0.4050 M sodium hydroxide standard solution. In the experiment, the %w/w of acid present in the 100.0 mL wine sample if he titrated a 25.00 mL aliquot using 43.56 mL NaOH solution? (Assume the density of the wine sample is 1.000 g/mL) What is the total (%w/w) acid content in the wine sample?
calculate molarity of acetic acid in vinegar: (volume of NaOH 3ml, cincentration of NaOH 24.215, titrate average use of NaOH 3.44mL). then convert your M concentration of acetic acid to %w/w, given the density of vinegar is 1.005 g/mL.
You are given a solution of HCOOH (formic acid) with an approximate concentration of 0.20 M and you will titrate this with a 0.1105 M NaOH. If you add 20.00 mL of HCOOH to the beaker before titrating, approximately what volume of NaOH will be required to reach the end point?