An aqueous ethylene glycol (HOCH₂CH₂OH, FW = 62.07 g/mol) solution with a mass of 214.3 mg is titrated with 61.9 mL of 0.0867 M Ce in 4 M HCIO. The solution is held at 60 °C for 15 min to oxidize the ethylene glycol to formic acid (HCO,H) and carbon dioxide. The excess Cet is titrated with 10.57 mL of 0.0479 M Fe²+ to a ferroin end point. What is the mass percent of ethylene glycol in the unknown solution?

An aqueous ethylene glycol (HOCH₂CH₂OH, FW = 62.07 g/mol) solution with a mass of 214.3 mg is titrated with 61.9 mL of 0.0867 M Ce in 4 M HCIO. The solution is held at 60 °C for 15 min to oxidize the ethylene glycol to formic acid (HCO,H) and carbon dioxide. The excess Cet is titrated with 10.57 mL of 0.0479 M Fe²+ to a ferroin end point. What is the mass percent of ethylene glycol in the unknown solution?

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

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 55.0 mL sample of 0.102M potassium sulfate solution is mixed with 35.0 mL of a 0.114M lead(II) acetate solution and the precipitation reaction shown here occurs: K2SO4(aq)+Pb(C2H3O2)2(aq)=2KC2H3O2(aq)+PbSO4(s). Determine the limiting reagent.
A 500.0-mg sample of impure sodium bicarbonate (NaHCO3; MM = 84.01 g/mol) is analyzed by titrating the sample with standard 0.1288 M HCI solution, requiring 38.27 mL. The reaction is NaCl + H₂O + CO₂ NaHCO3 + HCI Calculate the percent sodium bicarbonate in the sample. 0.9858% 82.82% 4.929% 0.08282% -
In the chemistry lab, aqueous solutions of sulfuric acid are usually prepared from a concentrated reagent of this acid which has a concentration of 18.4 M. To prepare a dilute solution of this acid, 1.00 mL of the concentrated reagent is dissolved in enough water and the volume of the mixture is adjusted to 1.00 L. In this process, sulfuric acid reacts with water to produce hydronium and sulfate ions,H2SO4(aq) + H2O(l) → H3O+(aq) + SO42-(aq)This reaction is known as acid-dissociation reaction. It is an example of an acid-base reaction where the acid (sulfuric acid) transfer its protons (H+) to a base (water). a. Balance the above chemical equation. b. Calculate the concentration (in molarity) of H3O+ in the prepared dilute solution of sulfuric acid. c. The strength of an acid can be measured by of the molar concentration of hydronium H3O+ (usually denoted as [H3O+]) produced when acid dissociates in water. The greater the [H3O+] the stronger is the acid. The value of [H3O+] is usually…
A chemistry student needs to standardize a fresh solution of sodium hydroxide. He carefully weighs out 54. 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 his sodium hydroxide solution. When the titration reaches the equivalence point, the student finds he has used 92.3 mL of sodium hydroxide solution. Calculate the molarity of the student's sodium hydroxide solution. Round your answer to 2 significant digits. do O Ar M X ?
The aluminum (AW=26.98 g/mol) in a 1.000-g sample of impure ammonium aluminum sulfate was precipitated with aqueous ammonia as the hydrous Al203.xOH. The precipitate was filtered and ignited at 1000 °C to give anhydrous Al203 (FW=101.96 g/mol), which weighed 0.2001 g. Calculate the % NH4AlSO4 (FW= 141.08 g/mol
A permanganate solution is prepared by dissolving 20.0123 g KMNO4 in 500 mL of distilled water and boiled for 1 hour to remove any organic material. Following sintered-glass filtration, the solution is quantitatively transferred to a 1.0 L volumetric flask and diluted to volume with distilled water. The permanganate solution was titrated against 0.1023 M oxalic acid prepared in sulfuric acid solution. A 50.00 mL aliquot of oxalic acid solution required 16.68 mL of permanganate solution. A titration blank required 0.04 mL of permanganate. What is the permanganate molarity? 5 H2C204 + 2 MnO4 + 6H* s 10 CO2 + 2 Mn²* + 8 H2O
Malic acid (C4H6O5) is a dicarboxylic acid that naturally occurs in the production of bignay wine. Maria was tasked to find out the acid content in a 200.0 mL wine sample by titrating it with a standardized solution of KOH. He was able to establish the working concentration of the KOH solution by using 39.12 mL of it to titrate a primary standard of KHP that weighed 3.021 g. The grams and %w/w of Malic acid present in the 200.0 mL wine sample were then determined by titrating a 20.00 mL aliquot using 48.95 mL of the standardized KOH solution. C4H6O5 (aq) + 2KOH (aq) ↔ K2C4H4O5 (aq) + 2H2O (l) Assume the density of the wine sample is 1.000 g/mL MM of KHP = 204.22 g/mol MM of C4H6O5 = 134.0874 g/mol ? What is the molar concentration of the prepared KOH solution?…
When 6.881 g of MgCl2 and NaCl mixture is dissolved in 500 mL of distilled water and 50 mL of AgNO3 is precipitated, 0.5923 g of AgCl precipitates are formed. The Mg in the other 50 mL portion is precipitated as MgNH4PO4. Calculate the percentages of MgCl2 and NaCl in the sample as the 0.1796 g Mg2P2O7 is weighed after the precipitate is heated.
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
4. A certain barium halide exists as the hydrated salt BaX2.2H2O, where X is the halogen. The barium content of the salt can be determined by gravimetric methods. A sample of the halide (0.2650 g) was dissolved in water (200 cm3) and excess sulfuric acid added. The mixture was then heated and held at boiling for 45 minutes. The precipitate (barium sulfate) was filtered off, washed and dried. Mass of precipitate obtained = 0.2533 § Determine the identity of X. 3 g.