The alcohol content of a certain low alcohol beer was determined using volumetric analysis. In this analysis, a 17.1-mL sample of the beer was pipetted into a 100-mL volumetric flask and the solution was made up to the mark. Then 20.4 mL aliquots of his solution were titrated against acidified potassium dichromate solution, K,Cr,0, of concentration 0.077 mol/L. A mean titre (or volume of the titrant) of 19.9 mL was obtained. The equation for the analysis is: 2- 3+ 2 Cr,0, (aq) + 3 C,H,OH (aq) + 16 H (aq) = 4 Cr (aq) + 3 CH,COOH (aq) + 11 H,0 (I) What was the molarity of the alcohol in the beer?

The alcohol content of a certain low alcohol beer was determined using volumetric analysis. In this analysis, a 17.1-mL sample of the beer was pipetted into a 100-mL volumetric flask and the solution was made up to the mark. Then 20.4 mL aliquots of his solution were titrated against acidified potassium dichromate solution, K,Cr,0, of concentration 0.077 mol/L. A mean titre (or volume of the titrant) of 19.9 mL was obtained. The equation for the analysis is: 2- 3+ 2 Cr,0, (aq) + 3 C,H,OH (aq) + 16 H (aq) = 4 Cr (aq) + 3 CH,COOH (aq) + 11 H,0 (I) What was the molarity of the alcohol in the beer?

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

Chapter17: Electrochemistry

Section: Chapter Questions

Problem 80AP

See similar textbooks

Similar questions

A solution is made by dissolving 0.455 g of PbBr2 in 100 g of H2O at 50C. Based on the data in Table 8-1, should this solution be characterized as a. saturated or unsaturated b. dilute or concentrated
1. A 0.3516 g sample of commercial phosphate detergent was ignited at a heat to destroy the organic matter. The residue was taken up in hot HCI which converted P to H3PO4. The phosphate was precipitated as MGNH4PO4.6H2O by addition of Mg+ followed by aqueous NH3. After being filtered and washed, the precipitate was converted to Mg2P2O7 by ignition at 1000 OC. This residue weighed 0.2161 g. Calculate the percent P (30.974) in the sample? Ans 17.11%
A 25.00mL wastewater sample was analyzed for its Mg2+ content using a standard gravimetric method. the sample was diluted to 3.00L and an 11.00mL aliquot was treated to precipitate magnesium as MgNH4PO4.6H2O using (NH4)2HPO4 as the precipitating agent. the precipitate was then filtered, washed, dried, and ignited resulting in a 0.1325mg Mg2P2O7 residue. How much Mg (in ppm) is present in the original sample
Hydrogen peroxide solutions can easily be decomposed by dust, trace amounts of metals or light. It istherefore necessary to periodically determine the purity of the peroxide solutions.This can be done via a redox titration as follows: The density of a particular surgical grade hydrogen peroxide solution is 1.11g.cm-3. Exactly 10 mL of this solution was pipetted and quantitatively transferred, along with a sufficientamount of a dilute sulphuric acid solution, into a 250.00 mL volumetric flask and made up to the mark. A 25.00 mL portion of this diluted solution is pipetted into a conical flask, and titrated with a0.372 M KMnO4 solution. The endpoint of the titration is determined when the colourless solution in the conical flask turns apersistent bright pink due to the presence of excess permanganate ions. The average titration value is 26.20 mL of the KMnO4 solution 1.Determine the percentage of the hydrogen peroxide in the solution sample.2. Naturally occurring manganese…
A solid sample contains unknown amounts of potassium and magnesium chloride and moisture. 1.193 g of the sample is dissolved in water and the solution is diluted to 250.00 mL. 25.0 mL of the sample is allowed to pass through an H + -saturated cation exchanger, the eluate consuming 22.03 mL of a 0.100 M NaOH solution. The moisture content of the sample was determined to be 5.22%. Calculate the % by weight of potassium and magnesium chloride in the sample.
To analyze an aspirin sample, 0.3470 g of crushed tablets are weighed and treated with 50.00 mL 0.1155 M sodium hydroxide, boiling for 10 minutes. Under these conditions the acid acetylsalicylic (MW, 180) reacts according to: CH3COO-C6H4-COOH + 2 OH- → OH-C6H4-COO- + CH3COO- The excess NaOH is then titrated with 11.5 mL of 0.2100 M HCl. What is the purity of said show ?.
A NazCO3 standard solution is prepared by transferring 2.4817 grams of primary standard-grade sodium carbonate to a 250.0 mL volumetric flask, dissolving the sample in -100 ml of distilled deionized water, and diluted to the mark. A 25.00 mL aliquot is taken and titrated with 42.65 mL of HCI solution to the bromocresol green endpoint. Calculate the concentration of the HCI solution. (A 0.1598 M B 0.1098 M c) 0.3196 M (D) 0.05490 M
A chemist receive different mixtures for analysis with the statement that it contain NaOH, NaHCO3 , Na2CO3 or compatible mixtures of these substances together with the inert material. From the data given, identify the respective materials and calculate the percentage of each component. 1.000g samples and 0.2500 N HCl were used in all cases. Sample 1 With phenolphthalein as the indicator, 24.32 ml of HCl was used. A duplicate sample required 48.64 ml HCl using methyl orange as the indicator. Sample 2. With phenolphthalein as the indicator it uses 28.2 ml of HCl to make it colorless and added with methyl orange indicator and uses 11.3 ml of HCl to reach the end point.
A 10.00 ml sample with an unknown concentration of KNO3 was studied at 60° C. If an additional 2.4 g of KNO, were added to reach saturation. What was initial concentration of Q3 KNO, in M.
You are required to standardize a dilute solution of sulphuric acid, and undertake the following steps:(i) 4.805 g of solid sodium tetraborate (Na2B4O7) are added to a 250 mL volumetric flask, and the solution made up to the mark with distilled water.(ii) 25.00 mL aliquots of the stock solution from (i) are transferred to conical flasks, for titration against the sulphuric acid solution in the burette.(iii) You perform titrations using two different indicators: bromocresol green, and phenolphthalein.With bromocresol green, the average titre volume is 22.50 cm3, while with phenolphthalein, the average volume is 9.50 cm3.(a) Write the balanced equation for the reaction between Na2B4O7 and sulphuric acid
When treating a mixture of metals( copper and zinc) with an excess of solution of hydrochloric acid, 2.24 liters of a gas(STP) were released. When the same mixture was treated with phosphoric acid precipitate of 93.5g is formed. Find the mass fraction of metals in the initial mixture.
A 0.1530 g of pure KIO3 was dissolved in 50 mL distilled water. This was then added with KI and 6N H₂SO4. After allowing the said solution to stand in the dark for 3 minutes, this was then titrated to end point with 31.35 mL sodium thiosulfate solution, with starch as the indicator. What is the normality of the sodium thiosulfate solution? Atomic weights: K = 39.1 1= 126.9 O= 16.0