Your titration involves using a 25.00mL pipette to deliver the ascorbic acid star (C,H3O6) to the conical flask beneath the burette then adding to this the unkn (12) until the end point is reached. The balanced equation for the reaction is gi CH&O6 + 12 → C6H,O6 + 21° + 2H* What is the number of moles of ascorbic acid (C&HgOg) in 25.00mL of the stan concentration 0.005mol/L? On = 0.125 O n= 0.20 O n= 1.25 x 104 On= 2.0 x 104

Your titration involves using a 25.00mL pipette to deliver the ascorbic acid star (C,H3O6) to the conical flask beneath the burette then adding to this the unkn (12) until the end point is reached. The balanced equation for the reaction is gi CH&O6 + 12 → C6H,O6 + 21° + 2H* What is the number of moles of ascorbic acid (C&HgOg) in 25.00mL of the stan concentration 0.005mol/L? On = 0.125 O n= 0.20 O n= 1.25 x 104 On= 2.0 x 104

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

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The SO2 present in air is mainly responsible for the phenomenon of acid rain. The concentration of SO2 can be determined by titrating against a standard permanganate solution as follows: 5SO2 + 2MnO4- + 2H2O ---> 5SO42- + 2Ms2 + 4H+ Calculate the number of grams of SO2 in a sample of air if 4.90mL of 0.00700M KMnO4 solution are required for the titration. Be sure your answer has the correct number of significant digits.
A commercial vinegar was analyzed by titration to determine the percent acetic acid. Briefly, 10.00 mL of vinegar sample was diluted to 100. mL solution in volumetric flask. A 25.00 mL aliquot from the diluted vinegar required 25.55 mL of 0.1005 M NaOH to reach the phenolphthalein endpoint. Which is the correct equation between the analyte and titrant reaction? CH3COOH + NaOH → NaCH3COO + H2O 2CH3COOH + NaOH → NaCH3COO + H2O C20H14O4 + NaOH → NaC20H14O4 + H2O CH3COOH + 2NaOH → NaCH3COO + H2O
(Eqn. 1) 1 OCl− + 3 I− + 2 H+ → 1 I3− + 1 Cl− + 1 H2O (Eqn. 2) 2 S2O32− + 1 I3− + 0 H+ → 3 I− + 1 S4O62− + 0 H2O Multiply Equation 2 by the molar ratio of 1/1 and add to Equation 1 to obtain the overall balanced net ionic equation for the titration of the diluted bleach sample. 1) What is the molar ratio of OCl− to S2O32− in the overall net ionic equation?
A 11.00 gram sample of Vodka was analysed for its alcohol content. The sample was placed in a300 mL volumetric flask and made to the mark with distilled water. A 20.0 mL aliquot of the dilutedVodka was taken from the volumetric flask and placed in a conical flask containing some distilled water from a previous washing.The 20.0 mL aliquots were titrated against a 0.1302 M Cr2O72-solution and an average titre of13.25 mL was obtained.The reaction between the alcohol and the dichromate solution is given below2Cr2O72–(aq) + 3CH3CH2OH(aq) + 16H+(aq)  4Cr3+(aq) + 3CH3COOH(aq) + 11H2O(l)a) Calculate the amount in mol of Cr2O72– in the average titre. b) Calculate the percentage, by mass, of ethanol in the vodka.
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The protein content of wheat flour can be determined reasonably accurately by multiplying the percentage of nitrogen present by 5.7. A 2.06-g sample of flour was taken through a Kjeldahl procedure and the ammonia produced was distilled into a boric acid solution. If this solution required 34.70 mL of 0.174 N HCl for titration to the methyl red end point, what is the a) % Nitrogen and b) % protein in the flour? (Use 1:1 stoich ratio between N and HCl)
A 1.000-g sample containing KHC2O4, H2C2O4, and impurities required 38.22 mL of 0.1000 M NaOH for acid-base titration. Another 1.000-g sample required 27.02 mLof 0.04000 M KMnO4 for redox titration in acid solution, according to the following reaction: MnO4- + 5C2O42- + 16H+ ⇄ 2Mn2+ + 10CO2 + 8H2O How many mmols of KHC2O4 are there in the sample?
The solubility of borax, which is made up of sodium tetraborate (Na2B4O5(OH)4 8H2O), was analyzed. The dissolution of borax is: Na2B4O5(OH)4 • 8H2O(s) ⇌ 2 Na+(aq) + B4O5(OH)42–(aq) + 8 H2O(l) A 50 mL saturated solution was prepared. After filtration of solution, 5 mL aliquot was transferred to a flask and titrated using 0.432 M HCl. The endpoint was found to be 4.73 mL of the titrant. Tetraborate anion (B4O5(OH)42-) is a weak base which reacts with HCl like the following reaction: B4O5(OH)42–(aq) + 2 H+(aq) + 3 H2O(l) ⇌ 4 H3BO3(aq) What is Ksp expression for the dissolution? What is the tetraborate ions concentration in the filtrate? What is the molar solubility and Ksp of borax if the titration was done at room temperature (298 K)?
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1. 2MnO4— + 5C2O42— + 16H+ 2Mn2+ + 10CO2 + 8H2O A solution of KMnO4 was prepared and 50.99 mL was used to completely titrate 0.5355 g of pure Na2C2O4. What is the concentration of the KMnO4 solution? Na2C2O4 = 134.00 g/mol 2. Titration of the I2 produced from 0.2645g of primary standard KIO3 required 45.36mL of sodium thiosulfate. Calculate the concentration of the Na2S2O3 in M. IO3- + 5I- + 6H+ --> 3I2 + 3H2O I2 + 2S2O32- --> 2I- + S4O62- KIO3 mw = 214.001g/mol
please help me The aluminum in a 1.200g sample of impure ammonium aluminum sulfate was precipitatedwith aqueous ammonia as the hydrous Al2O3 · XH2O. The precipitate was filtered and ignitedat 100°C to give anhydrous Al2O3, which weighed 0.2001 g. Express the result of this analysisin terms of % Al.
You were assigned to assay a product sample of milk of magnesia. A 0.600-g sample was reacted with 25.00 mL 0.10590 N H2SO4 . The excess unreacted acid in the solution required 13.00 mL of 0.09500 N NaOH when titrated to reach the methyl red end point. Determine the dosage strength of the product in terms of % Mg(OH)2 content. Type your answer in 2 decimal places, numbers only.