The amount of I, (aq) in a solution can be determined by titration with a solution containing a known concentration of S,0; (aq) (thiosulfate ion). The determination is based on the net ionic equation 25,0, (aq) + 15(aq) s,0 (aq) + 31 (aq) Given that it requires 34.6 ml of 0.460 M Na,s,0, (aq) to titrate a 15.0 ml sample of I, (aq), calculate the molarity of 5 (aq) in the solution. 51 = M + TOOLS

The amount of I, (aq) in a solution can be determined by titration with a solution containing a known concentration of S,0; (aq) (thiosulfate ion). The determination is based on the net ionic equation 25,0, (aq) + 15(aq) s,0 (aq) + 31 (aq) Given that it requires 34.6 ml of 0.460 M Na,s,0, (aq) to titrate a 15.0 ml sample of I, (aq), calculate the molarity of 5 (aq) in the solution. 51 = M + TOOLS

Chemistry: Principles and Reactions

8th Edition

ISBN:9781305079373

Author:William L. Masterton, Cecile N. Hurley

Publisher:William L. Masterton, Cecile N. Hurley

Chapter4: Reactions In Aqueous Solution

Section: Chapter Questions

Problem 58QAP: The iron content of hemoglobin is determined by destroying the hemoglobin molecule and producing...

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The iron content of hemoglobin is determined by destroying the hemoglobin molecule and producing small water-soluble ions and molecules. The iron in the aqueous solution is reduced to iron(II) ion and then titrated against potassium permanganate. In the titration, iron(ll) is oxidized to iron(III) and permanganate is reduced to manganese(II) ion. A 5.00-g sample of hemoglobin requires 32.3 mL of a 0.002100 M solution of potassium permanganate. The reaction with permanganate ion is MnO4(aq)+8H+(aq)+5Fe2+(aq)Mn2+(aq)+5Fe3+(aq)+4H2O What is the mass percent of iron in hemoglobin?
A student prepares a dilute solution of sodium hydroxide, NaOH (aq), starting with 6 M sodium hydroxide. She then titrates a 1.372 g sample of KHP with the dilute sodium hydroxide solution, NaOH (aq), to a phenolphthalein end point. 1. If the titration required 21.84 mL of sodium hydroxide, NaOH (aq), calculate the molar concentration of the sodium hydroxide solution, NaOH (aq). (Remember that KHP is potassium hydrogen phthalate, KHC8H4O4, NOT potassium hydrogen phosphorus!) 2.The student uses the same sodium hydroxide to titrate 10.00 mL of vinegar to a phenolphthalein end point. If the titration required 27.48 mL of sodium hydroxide, NaOH (aq), calculate the molar concentration of acetic acid, HC2H3O2 (aq), in the vinegar. 3. Calculate the mass percent of acetic acid, HC2H3O2 (aq), in the vinegar using the molar concentration for acetic acid, HC2H3O2 (aq), determined in part b and assuming the density of the solution is 1.01 g/mL.
A sample containing NaCl, NaBr, and inert materials weighs 1.000 g. With excess AgNO3 it gives a precipitate of AgCl and AgBr, which weighs 0.5260 g. By heating this precipitate in a current of Cl2 gas, the AgBr is converted to AgCl and the resulting precipitate then weighs 0.4260 g. What is the %NaCl and %NaBr present in the original sample?
A student prepares a dilute solution of sodium hydroxide, NaOH (aq), starting with 6 M sodium hydroxide. She then titrates a 1.372 g sample of KHP with the dilute sodium hydroxide solution, NaOH (aq), to a phenolphthalein end point. a) If the titration required 21.84 mL of sodium hydroxide, NaOH (aq), calculate the molar concentration of the sodium hydroxide solution, NaOH (aq). (Remember that KHP is potassium hydrogen phthalate, KHC8H4O4, NOT potassium hydrogen phosphorus!) b) The student uses the same sodium hydroxide to titrate 10.00 mL of vinegar to a phenolphthalein end point. If the titration required 27.48 mL of sodium hydroxide, NaOH (aq), calculate the molar concentration of acetic acid, HC2H3O2 (aq), in the vinegar. c) Calculate the mass percent of acetic acid, HC2H3O2(aq), in the vinegar using the molar concentration for acetic acid, HC2H3O2 (aq), determined in part b and assuming the density of the solution is 1.01 g/mL.
A student prepares a dilute solution of sodium hydroxide, NaOH (aq), starting with 6 M sodium hydroxide. She then titrates a 1.372 g sample of KHP with the dilute sodium hydroxide solution, NaOH (aq), to a phenolphthalein end point. A.) If the titration required 21.84 mL of sodium hydroxide, NaOH (aq), calculate the molar concentration of the sodium hydroxide solution, NaOH (aq). (Remember that KHP is potassium hydrogen phthalate, KHC8H4O4, NOT potassium hydrogen phosphorus!) B.) The student uses the same sodium hydroxide to titrate 10.00 mL of vinegar to a phenolphthalein end point. If the titration required 27.48 mL of sodium hydroxide, NaOH (aq), calculate the molar concentration of acetic acid, HC2H3O2 (aq), in the vinegar. C.) Calculate the mass percent of acetic acid, HC2H3O2 (aq), in the vinegar using the molar concentration for acetic acid, HC2H3O2 (aq), determined in part b and assuming the density of the solution is 1.01 g/mL.
The tartaric acid, H2C4H4O6 (150.087 g/mol ) concentration in 100.0 mL wine sample was determined using 0.4050 M sodium hydroxide standard solution. In the experiment, the %w/w of tartaric acid present in the wine sample by analyzing and titrating only 25.00 mL aliquot from the 100-ml wine sample. The endpoint of titration was reached upon the addition of exactly 43.56 mL NaOH solution? (Assume the density of the wine sample is 1.000 g/mL) H2C4H4O6 + 2NaOH⟶Na2C4H4O6+2H2O What is the total (%w/w) acid content in the wine sample? 1.324 %w/w 2.648 %w/w 5.296 %w/w 10.59 %w/w
To measure the amount of calcium carbonate CaCO3 in a seashell, an analytical chemist crushes a 4.500g sample of the shell to a fine powder and titrates it to the endpoint with 172.mL of 0.380M hydrogen chloride HCl solution. The balanced chemical equation for the reaction is: →+2HClaq CO2−3aq + H2CO3aq 2Cl−aq What kind of reaction is this? Percipitation, acid-base, or redox Calculate the mass percent of CaCO3 in the sample. Be sure your answer has the correct number of significant digits.
(a) Identify the species that was reduced in the titration reaction. Justify your answer in terms of oxidation numbers. (c) Given that the concentration of KMnO4(aq) was 0.0235M, calculate the number of moles of MnO4− ions that completely reacted with the H2C2O4. d) The student proposes to perform another titration using a 0.139g sample of H2C2O4, but this time using 0.00143MKMnO4(aq) in the buret. Would this titrant concentration be a reasonable choice to use if the student followed the same procedure and used the same equipment as before? Justify your respons
You have been provided with a 35.7 mL sample of lithium hydroxide (LiOH) of unknown concentration. You perform a titration with 1.75 M nitric acid (HNO3), and find that 2.37 × 10−2 L are required to reach the equivalence point (as determined using a coloured indicator). What is the concentration of the lithium hydroxide solution in mol L−1? Report your answer to the correct number of significant figures.
A solution is prepared by pipetting 25.0 mL of 0.350 M CuCl2 into a 100.0 mL volumetric flask, diluting to the calibration mark on the flask with water and quantitatively mixing the contents of the flask. What is the molar concentration of Cl- in the solution?
A 0.5504-g sample of KHP (potassium hydrogen phthalate, KHC8H4O4; molar mass = 204.22 g/mol) is completely dissolved in enough deionized water to make 50.00 mL of solution. The resulting solution is titrated with a NaOH solution of unknown concentration. If 21.50 mL of the base solution is needed to reach the end-point, what is the molar concentration of NaOH solution? The reaction occurs as follows: NaOH(aq) + KHC8H4O4(aq) --> NaKC8H4O4(aq) + H2O(l) (A) 0.2457 M (B) 0.1254 M (C) 0.05390 M (D) 0.03823 M
Iodometry is a standard method for redox titration. In many indirect methods one lets the analyte (the substance whose concentration is to be determined) react with iodide ions as then forms triiodide ions, I3- . The amount of triiodide ions is then determined by titration with thiosulphate ions, S2O32- which then form tetrathionate ions, S4O62- whereby the triiodide ions change into iodide ions. Determine the mass of triiodide ions in a solution from the following data. The sample containing triiodide ions was titrated with a 0.01002 M sodium thiosulfate solution of which 18.38 mL were required.