odometric titration of Vitamin C with sodium thiosulfate How many moles of iodine (I2) react with the thiosulfate? The equation is.. 5.66 x 10-4 M of sodium thiosulfate used in titration 0.62 g in 0.01 M in 250 mL conical flask 0.00075 M of iodine in the conical flask 0.00025 M of potassium iodate 1 iodine mole : 2 sodium thiosulfate mols

odometric titration of Vitamin C with sodium thiosulfate How many moles of iodine (I2) react with the thiosulfate? The equation is.. 5.66 x 10-4 M of sodium thiosulfate used in titration 0.62 g in 0.01 M in 250 mL conical flask 0.00075 M of iodine in the conical flask 0.00025 M of potassium iodate 1 iodine mole : 2 sodium thiosulfate mols

Fundamentals Of Analytical Chemistry

9th Edition

ISBN:9781285640686

Author:Skoog

Publisher:Skoog

Chapter17: Complexation And Precipitation Reactions And Titrations

Section: Chapter Questions

Problem 17.35QAP

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Iodometric titration of Vitamin C with sodium thiosulfate How many moles of iodine (I2) react with the thiosulfate? (reacts in a 1:2 ratio) 5.66 x 10-4 M of sodium thiosulfate used in titration 0.62 g in 0.01 M in 250 mL conical flask 0.00075 M of iodine in the conical flask 0.00025 M of potassium iodate
The potassium hydrogen phthalate, KHP, is a common primary standard used in the standardization of a strong base titrant. It is a monoprotic acid and reacts on a 1:1 stoichiometric ratio with NaOH. STANDARDIZATION OF NAOH SOLUTION A 0.4047 g sample of primary standard grade potassium hydrogen phthalate (MM = 204.23) was dissolved in distilled H2O. The solution required 22.42 mL of the NaOH solution to reach the phenolphthalein end point. How many moles of NaOH will react with the KHP dissolved in water?
A 75.0 mL solution of potassium iodate (KIO3, 214.0 g/mol, 98%) was treated with KI and H2SO4 and then titrated with sodium thiosulfate (Na2S2O3, 158.1 g/mol). The titration required 5.00 mL of the titrant. If the solution contained 0.0325 g of the primary standard, what is the concentration of the titrant?
A 1.7483-g sample containing Al(NO3)3, AlCl3, and inert material was dissolved in acid and divided into two equal portions. One portion was treated with 5.00 mmol of AgNO3. The excess Ag+ required 28.89 mL of 0.l002 M KSCN for titration. The other portion required 26.02 mL of 0.1193 M NaOH for titration:Al3+ + 3 OH- → Al(OH)3(s)Calculate the percentage composition of Al(NO3)3 and AlCl3 in the sample.
2.4414 g sample containing KCl, K2SO4and inert materials was dissolved in sufficient water to give 250 mL of solution. A Mohr titration of a 50 mLaliquot required 41.36 mL of 0.05818 M AgNO3. A second 50mL aliquot was treated with 40 mL of 0.1083M NaB(C6H5)4. The reaction is NaB(C6H5)4+ K+ KB(C6H5)4(s)+ Na+. The solid was filtered, redissolved in acetone, and titrated with 49.98mLof the AgNO3solution according to the reaction KB(C6H5)4+ Ag+ AgB(C6H5)4(s)+ K+. Calculate the percentage of KCl and K2SO4in the sample.
2.4414 g sample containing KCl, K2SO4and inert materials was dissolved in sufficient water to give 250 mL of solution. A Mohr titration of a 50 mLaliquot required 41.36 mL of 0.05818 M AgNO3. A second 50mL aliquot was treated with 40 mL of 0.1083M NaB(C6H5)4. The reaction is NaB(C6H5)4+ K=KB(C6H5)4(s)+ Na+. The solid was filtered, redissolved in acetone, and titrated with 49.98mLof the AgNO3solution according to the reaction KB(C6H5)4+ Ag= AgB(C6H5)4(s)+ K+. Calculate the percentage of KCl and K2SO4 in the sample.
A 25.0025.00 mL solution of 0.088300.08830 M NaINaI is titrated with 0.051500.05150 M AgNO3AgNO3. Calculate pAg+pAg+ following the addition of the given volumes of AgNO3AgNO3. The KspKsp of AgIAgI is 8.3×10−178.3×10−17. 37.40 mLpAg+=37.40 mLpAg+= VepAg+=VepAg+= 47.30 mLpAg+=47.30 mLpAg+=
Consider the titrimetric determination of acetic acid (60.05 g/mol) in vinegar. Titration of a 5.00 mL vinegar sample requires 14.25 mL of 0.150 M NaOH to reach the phenolphthalein endpoint. What is the molarity of acetic acid? choices 1.24 0.808 0.428 0.0526
Molarity of Na2S2O3 (stock solution). 0.100 M Volume of diluted bleach titrated (taken from the volumetric flask). 10ml Initial Burette Reading. 14.80 Final Burette Reading 25.60 Volume of Na2S2O3 used in the titration (mL). 10.80 Moles of Na2S2O3 used in the titration. 1.71 Moles of S2O3–2 used. 1.66 Moles of I2 initially present in titration mixture 0.83 Moles of NaOCl in the diluted bleach titrated. 0.415 Volume of bleach titrated. 1ml Mass of commercial bleaching solution titrated ?
Molarity of Na2S2O3 (stock solution). 0.100 M Volume of diluted bleach titrated (taken from the volumetric flask). 10ml Initial Burette Reading. 14.80 Final Burette Reading 25.60 Volume of Na2S2O3 used in the titration (mL). 10.80 Moles of Na2S2O3 used in the titration. 1.71 Moles of S2O3–2 used. 1.66 Moles of I2 initially present in titration mixture 0.83 Moles of NaOCl in the diluted bleach titrated. 0.415 Volume of bleach titrated. 1ml Mass of NaOCl in commercial bleach titrated. ?
Molarity of Na2S2O3 (stock solution). 0.100 M Volume of diluted bleach titrated (taken from the volumetric flask). 10ml Initial Burette Reading. 14.80 Final Burette Reading 25.60 Volume of Na2S2O3 used in the titration (mL). 10.80 Moles of Na2S2O3 used in the titration. 1.71 Moles of S2O3–2 used. 1.66 Moles of I2 initially present in titration mixture 0.83 Moles of NaOCl in the diluted bleach titrated. 0.415 Mass of NaOCl in the diluted bleach titrated. ?
Molarity of Na2S2O3 (stock solution). 0.100 M Volume of diluted bleach titrated (taken from the volumetric flask). 10ml Initial Burette Reading. 14.80 Final Burette Reading 25.60 Volume of Na2S2O3 used in the titration (mL). 10.80 Moles of Na2S2O3 used in the titration. 1.71 Moles of S2O3–2 used. 1.66 Moles of I2 initially present in titration mixture 0.83 Moles of NaOCl in the diluted bleach titrated. 0.415 Moles of OCl– in the diluted bleach titrated. ?