CtrlCapsShiftM Inbox (1,543)-ftantill@udeledu xMail-Francesca A Tantillo-Out xHomepage-CHM150-251 Chen X← C- сapp.101edu.coQuestion 19 of 20Vitamin C (ascorbic acid, CeHsO6, 176.12 g/mol) can be measured byredox titration with iodine solution. lodine is reduced to iodide ion,while ascorbic acid is oxidized to dehydroascorbic acid (C6H6O6). Theiodine solution is usually made in the presence of iodide ion, formingthe more stable triiodide ion, Is, giving the following overall reactionCeHsOc(aq) + Is (aq) + H₂O(1)→ CHO(aq) + 31-(aq) + 2H+(aq)The titration is carried out in the presence of starch, which forms adark blue complex with the excess iodine when the endpoint isreached. Ascorbic acid can be used to standardize the iodine solution.A 0.315 g sample of ascorbic acid was titrated with iodine solution,requiring 30.2 mL to reach the endpoint.Calculate [ls], the molar concentration of Is ion in the solution.OLTabEnEsc79°FSunny!1QANFI@2WSF2X#3EDF3$4CRF4FDII ESFS%105TVG후A6F6YAktiv ChemistryB*HF7&V po7PrtScnX +NHome★8UJOJF9M(9KEndOF10)147+/-PgUp0F11258PgDnPJILAR

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Mail-Francesca A Tantillo-Out X Homepage-CHM150-251 Chen X Question 19 of 20 Vitamin C (ascorbic acid, C&H:06, 176.12 g/mol) can be measured by redox titration with iodine solution. lodine is reduced to iodide ion, while ascorbic acid is oxidized to dehydroascorbic acid (CHO). The iodine solution is usually made in the presence of iodide ion, forming the more stable triiodide ion, Is, giving the following overall reaction CeHsOc(aq) + Is (aq) + H₂O(1)→ CHOs(aq) +31-(aq) + 2H*(aq) The titration is carried out in the presence of starch, which forms a dark blue complex with the excess iodine when the endpoint is reached. Ascorbic acid can be used to standardize the iodine solution. A 0.315 g sample of ascorbic acid was titrated with iodine solution, requiring 30.2 mL to reach the endpoint. Calculate [ls], the molar concentration of Is ion in the solution. LO M Inbox (1,543)-ftantill@udeledu x ← C app.101edu.co Aktiv Chemistry 79°F Sunny + 4 7 +/- 2 5 8

Mail-Francesca A Tantillo-Out X Homepage-CHM150-251 Chen X Question 19 of 20 Vitamin C (ascorbic acid, C&H:06, 176.12 g/mol) can be measured by redox titration with iodine solution. lodine is reduced to iodide ion, while ascorbic acid is oxidized to dehydroascorbic acid (CHO). The iodine solution is usually made in the presence of iodide ion, forming the more stable triiodide ion, Is, giving the following overall reaction CeHsOc(aq) + Is (aq) + H₂O(1)→ CHOs(aq) +31-(aq) + 2H*(aq) The titration is carried out in the presence of starch, which forms a dark blue complex with the excess iodine when the endpoint is reached. Ascorbic acid can be used to standardize the iodine solution. A 0.315 g sample of ascorbic acid was titrated with iodine solution, requiring 30.2 mL to reach the endpoint. Calculate [ls], the molar concentration of Is ion in the solution. LO M Inbox (1,543)-ftantill@udeledu x ← C app.101edu.co Aktiv Chemistry 79°F Sunny + 4 7 +/- 2 5 8

Chemistry: An Atoms First Approach

2nd Edition

ISBN:9781305079243

Author:Steven S. Zumdahl, Susan A. Zumdahl

Publisher:Steven S. Zumdahl, Susan A. Zumdahl

Chapter14: Acid- Base Equilibria

Section: Chapter Questions

Problem 118CP: Malonic acid (HO2CCH2CO2H) is a diprotic acid. In the titration of malonic acid w ith NaOH,...

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Malonic acid (HO2CCH2CO2H) is a diprotic acid. In the titration of malonic acid w ith NaOH, stoichiometric points occur at pH = 3.9 and 8.8. A 25.00-mL sample of malonic acid of unknown concentration is titrated with 0.0984 M NaOH, requiring 31.50 mL of the NaOH solution to reach the phenolphthalein end point. Calculate the concentration of the initial malonic acid solution. (Sec Exercise 113.)
A 0.3012g sample of an unknown monoprotic acid requires 24.13mL of 0.0944MNaOH for neutralization to a phenolphthalein end point. There are 0.32mL of 0.0997MHCl used for back titration. a. How many moles of OH are used? How many moles of H+ from HCl? _______moles OH ________moles H+ b. How many moles of H+ are there in the solid acid? Use Eq.5. ____________ moles H+ in solid c. What is the molar mass of the unknown acid? Use Eq.4. ____________ g/mol
The Merck Index indicates that 10 mg of guanidine,CH5N3, may be administered for each kilogram of bodymass in the treatment of myasthenia gravis. The nitrogenin a 4-tablet sample that had a total mass of 7.50 g wasconverted to ammonia by a Kjeldahl digestion, followedby distillation into 100.0 mL of 0.1750 M HCl. Theanalysis was completed by titrating the excess acid with11.37 mL of 0.1080 M NaOH. How many of thesetablets represent a proper dose for a patient who weighs(a) 100 lb, (b) 150 lb, and (c) 275 lb?
UEid- base tit ration the Consentrat ion of ammonia Solution excess HCL was titrated ith o.07om Na, cO3 Solutian. The volume of Na, Coz Solution reguired was 15.50 ml using the following eguations: 2HCLem> + Na, COgcaps CO2 Cays + HzO1) t NaCL Calculate the concentration (molarity and ppm) of ammonia in the Original Solution.(MM of NHzis 17.031.9/4) 10.0 was by of o.10OMI HCE to Then
3. A 2.0g sample of juice from a fresh lime was diluted with water and filtered to remove the suspended matter. The clear liquid required 40.39mL of 0.04022M NaOH for titration to the phenolphthalein end point. Calculate the % acidity as % citric acid. Equation: H3C6H5O7 + 3NaOH Na3C6H5O7+ 3HOH
A 2.1562 g sample that may contain NaOH, NaHCO3 and Na2CO3 alone or in compatible mixtures reqıires 31.2 ml of 0.1082 M HCl for titration to the phenolphthalein end point and additional 52.4 ml of the same acid to bromocresol green end point. Calculate the percentages of compound(s) in the sample (M. Mass of NaOH:40 g/mol, M. Mass of NaHCO3: 84.01 g/mol, M. Mass of Na2CO3: 105.99 g/mol)?
3. Complete neutralization of 10 ml of phosphoric acid solution by NaOH 0.I N in the presence of phenol phthalein until the appearance of purple color (pH, = 9) 11 ml. of NaOH is consumed. (a) What is the concentration of phosphoric acid? (b) Calculate the indicator error. pk2.1 pK. - 7.2 pK - 124
5. A 300.0 mg sample containing Na,CO3, NaHCO3 and NaOH and inert material either alone or in some combination was dissolved and titrated with 0.1000 M HCI the titration required 24.41 mL to reach the phenolphthalein endpoint. And an additional 8.67 mL to reach the methyl red endpoint. Determine the composition of the sample and calculate the percent of each titrated component.
Na2CO3 + HCl -> NaCl + NaHCO3 Na2CO3 served as the primary standard in a titration experiment. Find the molarity of the titrant given the following data in 3 decimal places. Show solutions Primary Standard Used: Na2CO3Formula Mass of 1º standard: 105.99 g/mol% purity of 1º standard: 95% Trial 1 2 3 1º Standard weight, g 0.1005 0.1001 0.0997 Net volume of HCl, mL 9.30 9.00 8.90 Molarity of HCl X1 X2 X3
The following titration curve shows the titration of triethylamine (C,H5)3N with hydrochloric acid. Which net ionic reaction explains the pH of the analyte solution before any titrant is added? 12 10 6. PH 4. 1. 10 50 mL of HCI 30 70 90 110 (CH;)3NH"(aq) + H,0(1) (C,Hg)gN(aq) + H3O*(aq) O C,H;)3N(aq) + H3O*(aq) (CH5)3NH*(aq) +OH (aq) (C2H5)3N(aq) + H*(aq) -> (C,H5)3NH"(aq) O H2O(1) H*(aq) + OH (aq) --> (C2H;)3N(aq) + H,0(1) OH (aq) + (CH5)3NH*(aq)
Consider the titration of 100.0 mL of 0.100 M hydrazine (H2NNH2, K, = 3.0×10-6) by 0.200 M HNO3. Despite the symmetric nature of the hydrazine's molecular structure, it accepts only a single proton from HNO3 in aqueous solution. (Kw = 1.00×10-14) %3D %3D (a) Calculate the pH of the solution after addition of 0.0, 20.0, 25.0, 40.0, 50.0, and 100.0 mL of HNO3 to the solution. (Note: you need to consider the range of applicability of the Henderson- Hasselbalch equation and need to check if water autoionization can be neglected. See Figure 15.18 in the textbook.) (b) Based on your answer to part (a), sketch the titration curve, marking the calculated points and labeling the equivalence and half-equivalence points. (c) Although still weak, ammonia (NH3, Kb = 1.8×10-5) is a stronger base than hydrazine. Sketch the titration curve for 100.0 mL of 0.100 M ammonia by 0.200 M HNO3 on the same axes as your answer to part (b); be sure to label the curve. %3D Note: a qualitative sketch is…
Consider the following infermation about sulfurous acid, a diprotic acid (11,S0,L LSO3=HSO, +1I* pK=1.81 HSO, S0,+H pK2-691 The titration curve for sodism sulfite, Na SO, with standard HCl is shown below PH VI V2 ml, HO added What are the major species present al point 3? O No