1. A 125 mL sample of orange juice was titrated using a redox reaction to the equivalence point with the addition of 7.6 mL of a 0.0025M iodine (I) solution. What is the concentration of vitamin C (CHO) in this sample? (Note that 1,000 mM = 1 M) a. 30 mM b. 15 mM c. 19 mM CHO (aq) + (aq) → CHO (aq) + 21 (aq) + 2H(aq) d. 0.30 mM e. 0.15 mM

1. A 125 mL sample of orange juice was titrated using a redox reaction to the equivalence point with the addition of 7.6 mL of a 0.0025M iodine (I) solution. What is the concentration of vitamin C (CHO) in this sample? (Note that 1,000 mM = 1 M) a. 30 mM b. 15 mM c. 19 mM CHO (aq) + (aq) → CHO (aq) + 21 (aq) + 2H(aq) d. 0.30 mM e. 0.15 mM

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

See similar textbooks

Similar questions

5. A student conducted a titration experiment. He/she used 12.0 mL of silver nitrate (titrant) solution to reach the endpoint. If the student used 25.4 mL of the chloride (analyte) for the titration and found the concentration of chloride ions to be 2.2 M, what is the mass (in grams) of silver nitrate titrant Clic)
Jack determines the concentration of NaOH by titrating it with 4.0 g KHP (a monoprotic acid). It takes 21.2 mL of NaOH to reach the equivalence point. What is the concentration of the NaOH? molar mass of KHP 204.2 g/mol [NaOH] = [?] M [NaOH], M Enter
Solution X containing 0.020 mol of iron(II) sulfate requires 22.5 mL of potassium manganate(VII) for a complete reaction. The equation for the reaction is: 5Fe^2+ + MnO4^- + 8H^+ → Mn^2+ + 4H2O + 5Fe^3+. What is the molarity of the KMnO4 solution?
In the following reaction, which species is the reducing agent? ClO3 ^-(aq) + 6 I^- (aq) + 6 H^+(aq) > Cl^- (aq) + 3 I2(s) + 3 H2O (aq) A. ClO3 B. H2O C. H+ D. I-
8888
Consider the neutralization reaction 2 HNO3(aq) + Ba(OH)2(aq). 2 H2O(l) + Ba(NO3)2(aq) A 0.105 L sample of an unknown HNO3 solution required 42.5 mL of 0.250 M Ba(OH)2 for complete neutralization. Wha the concentration of the HNO3 solution? concentration: .098
4. When a solutions of aluminum sulfate and potassium hydroxide are mixed, a precipitate forms. a. Write a balanced net ionic equation for the reaction. b. Calculate the mass of the precipitate when 3.89 g of aluminum sulfate in 100mL of solution is combined with 50 mL of the o.300 M KOH. c. What is the molarity of the ion in excess? (Ignore the spectator ions and assume that volumes are additive)
By the half-reaction method the balanced equation of the following redox reaction is Fe+3 Fe(s) + Mg (aq) +2 (aq)+ Mg(s) O a. Fe*3(aq)+ 3 e -Fe(s) O b. Fe*3(aq)+ Mg(s) - Fe(s) + Mg*2 (aq) Oc 3 Fe*3(aq)+ 2Mg(s) - 3Fe(s) + 2Mg*2 (aq) O d. 2Fe*3 (ag) + 3Mg - 2FEG) + 3Mg*2 (aq) page ourse Syllabus Jump to
1. What is the concentration of a 1.0 M solution of K+(aq) ions in equivalents/liter? 2. A solution having initial concentration of 0.445 M and initial volume of 45.0 mL is diluted to 100.0 mL. What is its final concentration?
According to the following (balanced) reaction, what volume of 0.244 mol/L KCI solution is required to react exactly with 50.0 mL of 0.210 mol/L Pb(NO3)2 solution? 2 KCI (aq) + Pb(NO3)2 (aq) → PbCl 2 (s) + 2 KNO3 (aq) A. 43.0 mL B. 116 mL c. 58.1 mL D. 86.1 mL E. 97.4 mL
2. Specify which of the following are oxidation-reduction reactions and identify the substance being oxidized and the substance being reduced, when appropriate. a. Cu (s) + 2 Ag (aq) + 2 Ag (s) + Cu²+ (aq) b. HCl (g) + NH, (g) → NH,Cl (s) c. SiCl, (l) + 2 H₂O (1)→ 4 HCl (aq) + SiO₂ (s) d. SiCl, (l) +2 Mg (s) 2 MgCl, (s) + Si (s) e. Al(OH), (aq) → AlO, (aq) + 2 H₂O (1) f. CH, (g) +H,O (g) + CO (g) + 3H, (g) g. Zn (s) + 2 HCl (aq) → ZnCl, (aq) + H₂(g) h. 2H* (aq) + 2 CrO, (aq) + Cr₂O," + H₂O (1)
Part 3: What mass of tin was used to make the tin solution? In a similar experiment, a sample of tin metal was dissolved in nitric acid to produce 28.00 mL of solution containing Sn²+. Titration analysis resulted in the calculation that the concentration of Sn²+ in this solution was 0.65 mol/L. b. What mass of tin was used to make the tin solution? Find the mass of the Sn(s) in g: (give your answer to 2 decimal places) Your Answer: Answer