Results & Discussion:Part 1: Oxidation-Reduction ReactionsNo. ReactionObservationGas evolved (H2)No reactionBrown gas evolved solution turned blue1 Zn piece +2 mL HCI (2M)2 Cu wire + 2 mL HCI (2M)3 Cu wire + 1 mL HNO3 (6M) // in FUME HOOD4 1 mL NazC204 + 10 drops H;SO4 + 10 drops KMnO. Reduced to Mn2+ purple colorchanges to colorless1. When a small piece of zinc added to HCI, hydrogengas was produced, and thezinc wastoZn (s) + HCI (aq) →2. When a copper wire added to HCI No reactionobserved, because copperconsidered asInactivemetal.3. Then, in fume hood 6 M HNO3 was added to a piece of copper wire.gas was formed, And the color of the solution becamewhich indicates thepresence ofion, thus,Cu wasto Cu2. The reaction was done inthe fume hood because NO2 gas isCu (s) + HNO3 (aq) →4. When sodium oxalate was reacted with KMNO4, the color of the solution was changedfromtodue to theof MnOa toKMNO4 act as a strongagent in acidic media, sowas addedto the test tube to provide anmedia for the reaction.Balanced equation in acidic media : 2 MnO, + 16 H* + 5 C20. → THIS EQUATION NOT REQUIRED

When a small piece of zinc added to HCl Hydrogen gas was produced, and the zinc was oxidized to…

-> er wire added to HCI No reaction observed Inactive metal. hood 6 M HNO3 was added to a piece of copper wire. ed, And the color of the solution became. ion, thus,Cu was to Cu*. The re d because NO2 gas is aq) → oxalate was reacted with KMNO4, the color of the solt to due to the rong. agent in acidic media, so provide an media for the reaction. n in acidic media : 2 MnO, + 16 H* + 5 C20, → TH

-> er wire added to HCI No reaction observed Inactive metal. hood 6 M HNO3 was added to a piece of copper wire. ed, And the color of the solution became. ion, thus,Cu was to Cu. The re d because NO2 gas is aq) → oxalate was reacted with KMNO4, the color of the solt to due to the rong. agent in acidic media, so provide an media for the reaction. n in acidic media : 2 MnO, + 16 H + 5 C20, → TH

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...

See similar textbooks

Similar questions

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?
In theory, most metals should easily corrode in air. Why? A group of metals called the noble metals are relatively difficult to corrode in air. Some noble metals include gold, platinum, and silver. Reference Table 17-1 to come up with a possible reason why the noble metals are relatively difficult to corrode.
A solution contains both iron(II) and iron(III) ions. A sample Of the solution is titrated with 35.0 ml, of M KMnO4, which oxidizes Fe2+ to Fe3+. The permanganate ion is reduced to manganese(ll) ion. The equation for this reaction is MnO4(aq)+8 H+(aq)+5Fe2+(aq)Mn2+(aq)+5Fe3+ +4H2OAnother 50.00-mL sample of the solution is treated with zinc, which reduces all the Fe3+ to Fe2+. The equation for this reaction is 2Fe3+(aq)+Zn(s)2Fe2+(aq)+Zn2+(aq)The resulting solution is again titrated with 0.0280 M KMnO4; this time 48.0 ml, is required. What are the concentrations of Fe2+ and Fe3+ in the solution?
Specify which of the following equations represent oxidation reduction reactions, and indicate the oxidizing agent, the reducing agent, the species being oxidized, and the species being reduced. a. CH4(g)+H2O(g)CO(g)+3H2(g) b. 2AgNO3(aq)+Cu(s)Cu(NO3)2(aq)+2Ag(s) c. Zn(s)+2HCl(aq)ZnCl2(aq)+H2(g) d. 2H+(aq)+2CrO42-(aq)Cr2O72-(aq)+H2O(l)
Which of the following must be an oxidation—reduction reaction? Explain your answer, and include an example oxidation—reduction reaction for all that apply. l type='a'> A metal reacts with a nonmetal. i>A precipitation reaction. i>An acid—base reaction.
When jump-starting a car with a dead battery, the ground jumper should be attached to a remote part of the engine block. Why?
A sample of solid calcium hydroxide, Ca(OH)2, is allowed to stand in water until a saturated solution is formed. A titration of 75.00 mL of this solution with 5.00102M HCl requires 36.6 mL of the acid to reach the end point. Ca(OH)2(aq)+2HCl(aq)CaCl2(aq)+2H2O(l) What is the molarity?
The Ostwald process for the commercial production of nitric acid involves the following three steps: 4NH3(g)+5O2(g)4NO(g)+6H2O(g) 2NO(g)+O2(g)2NO2(g) 3NO2(g)+H2O(l)2HNO3,(aq)+NO(g) a. Which reactions in the Ostwald process are oxidationreduction reactions? b. Identify each oxidizing agent and reducing agent.
Balance each of the following equations, and classify them as precipitation, acid-base, gas-forming, or oxidation-reduction reactions. Show states for reactants and products (s, , g, aq). (a) CuCl2 + H2S CuS + HCl (b) H3PO4 + KOH H2O + K3PO4 (c) Ca +HBr H2 + CaBr2 (d) MgC12 + NaOH Mg(OH)2 + NaCl