Tripoli Campus Chem 200 Lab Report Experiment 6 : Redox titration Course Instructor: Dr Lisa Diab Student Name: Marwa Noaman ID: 51230262 Introduction: To determine a substance analytically‚ oxidation- reduction reactions are used. During any redox reaction transferring of reactions occurs from a reducing agent to an oxidizing agent. Purpose: * To titrate "Mohr’s salt" solution with KMNO4‚(second standard) which has to be standardize with oxalic acid (first
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solution. HCl dissolves insoluble carbonates‚ chromates‚ sulfates‚ ammonia complexes‚ and hydroxides that may be present within a solution. Cations such as Ag+‚ Hg22+‚ and Pb2+ ions will precipitate into insoluble chlorides. A high concentration of HNO3 is essential to lower pH and oxidize sulfide ions present in solution. The importance of NaOH is to precipitate insoluble hydroxide and increase pH. NaOH will form hydroxide complexes. Adjusting pH allows for ions to bind to other ions that will
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Fe3+→e-+Fe2+ E0=0.777 V The loss of an electron‚ oxidation‚ from Fe3+ creates an electric potential of 0.777 volts. A “cell” is created when an electric potential is cyclically moving throughout a system. A half-cell reaction at the anode electrode is similar to the oxidation reaction shown above. (2) Pt/0.1 M Fe3+‚0.01M Fe2+ This oxidation reaction creates different masses of each state of iron where Fe3+ is favored at
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reducing agent ACIDIC CONDITION 1. BrO3- + N2H4 → Br- + N2 2. UO2+ + NO3- → UO22+ + NO(g) 3. S2O42- → S2O32- + HSO3- BASIC CONDITION 1. Ag(s) + CrO42- → Ag+ + Cr(OH)3 (s) 2. ClO2 → ClO3- + Cl- 3. CH3CH2OH + MnO4- → CH3COO- + MnO2 (s) What is the oxidation number of the indicated element in each of the following? a. S in S8 b. Hg in Hg2Cl2 c. Cr in Cr2O72- d. C in H2C2O4 e. Bi in BiO3- f. Cl in Cl2O g. B in B2Br4 h. S in SF6 III. PROBLEM SOLVING Show full calculation and box the final answer. Express
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1a: Review Redox Assign Oxidation Numbers to the following: a. HNO3 b. PbSO4 c. (NH4)2Ce(SO4)3 Balance the following in acidic medium Al (s) + MnO4- (aq) Al3+ (aq) + Mn2+ (aq) Balance the following in a basic medium Mg (s) + OCl- (aq) Mg(OH)2 (s) + Cl- (aq) Balance the following Redox Reaction: The big nasty problem K4Fe(CN)6 + KMnO4 + H2SO4 KHSO4 + Fe2(SO4)3 + MnSO4 + HNO3 + CO2 +H2O 17.1: Galvanic Cells Review of Redox Reactions Oxidation: _______________________
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nitrate‚ NaNO3‚ 0.2 M Test Reagents: Silver nitrate‚ AgNO3‚ 0.1 M Ammonia‚ NH3‚ 6 M Nitric acid‚ HNO3‚ 6 M Potassium permanganate‚ KMnO4‚ 0.1 M Mineral oil Sodium hydroxide‚ NaOH‚ 6 M Barium hydroxide‚ Ba(OH)2‚ saturated Barium chloride‚ BaCl2‚ 0.1 M Acetic acid‚ HC2H3O2‚ 6 M Aluminum(s)‚ granules Iron(III) nitrate‚ Fe(NO3)3 0.1 M in nitric acid‚ HNO3‚ 0.6 M To neutralize spills: Baking soda‚ NaHCO3(s) Vinegar‚ HC2H3O2 Equipment Test tubes
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Oxidation-Reduction Worksheet For each reaction below‚ identify the atom oxidized‚ the atom reduced‚ the oxidizing agent‚ the reducing agent‚ the oxidation half reaction‚ the reduction half reaction‚ and then balance the equation by the method of oxidation-reduction showing all electrons transfers. 1.Mg + HCl ( MgCl2 + H2 2.Fe + V2O3 ( Fe2O3 + VO 3.KMnO4 + KNO2 + H2SO4 ( MnSO4 + H2O + KNO3 + K2SO4 4.K2Cr2O7 + SnCl2 + HCl ( CrCl3 + SnCl4 + KCl + H2O 5.KMnO4 + NaCl + H2SO4 ( Cl2 +
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experiment the following equipment: copper wire‚ hot plate‚ 3M HCl(aq)‚ 6M HNO3(aq)‚ 6M NaOH (aq)‚ 2 M H2SO4‚ 100ml beaker‚ graduated cylinder‚ filter flask‚ Buchner funnel/vacuum flask ‚ scale‚ and pipets alongside the fume hood--for the omission of NO2-- was used to conduct the copper cycle experiment. First‚ the given copper wire (.29g) was cut into minute pieces then placed in a beaker with the aqueous solution of HNO3. The beaker was then placed on the hot plate to present a blue transparent
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end‚ we will return it to it¡¦s normal solid state. Determine the percentage yield (quantitative). Define what happen at level of electron for oxidation/reduction‚ double replacement‚ neutralization and decomposition. There are five reactions that the copper will go through. 1. Cu(s) + 4HNO3(aq) --- Cu(NO3)2(aq) + 2H2O(aq) + NO2(aq) 2. HNO3(aq) + NaOH(aq)--NaNO3(aq) + H20(l) 3. Cu(OH)2(s)--CuO(s) + H2O(l) 4. CuO(s) + H2SO4(aq)-- CuSO4(aq) +H2O(l) 5. CuSO4(aq) + Zn(s)--
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Section 10.10 Balancing Oxidation–Reduction Equations ENERGY General Chemistry 2 (Chem 112) Return to TOC Copyright © Cengage Learning. All rights reserved 1 Section 10.10 Balancing Oxidation–Reduction Equations UNIT 1: ENERGY MODULE 1: ELECTROCHEMICAL ENERGY MODULE 2: NUCLEAR ENERGY MODULE 3: FUELS Return to TOC Copyright © Cengage Learning. All rights reserved 2 Section 10.9 Oxidation–Reduction Reactions Redox Reactions • Reactions in which one
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