ions in a solution can be found by reaction with an excess of aqueous iodide ions to produce iodine. The amount of iodine formed can be found by titration with thiosulfate ions‚ S2O32–. For Examiner’s Use FB 1 is aqueous copper(II) sulfate‚ CuSO4. FB 2 is 0.100 mol dm–3 sodium thiosulfate‚ Na2S2O3. FB 3 is aqueous potassium iodide‚ KI. starch indicator Read through the instructions carefully before starting any practical work.
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like small flakes of silver Turned bright red and obviously to a very high temp. Turned bright red and gave off gas Zn Much bigger and sturdier than magnesium‚ although very similar in look (besides size). Completely melted and then solidified into a new form. Continued to melt CuCO3 Green powder Turned dark black instantly as if it was completely burning Again turned dark black Cu(NO3)2 Looked like aqua and navy blue glitter mixed together Fizzled and looked like it was turning into a gaseous solution
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Balancing Equations Balancing equations is a fundamental skill in Chemistry. Solving a system of linear equations is a fundamental skill in Algebra. Remarkably‚ these two field specialties are intrinsically and inherently linked. 2 + O2 ----> H2OA. This is not a difficult task and can easily be accomplished using some basic problem solving skills. In fact‚ what follows is a chemistry text’s explanation of the situation: Taken from: Chemistry Wilberham‚ Staley‚ Simpson‚ Matta Addison Wesley
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ELECTROPLATING Electroplating is the application of electrolytic cells in which a thin layer of metal is deposited onto an electrically conductive surface. Electroplating is a plating process that uses electrical current to reduce cat ions of a desired material from a solution and coat a conductive object with a thin layer of the material‚ such as a metal. Electroplating is primarily used for depositing a layer of material to bestow a desired property (e.g.‚ abrasion and wear resistance‚ corrosion
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anode and cathode half-reactions‚ and the net cell reaction for the above diagram. [ T/I / 2 ] Oxidation: Zn (s) Zn2+ (aq) + 2e- Reduction: Cu2+ (aq) +2e- Cu(s) Zn (s) + Cu2+ (aq) +2e- Zn2+ (aq) + 2e- + Cu(s) Zn (s) + Cu2+ (aq) Zn2+ (aq) + Cu(s) c) Write the cell notation for the above galvanic cell drawn. [ T/I / 1 ] Cu(s) | Cu2+(aq) || Zn 2+(aq) | Zn (s) d) Calculate the percent error of the cell potential for the above galvanic cell. Show all work. [ T/I
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4 _____8. Iron is more active than silver but less active than zinc. Which one of the following reactions will occur? A. Fe + 2Ag+ ( Fe+2 + 2Ag B. Fe + Zn+2(Fe+2 + Zn C. 3Ag + Fe+3( 3Ag+ + Fe D. Zn+2 + 2Ag( Zn + 2Ag+ _____9. Based on the solubility rules‚ which of the following is insoluble? A. CuSO4 B. CuS C. CuCl2
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H +1‚ O −1 e) Ca(ClO)2; Ca +2‚ Cl +2‚ O −2 f) Zn(NH3)6Cl2; Zn 2+‚ N 3−‚ H 1+‚ Cl 1− (Cl is +1 in this compound. Ca: 1 × (+2) = +2. O: 2 × (−2) = −4. Charge on the compound = 0; therefore‚ (+2) + (−4) + 2 × Cl = 0. The charge on Cl is 1+.) 2- A voltaic cell is constructed. One electrode compartment consists of a zinc strip placed in an aqueous solution of Zn(NO3)2‚ and the other has a nickel strip placed in an aqueous solution of NiCl2. E°red(Zn2+/Zn) = −0.76 V E°red(Ni2+/Ni) = −0.28 V Which one of
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Benedict ’s solution contains Cu+2 ions that are blue in colour. This means that when Benedict ’s solution is added to clear transparent or translucent solutions‚ the solutions turn light blue due to the presence of the Cu+2 ions. Out of the 12 solutions‚ solution 10 (beer) was a light brown-yellow colour‚ while the remaining 11 were either transparent or translucent. Thus‚
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TO QUESTIONS: 1. a. in distilled water: Cu(OH)2(s) (( Cu2+(aq) + 2OH-(aq) Ksp Cu(OH)2 Keq = Ksp Cu(OH)2 = 2.2 x 10-20 b. + 6.0M H2C2O4 Cu(OH)2(s) (( Cu2+(aq) + 2OH-(aq) Ksp Cu(OH)2 H2C2O4 (( H+ + HC2O4- Ka1 H2C2O4 HC2O4- (( H+ + C2O42- Ka2 H2C2O4 Cu2+ + C2O42- (( CuC2O4 1/Ksp CuC2O4 2(OH- + H+ (( H2O) 1/K2w Net Keq = (Ksp Cu(OH)2 x Ka1 x Ka2 )/Ksp CuC2O4 = 1
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10 M Cu(NO3)2 and into each test tube‚ 1.0 mL of 0.10 M NaOH was added. Using a centrifuge‚ the precipitate was settled and the supernate was discarded. 3.0 mL of distilled water and 10 drops of 0.10 M NaOH were added into each test tube. The test tubes were then prepared according to Table 1. Table 1. The reagents to be added for Cu(OH)2(s) equilibrium Test tube | Reagent to be added | 1 | 2.0 mL distilled water | 2 | 2.0 mL 1.0 M H2C2O4 solution | 3 | 2.0 mL water + pinch of Zn dust
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