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- (c)Ions that react with Ag+ like SCN- can be determined electrogravimetricallyby deposition on a silver working anode:Ag(s) + SCN- ≤ AgSCN(s) + eA silver anode with initial mass of 12.4730 g was used to electrolyse 85.00 mL of asolution of 0.0245 M KSCN. At the end of the experiment, the anode weighed12.5767 g. How long did the experiment take, if a current of 100 mA was used?Which of the oxidizing agent listed is (are) capable of oxidizing Br - (aq) to BrO 3 - (aq) in acidicsolutions). Please answer with explanations. Thanks(a) A Cr3+(aq) solution is electrolyzed, using a current of7.60 A. What mass of Cr(s) is plated out after 2.00 days?(b) What amperage is required to plate out 0.250 mol Crfrom a Cr3+ solution in a period of 8.00 h?
- In the redox analyysis of iron, there are peices of tin metal on the botom of the SnCl2 reagen solution. Why is it there?Halide ions can he deposited at a silver anode, the reaction being Ag(s) + X- AgX(s) +e- Suppose that a cell was formed by immersing a silver anode in an analyte solution that was 0.0250 M Cl-,Br-, and I -ions and connecting the half-cell to a saturated calomel cathode via a salt bridge. (a) Which halide would form first and at what potential? Is the cell galvanic or electrolytic? (b) Could I- and Br- be separated quantitatively? (Take 1.00 l0-5 M as the criterion for quantitative removal of an ion.) If a separation is feasible, what range of cell potential could he used? (c) Repeat part (b) for I- and Cl-. (d) Repeat part (b) for Br- and Cl-.Explain 3 applications of electrochemistry in common industrial processes and describe them in brief. And Also the corrosion of metals in terms of an electrochemical process, and describe some common corrosion-inhibiting techniques?
- Many applications of electrochemistry have been in chemical analysis.Suppose a Fe|Fe2+ concentration cell is set-up in which the [Fe2+] = 1.0 x10¯2 M in one compartment but the concentration in the othercompartment is unknown. The Ecell was measured at 0.024V when thehalf-cells were connected.(i) Without doing a numerical calculation, is the unknown more orless concentrated than the 1.0 x 10¯2 M solution? Justify youranswerWhich of the following aboutsacrificial anodes is wrong? a)Generally, low percentage alloys are preferred instead of pure metal as the galvanic anode. b)Noble metals in the anode composition have a passivating effect on the anode. c)Magnesium anodes,especially high potential magnesium anodes,are preferred for high resistance grounds andfresh waters. d)Aluminum anodes cannotbe used in pure form, as they passivateeasily. e)The current strength drawnfrom the sacrificial anode is independent of the anode resistance and the potentialdifference between the anode-cathode.The electrochemical cell: SCE||H+(a=x)|glass electrodehas a potential of 0.2094 V when the solution in the right-hand compartment is abuffer of pH 4.006. The potential reading for an unknown solution measured by thesame glass electrode was –0.3011 V. Calculate the pH and the hydrogen ion activityof the unknown solution. Assume a Nernstian response for the glass electrode.
- The standard reduction potential of the permanganate ion, MnO4-, to Mn2+ is 1.51 volt, when it takes place in an acidic aqueous solution. The normal reduction potentials of ions Zn2+, Ag+ and Au+ are, respectively, 0.7618, 0.7992 and 1.692 V (in aqueous solution).Introducing a Pt electrode in a MnO4-/ Mn2+ solution, with a salt bridge, and putting it together with the other electrodes (Zn, Au or Ag) and their aqueous solutions,a) Comment in which case will the permanganate oxide the metalsb) Justify your answerc) In those cases where the oxidation takes place, write the diagram of the celld) Calculate the standard potential of the cells, Eºcell. Result: a) Eºcell >0 d) 0.7108 V, 0.7482 VA 1 M solution of Cu(NO3)2 is placed in a beaker with astrip of Cu metal. A 1 M solution of SnSO4 is placed in asecond beaker with a strip of Sn metal. A salt bridge connectsthe two beakers, and wires to a voltmeter link the twometal electrodes. (a) Which electrode serves as the anode,and which as the cathode? (b) Which electrode gainsmass, and which loses mass as the cell reaction proceeds?(c) Write the equation for the overall cell reaction. (d) Whatis the emf generated by the cell under standard conditions?A salt of each of the ions in Table is dissolvedin water. A Pt electrode is immersed in each solution and con-nected to a 0.38-V battery. All of the electrolytic cells are run forthe same amount of time with the same current.(a) In which cell(s) will a metal plate out? Explain.(b) Which cell will plate out the least mass of metal? Explain.