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- The measurement of pH using a glass electrode obeys the Nernst equation. The typical response of a pH meter at 25 00C is given by the equation where contains the potential of the reference electrode and all other potentials that arise in the cell that are not related to the hydrogen ion concentration. Assume that = 0.250 V and that a. What is the uncertainty in the values of pH and [H+] if the uncertainty in the measured potential is 1 m V ( 0.001 V)? b. To what precision must the potential be measured for the uncertainty in pH to be 0.02 pH unit?In some old European churches, the stained-glass windowshave so darkened from corrosion and age that hardly anylight comes through. Microprobe analysis showed that tinycracks anddefects on the glass surface were enriched ininsoluble Mn(III) and Mn(IV) compounds. From AppendixE, suggest a reducing agent and conditions that might successfullyconvert thesecompounds to soluble Mn(II) withoutsimultaneously reducing Fe(III) (which gives the glassits colors) to Fe(II). Take MnO2 as representative of theinsoluble Mn(III) and Mn(IV) compounds.The formation constant for the mercury(II) acetate complex is Hg2++ 2OAc- Hg(OAc)2(aq) Kf = 2.7 108 Calculate the standard potential for the half-reaction Hg(OAc)2(aq) + 2e- Hg(l) + 2OAc-
- Consider a cell in which the reaction is 2Ag(s)+Cu2+(aq)2Ag+(aq)+Cu(s) (a) Calculate E° for this cell. (b) Chloride ions are added to the Ag|Ag+ half-cell to precipitate AgCl. The measured voltage is +0.060 V. Taking [Cu2+]=1.0M, calculate [Ag+]. (c) Taking [Cl-] in (b) to be 0.10 M, calculate Kspof AgCl.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-.Why is it not possible for hydroxide ion (OH-) to appear in either of the half-reactions or the overall equation when balancing oxidation—reduction reactions in acidic solution?
- A precipitate of AgCl + AgBr weighs 0.8132 g. On heating on a current of Cl2, the AgBr is converted to AgCl, the mixture loses 0.1450 g in wt. Find the percentage Cl in the original sample.1. , A standard 0.0100 M solution of Na is required to calibrate an ion-selective electrode method to determine sodium. Describe how 500 mL of this solution can be prepared from primary standard Na:CO: (105.99 g/mol).Balance the following in acidic medium: MnO4- + Fe2+ ---> Mn2+ + Fe3+ How many Fe2+ are there in the balanced equation?
- Which of the statements below are true for the titration of Fe2t with standard Ce? I. The indicator electrode potential before the addition of Cet solution is calculated using the Fea+ half-reaction after calculating the equilibrium concentrations of Fe3+ and Fe2+ in solution. II. Before the equivalence point, the indicator electrode potential is calculated using the Fe3+ half-reaction because only [Fe3] and [Fe2*] are known. III. At the equivalence point, the indicator potential is the average of E" for Fet and Cet. IV. After the equivalence point, the indicator electrode potential is calculated using the Ce** half-reaction because only [Ce"] and [Ce2*] are known. 1, II, II, and IV I, II, and IV II, III, and IV 1, I1. and IVA 60.0 mL solution of 0.00750 M OsCl,3- in 1 M HCI was titrated with 0.0300 M IrCI,2- to give OsCl,2- and IrClg3-. a) What is the reducing agent in this reaction? Write "a" for the titrant or "b" for the analyte. b) From the standard potentials table, what is the standard potential of the Os half-reaction? E°, = V c) What is the standard potential of the Ir half-reaction? E°, = V d) At what volume of analyte is the equivalence point? Ve = mL e) Calculate the potential (vs. Ag | AGCI) when 10.8 mL of titrant is added. E = V f) Calculate the potential (vs. Ag | AgCI) at the equivalence point. E = g) Calculate the potential (vs. Ag | AGCI) when 17.6 mL of titrant is added. E = v h) At what volume of analyte will the potential be equal to the standard potential of the Ir half-reaction (ignoring the Ag | AgCl electrode)? V = mLA 60.0 mL solution of 0.00750M OSCI63- in 1 M HCI was titrated with 0.0300 M IrCl,2- to give OsCl,2- and IrCl,3-. a) What is the reducing agent in this reaction? Write "a" for the titrant or "b" for the analyte. b) From the standard potentials table, what is the standard potential of the Os half-reaction? E°+ = c) What is the standard potential of the Ir half-reaction? E°+ = V d) At what volume of analyte is the equivalence point? Ve = mL e) Calculate the potential (vs. Ag | AgCl) when 10.8 mL of titrant is added. E = V f) Calculate the potential (vs. Ag | AgCI) at the equivalence point. E = V g) Calculate the potential (vs. Ag | AgCI) when 17.6 mL of titrant is added. E = h) At what volume of analyte will the potential be equal to the standard potential of the Ir half-reaction (ignoring the Ag | AgCl electrode)? V = mL