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- 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-.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?true or false 9 __ The equilibrium constant of a redox reaction can be calculated from the standard reduction potentials of involved redox couples at given temperature. __ The charge balance for mixture 0.5 M K2HPO4 + 0.1 M H3PO4 is : [ H +] = [ H2PO4 -] + [ HPO4 2-] + [ PO4 3-] + [ OH-] __ The reduction reaction always occurs at a cathode. __ In EDTA titration, the media pH can impact the conditional formation constant Kf ’ . __ Adding table salt into a sugar solution will result in the increasing activity of coefficient of sugar molecules.
- Which of the statements below are true for the titration of Fe2+ with standard Ce4+?I The indicator electrode potential before the addition of Ce4+ solution is calculated using the Fe3+ 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 Eo for Fe3+ and Ce4+.IV After the equivalence point, the indicator electrode potential is calculated using the Ce4+ half-reaction because only [Ce4+] and [Ce2+] are known. A. I, III, and IV B. I, II, and IV C. II and IV D. II, III, and IV E. I, II, III, and IVA 50.00 mL of 0.100 M Fe(II) is to be analyzed by redox titration with suitable reagents For the redox titration of 50.00 mL of 0.100 M Fe(II) with 0.100 M Ce(IV) in1 M H2SO4, (i) What is the reaction involved? (ii) Explain how the potential at the equivalence point can be determined.Calculate the potential at the equivalence point as measured by a platinumindicator electrode against a standard hydrogen electrode.A pH meter is calibrated using a pH 4.00 buffer with 174.48 mV, pH 7.00 with 0 mV and pH 10.0 buffer with (-)174.48 mV. Calculate the Molar concentration of a HCl solution with electrode potential of 396.31 mV.
- The F- concentration of a solution was determined by measurements with a liquid-membrane electrode. The electrode system developed a potential of 0.5021 V when immersed in 25.00 mL of the sample, and 0.4213 V after the addition of 2.00 mL of 5.45x10^-2 M NaF. Calculate pF for the sample.Can someone please explain the concept of this thank youWhy do both Reference and Indicator electrodes need in Potentiometric titration? answer at your own words ans answer to the point not any irrelevant wordsA 30.0 mL solution of 0.0180 M Rh3+ in 1 M HClO4 was titrated with 0.0900 M Ce4+ to give Rh6+ and Ce3+. Calculate the potential (vs. Ag | AgCl) at the equivalence point. At what volume of titrant will the potential be equal to the standard potential of the Ce half-reaction (ignoring the Ag | AgCl electrode)?
- Black-and-white photographic film is coated with silver halides. Because silver is expensive, the manufacturer monitors the Ag⁺ content of the waste stream, [Ag⁺]ᵥᵥₐₛₜₑ, from the plantwith an Ag-selective electrode at 25°C. A stream of known Ag⁺ concentration, [Ag⁺](standard), is passed over the electrode inturn with the waste stream and the data recorded by a computer.(a) Write the equations relating the nonstandard cell potential tothe standard cell potential and [Ag⁺] for each solution.(b) Combine these into a single equation to find [Ag⁺]ᵥᵥₐₛₜₑ.(c) Rewrite the equation from part (b) to find [Ag⁺]ᵥᵥₐₛₜₑ in ng/L.(d) If Eᵥᵥₐₛₜₑ is 0.003 V higher than E(standard), and the standard so-lution contains 1000. ng/L, what is [Ag⁺]ᵥᵥₐₛₜₑ?(e) Rewrite the equation in part (b) to find [Ag⁺]ᵥᵥₐₛₜₑ for a sys-tem in which T changes and Tᵥᵥₐₛₜₑ and T(standard) may be different.1. A pH electrode obeys the equation E= constant - 0.0592 pH. If the electrode potiential (E) is -0.105 V at 0.002500 M [H+], what is the electrode constant? 2. Using the electrode constant calculated abobe, determine the pH of a solution that gives the electrode potiential of -0.450V. Sketch the calibration plot for the pH electrode. Label the axes, electrode constant and the value of the slope on the calibration plot. Answer question 1A redox titration is performed to investigate iron content in an alloy sample. The potential of titration is monitored against a standard hydrogen electrode at 25 °C. All materials needed for redox titration were prepared accordingly. The half reactions involved in his experiment are:Fe3+ + e ̄ → Fe2+ E° = 0.771 V I3 ̄ + 2e ̄ → 3I ̄ E° = 0.535 Va) Construct a balanced titration equation.b) Assess the E° for this redox reaction.c) Depict whether the name of pH indicator that could be used to determine the endpoint of thistitration.d) Given a 25 mL portion of 0.5 M Fe3+ was titrated with 1 M titrant. Calculate the volumeof titrant required to reach equivalence point.e) Evaluate the cell potential at this point if over-titrated by 2.50 mL.