a) The selectivity coefficient for a Bromide ion-selective electrode is K Br,OH 0.15. What will the change in the electrode potential be for a 1.4 x 10 M Br¯ at pH 5.5 if the pH is raised to pH 11.0? b) A pH probe is calibrated against pH 4 and pH 7 buffers. For pH 4 buffer, E = 200 mV and for pH 7 buffer, E = 23 mV. If the potential for an unknown solution is 157 mV, calculate the pH of the solution. Shew yo wk

a) The selectivity coefficient for a Bromide ion-selective electrode is K Br,OH 0.15. What will the change in the electrode potential be for a 1.4 x 10 M Br¯ at pH 5.5 if the pH is raised to pH 11.0? b) A pH probe is calibrated against pH 4 and pH 7 buffers. For pH 4 buffer, E = 200 mV and for pH 7 buffer, E = 23 mV. If the potential for an unknown solution is 157 mV, calculate the pH of the solution. Shew yo wk

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

See similar textbooks

Similar questions

If the half-cell Li(s)|Li+(aq)(1.0 M) is coupled to SHE, the Li(s) electrode will lose mass during the operation of the cell. (Note: E°red Li+/Li = –3.05 V). true or false
3. Calculate the voltage of a cell composed of Ni2+ | Ni and Cu2+ | Cu electrodes at 298 K, if ANI* = 0.85 and acu+ = 0.22.
12- An electrochemical cell is composed of pure copper and pure cadmium electrodes immersed in solutions of their respective divalent ions. For a 6.5 × 102 M concentration of Cd²+, the cadmium electrode is oxidized, yielding a cell potential of 0.775 V. Calculate the concentration 2+ of Cu ions if the temperature is 25°C. Electrode Reaction Au³+ + 3e - Au O₂ + 4H+ 4e¯ Pt2+ + 2e Ag+ e Fe³+ + e O₂ + 2H₂O + 4e4(OH™) Cu H₂ Pb Cu²+ + 2e → 2H₂O Pt Ag Fe²+ 2H + 2e Pb²+ + 2e - Sn²+ + 2e -> Sn Ni²+ + 2e →→→ Ni Co²+ + 2e Co Cd²+ + 2e Cd Standard Electrode Potential, V° (V) +1.420 +1.229 ~+1.2 +0.800 +0.771 +0.401 +0.340 0.000 -0.126 -0.136 -0.250 -0.277 -0.403
A gallium electrode and a Ag/AgCl reference electrode (+0.197 V vs SHE) are immersed in a solution containing Ga*. The cell voltage is -0.766 V. Calculate the molar concentration of Ga3+. 3. Ag/AgCl ref. || Ga³+ | Ga(s) Ga+ + 3e Ga(s) E° = -0.560 V
When an ion-selective electrode for X* was immersed in 0.0362 M XCI, the measured potential was 0.0240 V. What is the concentration of X+ when the potential is 0.0390 V? Assume that the electrode follows the Nernst equation, the temperature is at 25 °C, and that the activity coefficient of X* is 1. [x+] = M
Calculate the cell potential when 150.00 mL of 0.100 M Ag+ solution is titrated with 25.00 mL of 0.150 M Cl- solution. Silver wire indicator electrode and Ag-AgCl electrode are used as reference electrodes. E0 (Ag/AgCl) = 0,197 V , E0 Ag+/Ag = 0,799 V, Ksp (AgCl) = 1,8 x10-8
A solution prepared by mixing 60.0 mL of 0.360 M AGNO, and 60.0 mL of 0.360 M TINO, was titrated with 0.720 M NaBr in a cell containing a silver indicator electrode and a reference electrode with a constant potential of 0.175 V. The reference electrode is attached to the positive terminal of the potentiometer, and the silver electrode is attached to the negative terminal. The solubility constant of TIBr is Kp = 3.6 × 10-6 and the solubility constant of AgBr is = 5.0 x 10-13. Ksp Which precipitate forms first? O TIBI O AgBr Which of the expressions shows how the cell potential, E, depends on [Ag*]? E = 0.175 V – [0.799 V – 0.05916log ([Ag+])] 1 E = |0.799 V – 0.05916log - 0.175 V [Ag*) E = [0.799 V – 0.05916log ([Ag*]D] – 0.175 V E = 0.175 V - |0.799 V – 0.05916log [Ag* * (ল) Calculate the first and second equivalence points of the titration. first equivalence point: mL second equivalence point: mL What is the cell potential after each of the given volumes of 0.720 M NaBr have been…
Find the potentials of the following electrochemical cell:Cd | Cd2+, M = 0.10 ‖ Ni2+, M = 0.50 | Ni
When an ion-selective electrode for X+ was immersed in 0.0362 M XC1, the measured potential was 0.0240 V. What is the concentration of X+ when the potential is 0.0390 V ? Assume that the electrode follows the Nernst equation, the temperature is at 25 °C, and that the activity coefficient of X+ is 1. [x+] = M
Consider the titration of 60.00 mL of 0.100 M Co3+ with 0.130 M MnO²- . What is the potential after 30.00 mL of 0.130 M MnO²- has been added in units of Volts? The potential is measured against the Ag|AgCl reference electrode (E(saturated KCI) = 0.197 V). Co 3+ + e =Co 2+ E°= 1.92 V MnO¯ + e ¯ = MNO2- E°= 0.56 V
The selectivity coefficient, Kg-r, for a K ion-selective electrode is 0.00348. When the electrode is placed into a 8.69 x 10-5 M K* solution at pH 6.77, the potential is -0.150 V vs. SCE. If the pH of the solution is lowered to 1.34 and the ionic strength is kept constant, what is the potential of the electrode? Assume 8 = 1 for the electrode. E = V vs. SCE
50.0 mL of 0.100 M Co3+ solution is titrated with 35.00 mL of 0.130 M MnO42- solution. The potential is measured against the Ag-AgCl reference electrode. Find the measured cell potential. E0 (Ag/AgCl) = 0,197 V Co3+ + e- ↔ Co2+ E0 = 1,92 V MnO4- + e- ↔ MnO42- E0 = 0,56 V