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- 14-6. A cell was prepared by dipping a Cu wire and a saturated calomel electrode into 0.10 M CUSO4 solution. The Cu wire was attached to the positive terminal of a potentiometer and the calomel electrode was attached to the negative terminal. (a) Write a half-reaction for the Cu electrode. (b) Write the Nernst equation for the Cu electrode. (c) Calculate the cell voltage.Calibration of a glass electrode gave a reading of 134.9 mV with a 0.05 m potassium hydrogen phthalate buffer standard ( pH = 4.015), and a reading of -69.1 mV with a 0.08 m HEPES, 0.08 m NaHEPES, 0.08 m NaCl buffer standard (pH = 7.454), both measured at 30 °C. What is the observed slope (mV/pH unit) of the calibration curve? slope observed slope theoretical What is the theoretical slope at 30 °C? pH -58.1 5.29 Incorrect What is the pH of an unknown that gives a reading of 41.4 mV with this electrode at 30 °C? Incorrect Incorrect mV/pH mV/pH3) Name the errors of glass electrodes in potentiometric measurements (please write correctly and concisely).
- Consider the titration of 100.0 mL of 0.010 0 M Ce4+ in 1 M HClO4 with 0.040 0 M Cu+ to give Ce3+ and Cu2+. Calculate the potential of the indicator electrode after adding 24.5 mL of Cu+.21-27, The F- concentration of a solution was determined by measurements with a liquid-membrane elec- trode. The electrode system developed a potential of 0.5021 V when immersed in 25.00 mL of the sam- ple, and 0.4213 V after the addition of 2.00 mL of 5.45 × 10¬²M NaF. Calculate pF for the sample.A Cu²+ ion-selective electrode was calibrated using metal ion buffers with a constant ionic strength. The response of [Cu²+] (M) [Mg?+] (M) Response (mV) 3.08 × 10-6 -66.78 the electrode to these buffer solutions is shown in the table. 7.79 × 10-4 1.49 Additionally, the response of the electrode to a solution containing Cu2+ and Mg²+ is also shown in the table. From 3.08 x 10-6 0.0169 -34.86 this information, calculate the selectivity coefficient for Mg²+, KPOM24, for this Cu2+ ion-selective electrode. K Pot Cu2+,Mg²+
- 14-44. A Ca* ion-selective electrode was calibrated in metal ion buffers with ionic strength fixed at 0.50 M. Using the following elec- trode readings, write an equation for the response of the electrode to Ca²* and Mg**. [Ca²*] (M) 2+ [Mg*] (M) mV . 1.00 X 10-6 2.43 X 10 1.00 X 10 -52.6 4 +16.1 9- 3.68 X 10 - 38.0The potential difference between a potassium ion and saturated calomel electrode immersed in 100.0 ml of 1.073 x 103 M KCI was 362 mV. When 594 mg of NHẠCI was added to the KCI solution (no volume change), the potential difference was 386 mV. Calculate the selectivity coefficient kxt,NH, for K* over NH4. Assume that there is no loss of NH4 due to acid-base equilibrium effects.7. In an experiment on the Pt| Ha| H' electrode in dilute H.SO4, the following current densities were observed at 25°C. Evaluate a and I, for the electrode. n/mV 50 100 150 I/ mA cm2 200 29.9 100 250 335 2.66 8.91
- The following data were measured in a 1.00-cm cell. Concentration (M) %T 1.50x10-4 14.9 1.00×10-4 26.1 7.50x10-5 38.0 5.00x10-5 54.3 3.00x10-5 65.7 Determine the molar absorptivity( in cm ¹M-¹) using graphical methods.Chemistry 15-42. The selectivity coefficient, KP, H, for a Li ion-selective electrode is 4 x 10-4. When this electrode is placed in 3.44 x 104 M Lit solution at pH 7.2, the potential is -0.333 V versus S.C.E. What would be the potential if the pH were lowered to 1.1 and the ionic strength were kept constant? Answer should be -0.331 VA 40.00-mL aliquot of 0.05000 M HNO2 is diluted to 75.00 mL and titrated with 0.0800 M Ce4+. The pH of the solution is maintained at 1.00 throughout the titration; the formal potential of the cerium system is 1.44 V. Calculate the potential of the indicator electrode with respect to a saturated calomel reference electrode after the addition of 5.00, 10.00, 15.00, 25.00, 40.00, 49.00, 49.50, 49.60, 49.70, 49.80, 49.90, 49.95, 49.99, 50.00, 50.01, 50.05, 50.10, 50.20, 50.30, 50.40, 50.50, 51.00, 60.00, 75.00, and 90.00 mL of cerium(IV). Generate a titration curve for these data. Upload your excel file showing the titration curve and manual computations. Upload Choose a file
