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A sodium ISE and a SCE were immersed in a solution containing 2.0x103 M Na. The...
A Ca ISE and a SCE were immersed in a standard containing 2.0x10" M Ca**. The cell potential was +0.2714 V. The two...
A Ca ISE and a SCE were immersed in a standard containing 2.0x10" M Ca**. The cell potential was +0.2714 V. The two electrodes were then rinsed and transferred to a sample; the cell potential was +0.2837 V. Calculate the concentration of Caassuming that the Ca ISE has an ideal slope of 0.02958 V.
A Mg* liquid membrane ISE and a Ag/AgCl reference electrode were mL of solution containing an...
A Mg* liquid membrane ISE and a Ag/AgCl reference electrode were mL of solution containing an unknown concentration of Mg2+. The cell voltage was +0.4960 V. Without removing the electrodes, 10.0 mL of 5.0x10-2 M Mg was the solution and mixed. The new cell voltage was +0.5025 V. Assuming that the Mg has an ideal slope of 0.02958 V; calculate the original Mg2+ concentration.
In a cell constructed between a compartment containing a zinc electrode immersed in a 0.10 M...
In a cell constructed between a compartment containing a zinc electrode immersed in a 0.10 M ZnSO4(aq) solution and a compartment containing a copper electrode immersed in a 0.10 M CuSO4(aq) solution, a.) which electrode will be the anode? b.) what is the standard cell potential? c.) what is the theoretical cell potential with these concentrations? d.) write the line notation for this cell.
A sodium ion electrode was calibrated by measuring the cell potentials of several standard Na+ solutions....
A sodium ion electrode was calibrated by measuring the cell potentials of several standard Na+ solutions. The other electrode was the SCE. The calibration data are shown in the following table. Log[Na+] Ecell (mV) -1 -165.6 0 -110.0 1 -51.8 2 6.5 3 64.5 a. Plot a calibration curve for these data. b. Determine the slope and intercept for the regression line of this plot. Is the response of this sodium electrode Nernstian? Explain. c. A 10.00mL aliquot of table...
Potential (mV) [Br](M) 0.300 Calibration data for a bromide ion-selective electrode (ISE) was collected and recorded in...
Potential (mV) [Br](M) 0.300 Calibration data for a bromide ion-selective electrode (ISE) was collected and recorded in the table. The potential of the ISE was measured against a saturated calomel electrode (SCE). All solutions were buffered at a pH of 7.56. A linear calibration curve can be constructed from this data as a plot of potential (in mV) vs. pBr. Determine the slope and y-intercept of such a plot of the calibration data given. -21.2 0.0300 36.2 95.7 0.00300 0.000300...
A copper, Cu(s), electrode is immersed in a solution that is 1.00 M in ammonia, NH3,...
A copper, Cu(s), electrode is immersed in a solution that is 1.00 M in ammonia, NH3, and 1.00 M in tetraamminecopper(II), [Cu(NH3)4]2+. If a standard hydrogen electrode is used as the cathode, the cell potential, Ecell, is found to be 0.068 V at 298 K. Based on the cell potential, what is the concentration of Cu2+ in this solution? Express your answer to one significant figure and include the appropriate units.
A 0.200 M solution of HCl is added to a solution containing 0.150 moles of sodium...
A 0.200 M solution of HCl is added to a solution containing 0.150 moles of sodium phosphate (Na3PO4). The resulting solution is then diluted to exactly 1.00 L, at which time the pH was found to be pH 8.00. What is the concentration of H2PO4- in the solution? For phosphoric acid, Ka1 = 7.11 x 10-3, Ka2 = 6.32 x 10-8, and Ka3 = 7.1 X 10-13.
1-7 Data Concentration of the Na S.O, solution: 0.0500 M Part I. Molar Solubility in pure...
1-7
Data Concentration of the Na S.O, solution: 0.0500 M Part I. Molar Solubility in pure water Data Trial 1 Trial 2 Volume saturated Ca(10), titrated, mL 10.00 10.00 Final buret reading, mL (Sin becomes colorless.) 28.15 27.50 Initial buret reading, mL 0.00 0.00 Volume delivered, mL AV = V-V Part II. Molar Solubility in 0.0100 M KIO, Data Trial 2 Trial 1 10.00 10.00 Volume Ca(10), in KIO, titrated, mL 40.45 39.95 Final buret reading, mL (Sin becomes colorless.)...
A cell consisting of a saturated calomel electrode and a lead electrode developed a potential of...
A cell consisting of a saturated calomel electrode and a lead electrode developed a potential of -0.4706 V when immersed in 50.00 mL of a sample. A 5.00 mL addition of standard 0.02 M lead solution caused the potential to shift to -0.4490 V. Calculate the molar concentration of lead in the sample.
3. For a voltammetric measurement, calculate the decomposition potential relative to SCE, for the reduction of Sr to Sr in a solution containing 2.23 mM of Sr(NOs)h and a total ionic strength of 0.01...
3. For a voltammetric measurement, calculate the decomposition potential relative to SCE, for the reduction of Sr to Sr in a solution containing 2.23 mM of Sr(NOs)h and a total ionic strength of 0.01 M. Be sure to account for effects of activity
3. For a voltammetric measurement, calculate the decomposition potential relative to SCE, for the reduction of Sr to Sr in a solution containing 2.23 mM of Sr(NOs)h and a total ionic strength of 0.01 M. Be sure...
A Ca ISE and a SCE were immersed in a standard containing 2.0x10" M Ca**. The cell potential was +0.2714 V. The two electrodes were then rinsed and transferred to a sample; the cell potential was +0.2837 V. Calculate the concentration of Caassuming that the Ca ISE has an ideal slope of 0.02958 V.
A Mg* liquid membrane ISE and a Ag/AgCl reference electrode were mL of solution containing an unknown concentration of Mg2+. The cell voltage was +0.4960 V. Without removing the electrodes, 10.0 mL of 5.0x10-2 M Mg was the solution and mixed. The new cell voltage was +0.5025 V. Assuming that the Mg has an ideal slope of 0.02958 V; calculate the original Mg2+ concentration.
Potential (mV) [Br](M) 0.300 Calibration data for a bromide ion-selective electrode (ISE) was collected and recorded in the table. The potential of the ISE was measured against a saturated calomel electrode (SCE). All solutions were buffered at a pH of 7.56. A linear calibration curve can be constructed from this data as a plot of potential (in mV) vs. pBr. Determine the slope and y-intercept of such a plot of the calibration data given. -21.2 0.0300 36.2 95.7 0.00300 0.000300...
1-7
Data Concentration of the Na S.O, solution: 0.0500 M Part I. Molar Solubility in pure water Data Trial 1 Trial 2 Volume saturated Ca(10), titrated, mL 10.00 10.00 Final buret reading, mL (Sin becomes colorless.) 28.15 27.50 Initial buret reading, mL 0.00 0.00 Volume delivered, mL AV = V-V Part II. Molar Solubility in 0.0100 M KIO, Data Trial 2 Trial 1 10.00 10.00 Volume Ca(10), in KIO, titrated, mL 40.45 39.95 Final buret reading, mL (Sin becomes colorless.)...
3. For a voltammetric measurement, calculate the decomposition potential relative to SCE, for the reduction of Sr to Sr in a solution containing 2.23 mM of Sr(NOs)h and a total ionic strength of 0.01 M. Be sure to account for effects of activity
3. For a voltammetric measurement, calculate the decomposition potential relative to SCE, for the reduction of Sr to Sr in a solution containing 2.23 mM of Sr(NOs)h and a total ionic strength of 0.01 M. Be sure...
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