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 0.3691 V after the addition of 2.00 mL of M . Calculate pF for the sample.
The F- concentration of a solution was determined by measurements with a liquid-membrane electrode. The electrode...
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 0.4271 V after the addition of 2.00 mL of 5.45 x 10-2 M NaF. Calculate pF for the sample.
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.
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.
When a hydrogen electrode and a normal electrode are immersed in a solution at 25C a potential of 0.664 V is obtained. Calculate (a) the pH and (b) the hydrogen-ion activity.
Help! Electrochem questions: (1) An electrochemical cell consisting of a cadmium electrode immersed in a solution of 0.001M cadmium (II) nitrate, and a hydrogen electrode. The hydrogen electrode contains a solution of hydrogen cyanide. The pressure of the hydrogen gas is 1 atm. What is the concentration of the acid when there is measured a potential of 0,220V at 25 ° C. (2)A galvanic cell is composed of copper / copper ion solution (0.1M) on the one hand, and a...
The concentration of a Fe2+ solution
is determined by titrating it with a 0.1462 M
solution of Ce4+. The balanced net
ionic equation for the reaction is shown below.
Ce4+(aq)
+ Fe2+(aq)
Ce3+(aq)
+ Fe3+(aq)
In one experiment, 16.48 mL of the
0.1462 M Ce4+ solution
is required to react completely with 25.00 mL of
the Fe2+ solution. Calculate the
concentration of the Fe2+ solution.
7) An ion selective electrode and reference electrode pair were placed in 100.00 mL of the sample, and a reading of 21.6 mV was obtained. After the addition of 10.00 mL of a standard solution with a concentration of 100 ug/mL, the electrode pair gave a reading of 43.7 mV. The response slope (i.e., the slope of the line give by the equation E=mx+ constant, where x = log[ion]) was previously determined to be 57.8 mV. What is the sample...
The concentration of Cu+ in a solution is determined by titrating it with a 0.1621 M permanganate solution. The balanced net ionic equation for the reaction is: MnO4-(aq) + 5Cu+(aq) + 8H3O+(aq) Mn2+(aq) + 5Cu2+(aq) + 12H2O(l) In one experiment, 18.21 mL of the 0.1621-M permanganate solution is required to react completely with 25.00 mL of the Cu+ solution. Calculate the concentration of the Cu+ solution.
The concentration of H3AsO3 in a solution is determined by titrating it with a 0.1807 M Ce4+ solution. The balanced net ionic equation for the reaction is: 2Ce4+(aq) + H3AsO3(aq) + 5H2O(l) 2Ce3+(aq) + H3AsO4(aq) + 2H3O+(aq) In one experiment, 22.27 mL of the 0.1807 M Ce4+ solution is required to react completely with 25.00 mL of the H3AsO3 solution. Calculate the concentration of the H3AsO3 solution?
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.