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.
When a hydrogen electrode and a normal electrode are immersed in a solution at 25C a...
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...
When an ion‑selective electrode for X+ was immersed in 0.0709 M XCl, the measured potential was 0.0430 V . What is the concentration of X+ when the potential is 0.0580 V ? Assume that the electrode follows the Nernst equation, the temperature is at 25 °C, and that the activity coefficient of X+ is 1.
When an ion‑selective electrode for X+ was immersed in 0.0652 M XCl, the measured potential was 0.0420 V . What is the concentration of X+ when the potential is 0.0570 V ? Assume that the electrode follows the Nernst equation, the temperature is at 25 °C, and that the activity coefficient of X+ is 1.
When an ion‑selective electrode for X+ was immersed in 0.0312 M XCl, the measured potential was 0.0230 V . What is the concentration of X+ when the potential is 0.0380 V ? Assume that the electrode follows the Nernst equation, the temperature is at 25 °C, and that the activity coefficient of X+ is 1.
A pH electrode is attached to a voltmeter that reads 0.253V when the electrode is immersed in a buffer solution with a pH of 3.25 at 25 degree C. After the pH electrode is moved to an unknown buffer solution at 25 degree C, the reading of the voltmeter is lowered by 43%. From the Nernst potential equation, come up with an equation relating the measured voltage (delta psi = psi_sensor - psi_solution) to the pH of the solution. Calculate...
When an ion-selective electrode for X was immersed in 0.0470 M XCI, the measured potential was 0.0340 V. What is the concentration of X when the potential is 0.0490 V? Assume that the electrode follows the Nernst equation, the temperature is at 25°C, and that the activity coefficient of X is 1 Number
When an ion-selective electrode for X+ was immersed in 0.0784 M XCI, the measured potential was 0.0430 V. What is the concentration of X* when the potential is 0.0580 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]0.117
When an ion-selective electrode for X was immersed in 0.0520 M XCI, the measured potential was 0.0380 V. What is the concentration of X when the potential is 0.0530 V? Assume that the electrode follows the Nemst equation, the temperature is at 25 C, and that the activity coefficient of X* is 1 Number 0.3M
When an ion-selective electrode for X+ was immersed in 0.0480 M XCI, the measured potential was 0.0430 V. What is the concentration of X+ when the potential is 0.0580 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+) = 1.792 1.792
A voltaic cell is constructed in which the cathode is a standard hydrogen electrode and the anode is a hydrogen electrode ()= 1atm) immersed in a solution of unknown [H+]. If the cell potential is 0.179 V, what is the pH of the unknown solution at 298 K? pH =