Potentiometry in Electrochemistry Quiz

A method of analysis where the concentration of a specific ion or substance is determined by measuring the potential difference generated when a special electrode is placed in its solution.

An instrument used in potentiometry to measure the potential difference between two electrodes in a circuit.

A device used to connect two solutions of different compositions, allowing for the flow of ions while maintaining electrical neutrality.

The potential difference that arises at the interface between two solutions with different ionic compositions.

Electrodes that maintain a constant and predictable potential, serving as a reference point for measuring the potential of the other electrode.

The tendency of a metal to lose electrons and go into solution as ions, creating a positive charge.

The tendency of ions in solution to gain electrons and deposit onto the metal surface.

The relationship between the potential difference of an electrochemical cell and the concentrations of the reactants involved, governed by the Nernst Equation.

A type of electrode used in electrochemical reactions that doesn't participate in the reaction, only facilitating electron transfer.

The potential of a half-cell under standard conditions, where all concentrations are 1M and the temperature is 25 °C.

Oxidation and reduction reactions where the reactants are ions in solution, often facilitated by an inert electrode.

The potential of a single electrode cannot be measured directly. It must be compared to a reference electrode with a known and stable potential, creating an electrochemical cell.

The force that drives the flow of electrons in an electrochemical cell, measured in volts.

The electrode that determines the concentration of the ion being measured.

A device that provides a variable potential to oppose the cell's EMF, allowing for precise EMF measurement without drawing current.

The change in EMF of an electrochemical cell is directly related to the change in the indicator electrode's potential, which is influenced by the ion concentration in the solution.

A device that connects two half-cells in an electrochemical cell, allowing for the flow of ions while preventing the solutions from mixing.

The potential difference that arises at the interface between two solutions with different ionic compositions. It's caused by the difference in migration rates of ions.

A potential generated due to the unequal distribution of charges at the boundaries of a salt bridge. This is caused by differences in the migration rates of anions and cations.

A potential developed at the boundaries of the junction between a salt bridge and the half-cell solutions. It's caused by the difference in ion migration rates.

A special type of voltage divider that allows for accurate measurement of a galvanic cell's potential difference. It adjusts the potential across the cell until zero current is detected, signifying potential equality.

It's a method used to minimize junction potential by selecting a salt bridge electrolyte with similar ion mobilities. This ensures equal charge distribution and reduces the potential difference.

A device that supplies a variable potential to a galvanic cell until a zero current reading is observed, indicating the potential difference between the cell and the voltage divider is equal.

The tendency of a metal to lose electrons and form ions in solution, creating a positive charge.

The Nernst equation links the potential of an electrochemical cell to the concentrations of the reactants involved.

The silver-silver chloride electrode is a reference electrode commonly used in electrochemistry, where the potential is dependant on the chloride ion concentration.

The solubility product of silver chloride (AgCl) is expressed as the product of the concentrations of silver ions (Ag+) and chloride ions (Cl-), representing the maximum amount of dissolved AgCl.

The potential of the silver-silver chloride electrode is influenced by the chloride ion concentration, with higher chloride concentrations resulting in lower electrode potentials.

The electrode potential of the silver-silver chloride electrode is determined by the chloride ion concentration in the solution it's in.

The electrode potential is 0.197 V for saturated KCl and 0.205 V for 3.5M KCl.

The electrode potential is a measure of the tendency for a chemical reaction to occur at an electrode. A positive potential indicates a tendency for the reaction to occur.

The potential of the silver-silver chloride electrode is a standard reference point used for measuring the potential of other electrodes in electrochemical cells.

When a high concentration of a salt is used in the bridge to minimize the impact of different ion migration rates. This results in a more stable and predictable potential measurement.

A primary reference electrode based on the reaction between hydrogen ions and hydrogen gas. Its potential is defined as 0 volts at standard conditions.

A type of reference electrode that uses a combination of mercury, mercurous chloride (calomel), and a specific electrolyte solution to maintain a stable potential.

This electrode utilizes silver, silver chloride, and a saturated potassium chloride solution to maintain a constant and predictable reference potential.

These electrodes are used for measuring potential differences in electrochemical cells. Their potential is constant and well-defined, acting as a reference point for measuring the potential of other electrodes.