Electrolytic Conductance and Cells

False (B)

Conductivity increases with temperature.

<p>resistance</p> Signup and view all the answers

<p>Specific conductance = Conductance of a solution per unit length and area Equivalent conductance = Conductance related to the amount of solute Normality = Number of equivalents of solute per liter of solution Molarity = Number of moles of solute per liter of solution</p> Signup and view all the answers

<p>Color of the solution (A)</p> Signup and view all the answers

<p>Resistance is 5 ohms.</p> Signup and view all the answers

<p>False (B)</p> Signup and view all the answers

<p>It increases. (D)</p> Signup and view all the answers

<p>True (A)</p> Signup and view all the answers

<p>Each ion makes a definite contribution to the conductance regardless of the associated ions.</p> Signup and view all the answers

<p>AB ↔ A+ + B-</p> Signup and view all the answers

<p>Molar Conductance = Increases with higher dilution Degree of Dissociation = Fraction of molecules dissociated into ions Ostwald Dilution Law = Degree of dissociation proportional to square root of dilution Kohlrausch's Law = Ions contribute to conductance at infinite dilution</p> Signup and view all the answers

<p>$ohm^{-1} cm^2 eqvt^{-1}$ (A)</p> Signup and view all the answers

<p>True (A)</p> Signup and view all the answers

<p>It increases and attains a maximum value called the limiting value.</p> Signup and view all the answers

<p>cell constant</p> Signup and view all the answers

<p>Concentration of ions (B)</p> Signup and view all the answers

<p>Specific conductance = Conductance of 1 cc of solution Equivalent conductance = Conductance related to 1 gram equivalent of electrolyte Molar conductance = Conductance related to 1 mole of electrolyte Cell constant = Ratio of distance between electrodes to cross-sectional area</p> Signup and view all the answers

<p>Equivalent conductance increases with dilution and is dependent on the degree of dissociation (α).</p> Signup and view all the answers

<p>$\frac{l}{A}$</p> Signup and view all the answers

<p>Mho per centimeter (mho/cm) (B)</p> Signup and view all the answers

<p>False (B)</p> Signup and view all the answers

<p>Electrolysis</p> Signup and view all the answers

<p>resistance</p> Signup and view all the answers

<p>Wheatstone bridge (D)</p> Signup and view all the answers

<p>False (B)</p> Signup and view all the answers

<p>Molar conductance is the conducting ability of one mole of an electrolyte in a solution.</p> Signup and view all the answers

<p>Solutions with high conductivity (C)</p> Signup and view all the answers

<p>False (B)</p> Signup and view all the answers

<p>Siemens per meter (S/m)</p> Signup and view all the answers

<p>electrical conductivity</p> Signup and view all the answers

<p>All of the above (D)</p> Signup and view all the answers

<p>Acid-base titration = Involves a change in pH Redox titration = Involves electron transfer reactions Complexometric titration = Involves the formation of complexes Precipitation titration = Involves the formation of a precipitate</p> Signup and view all the answers

<p>True (A)</p> Signup and view all the answers

<p>It is faster</p> Signup and view all the answers

<p>Equivalent conductance at infinite dilution (C)</p> Signup and view all the answers

<p>False (B)</p> Signup and view all the answers

<p>λ_∞ = λ_a + λ_c</p> Signup and view all the answers

<p>velocity</p> Signup and view all the answers

<p>Strong acid-strong base titration = Conductance decreases then increases Weak acid-strong base titration = Conductance increases slowly then sharply Strong acid-weak base titration = Conductance decreases then increases after equivalence point Weak acid-weak base titration = Conductance decreases then increases after equivalence point</p> Signup and view all the answers

<p>Weak acid-strong base titration (C)</p> Signup and view all the answers

<p>True (A)</p> Signup and view all the answers

<p>Conductance initially decreases, then increases.</p> Signup and view all the answers

The ability of a solution to conduct electricity due to the presence of ions.

The conductance of a 1 cm³ cube of a solution.

Conductance of ions produced by one gram equivalent of an electrolyte in a solution.

A substance that forms ions in solution and conducts electricity.

The ability of a substance to conduct electricity.

Resistance is directly proportional to length and inversely proportional to cross-sectional area.

A titration method using conductance to determine the concentration of an unknown solution.

Resistance of a material with a unit length and area.

The conductance of 1 cubic centimeter (cc) of an electrolyte solution.

Conductance of 1 mole of an electrolyte in solution.

Maximum equivalent conductance of an electrolyte, measured at infinite dilution

Electrolytes that completely ionize in solution.

Electrolytes that only partially ionize in solution.

Ratio of distance between electrodes to cross-sectional area of electrode.

Process of finding conductance of a solution by measuring its resistance via Wheatstone bridge.

Molar conductance of an electrolyte increases with dilution, as more ions are present in the solution, leading to better conductivity.

Strong electrolytes fully dissociate into ions in solution, while weak electrolytes partially dissociate. This explains their varying conductivity.

The fraction of electrolyte molecules that break up into ions in a solution. It indicates the strength of an electrolyte.

This law states that the degree of dissociation of a weak electrolyte is proportional to the square root of its dilution.

At infinite dilution, each ion contributes independently to the total conductivity, regardless of the other ions. This allows us to calculate molar conductivity at infinite dilution.

The ratio of the distance between the electrodes (l) to the cross-sectional area of the electrodes (A) in a conductivity cell. It represents the cell's ability to conduct electricity.

Conductance of an electrolytic solution usually increases with temperature. This happens due to increased ion movement and decreased solvent viscosity.

For weak electrolytes, temperature's effect on conductance depends on the change in enthalpy during their ionization. An endothermic ionization increases conductance with temperature, while an exothermic ionization decreases conductance.

A Wheatstone bridge is used to measure the resistance of a conductivity cell. It allows for precise measurement of the cell's resistance.

The cell constant is crucial for calculating the specific conductance of a solution. It takes into account the dimensions of the conductivity cell, ensuring accurate measurement of the conductivity.

The conductance of a solution containing one gram equivalent of an electrolyte when the concentration approaches zero. This value represents the maximum possible conductance for the electrolyte.

The equivalent conductance of an electrolyte at infinite dilution is the sum of the equivalent conductances of the individual ions.

The velocity of an ion in cm/sec under a potential gradient of one volt per centimeter.

Conductometric titration involving a strong acid and strong base. The conductance initially decreases and then increases after complete neutralization.

Conductometric titration involving a weak acid and strong base. Conductance increases slowly initially, then increases sharply after the equivalence point.

Conductometric titration involving a strong acid and weak base. Conductance decreases initially then increases after the equivalence point.

Conductometric titration involving a weak acid and weak base. Conductance initially decreases then increases after the equivalence point, but the endpoint is not as sharp as strong acid-strong base titrations.

They are inversely proportional. Higher conductivity means lower resistance, and vice versa.

Temperature, Pressure, and pH all impact the electrical conductivity of a solution.

Siemens per meter (S/m)

A conductance cell is used to measure the conductivity of a solution.

It's indicated by the maximum change in electrical conductivity. This is when the reaction is complete.

Solutions with low conductivity are most suitable.

It's faster and requires fewer reagents compared to other titration methods.