A catalyst does not affect the position of equilibrium; it only speeds up the rate at which equilibrium is reached.

The addition of a non-volatile solute raises the boiling point of the solvent, a phenomenon known as boiling point elevation.

A catalyst speeds up the rate of both the forward and reverse reactions equally, thus having no effect on the position of equilibrium.

A catalyst increases the rate of both the forward and reverse reactions equally, thus it does not shift the position of equilibrium.

Adding a common ion decreases the solubility of a salt in a saturated solution due to the common ion effect.

Adding a non-volatile solute decreases the vapor pressure of the solvent due to the reduction in the mole fraction of the solvent.

Adding a solute to a solvent increases the boiling point of the solution, a phenomenon known as boiling point elevation.

A buffer solution is designed to resist changes in pH, so adding a strong acid will cause only a small change in pH.

Adding a strong base to a buffer solution will increase the pH, but the buffer will resist significant changes in pH due to the presence of the weak acid.

Adding an inert gas at constant volume does not change the partial pressures of the reactants and products, so the equilibrium position remains unchanged.

Adding an inert gas at constant volume does not change the partial pressures of the reactants and products, thus it has no effect on the equilibrium position.

Adding an inert gas at constant volume does not change the partial pressures of the reactants or products, hence no effect on equilibrium.

Diluting a strong acid decreases its concentration, which increases the pH (making it less acidic).

Dilution of a strong acid decreases its concentration, thus increasing the pH.

Dilution of a weak acid decreases its concentration, which shifts the equilibrium to the right, increasing the concentration of H+ ions and thus increasing the pH.

Increasing electronegativity difference between two atoms leads to an increase in ionic character of the bond.

Increasing pressure raises the boiling point of a liquid.

Increasing temperature will make ΔG more negative for a reaction with a negative ΔH and positive ΔS, enhancing spontaneity.

For a reaction with ΔH > 0 and ΔS < 0, increasing temperature will make ΔG more positive, thus decreasing spontaneity.

For an exothermic reaction, increasing the temperature shifts the equilibrium to the left, favoring the reactants.

Increasing temperature generally decreases physisorption because it disrupts the weak van der Waals forces.

The effect of increasing temperature on cell potential depends on the reaction and its enthalpy change.

The effect of temperature on cell potential depends on the reaction and its enthalpy change.

Generally, the density of liquids decreases with an increase in temperature.

Increasing temperature generally increases the kinetic energy of particles, leading to greater disorder and thus an increase in entropy.

Increasing temperature generally increases the entropy of a system as the molecular motion becomes more chaotic.

For endothermic reactions, increasing temperature shifts the equilibrium to the right, increasing Kc.

For an endothermic reaction, increasing the temperature increases the equilibrium constant.

According to Le Chatelier's principle, increasing the temperature of an exothermic reaction shifts the equilibrium to the left, decreasing the equilibrium constant.

Increasing temperature increases the kinetic energy of gas molecules.