Weak acids do not completely dissociate in solution and typically have a higher pKa value compared to strong acids.

Molecular orbital theory explains the magnetic properties of molecules, including paramagnetism and diamagnetism.

Not all molecular orbitals are degenerate; some can have different energy levels.

A buffer solution resists changes in pH upon the addition of small amounts of acid or base.

At equilibrium, the rates of the forward and reverse reactions are equal, not necessarily the concentrations.

An exothermic reaction releases heat, resulting in a negative enthalpy change.

Catalysts provide an alternative pathway with lower activation energy, thus increasing the rate of the reaction without being consumed.

Dynamic equilibrium occurs when the rate of the forward reaction equals the rate of the reverse reaction, not necessarily when concentrations are equal.

Electrolysis involves the decomposition of a compound using electrical energy.

Electrolytic cells require an external power source to drive the non-spontaneous reactions.

Gases fill the shape of their container because their particles are far apart and move freely.

The correct equation for Gibbs Free Energy is ΔG = ΔH - TΔS, which relates enthalpy, entropy, and temperature.

Ionic compounds are generally soluble in water due to the polar nature of water molecules.

Isotopes have the same number of protons but different numbers of neutrons.

Liquids have a fixed volume and are incompressible, but they do not have a definite shape.

Real gases experience intermolecular forces, which is why they deviate from ideal behavior under certain conditions.

Redox reactions involve the transfer of electrons between species.

Both statements A and B are true regarding electron configurations.

Kp is dependent on temperature and can vary with changes in temperature.

Molecular orbital theory explains the magnetic properties of molecules, particularly the presence of unpaired electrons.

The second law of thermodynamics states that the total entropy of an isolated system can never decrease over time.

Bonding orbitals are lower in energy than antibonding orbitals, which is a fundamental principle of molecular orbital theory.

Raoult's Law indicates that the vapor pressure of a solution is lower than that of the pure solvent due to the presence of solute.

The first law of thermodynamics states that energy can only be transformed from one form to another, not created or destroyed.

According to the kinetic molecular theory, gas particles are in constant motion.

The second law states that heat cannot spontaneously flow from a colder body to a hotter body, which implies that entropy of the universe tends to increase.

In an adiabatic process, the system is insulated from heat transfer, meaning no heat is exchanged with the surroundings.

In an endothermic reaction, the enthalpy change (ΔH) is positive as heat is absorbed.

In an exothermic reaction, heat is released, so ΔH is negative.

In an isobaric process, the pressure remains constant.