Chemical Reactions

The rise in pressure due to heating causes more N₂O₄ to gasify, resulting in higher concentrations and stronger color.

The equilibrium between N₂O₄ and NO₂ shifts to the right, favoring formation of more NO₂, a brown colored gas, in response to the increase in temperature.

Heat causes the decomposition of some N₂O₄ into individual nitrogen and oxygen atoms with no color change involved.

The mixture has reacted with the container material to form additional NO₂, giving rise to increased color intensity.

H₃PO₃

PO₃²⁻

H₂PO₄⁻

H₃PO₄

The equilibrium shifts towards the side with fewer moles of gas due to increased pressure favoring lower volume.

It causes equal shifts in both directions since all gases compress uniformly upon volume reduction.

The equilibrium shifts towards the side with more moles of gas trying to restore original pressure conditions.

Equilibrium remains unchanged because temperature is constant and not affected by volume changes.

Redox potential of a solution.

Concentration of hydroxide ions in a solution.

Concentration of hydronium ions in a solution.

Acidity or basicity of a solution.

One-to-one correlation means both counterbalance each other entirely.

Effectively, large values indicate equally powerful acids and bases.

Larger value Ka corresponds to a smaller value Kb, inversely related strength.

Generally, higher indicates greater reactivity regardless of acidity or baseness.

Ion-dipole interactions in both substances

Hydrogen bonding in water but not acetone

Dipole-induced dipole interactions being stronger in water

London dispersion forces being dominant in acetone

HNO₃

HCl

HBr

H₂O

Nitrous acid (HNO2)

Hydrocyanic acid (HCN)

Acetic acid (CH3COOH)

Hypochlorous acid (HOCl)

Kw variation indicates that pH levels of the solution remain fixed irrespective of temperature alterations as suggested by neutralization reactions.

An alteration in Kw would impact electrolytic conductivity without changing acid/base characteristics as this remains constant under Bronsted-Lowry theory.

The change in Kw signifies that temperature modulation affects the extent of ionization of water molecules subject to the specific conditions provided by Arrhenius definition of acids and bases.

Change in Kw implies that salts' dissolving capacity is independent of fluctuations in temperature guided by a concept similar to a solution's saturation point.

Acidity

Reducing ability

Oxidation potential

Basicity