Acids and Bases

It is monoprotic

It is diprotic

It is polyprotic

Cannot be determined

Increasing pressure has no effect on gas-phase reactions at equilibrium.

Increased pressure slows down all gas-phase reactions due to decreased volume available for collisions.

Increasing pressure shifts equilibrium toward fewer moles of gas if possible.

Increasing pressure always results in equal adjustments among all gases present.

Binary acid

Oxyacid

Carboxylic acids

Metal hydroxides.

Decreasing temperature

Removing O2

Adding more SO2

Increasing pressure

CH3OH2 is stronger than CH3OH

For a strong acid-weak base titration, the pH at equiv. point is less than 7.

For a strong acid-base titration, the equiv. point occurs when the pH is 7.

HBr is more acidic than HI.

NH3 (ammonia)

CH4 (methane)

BeH2 (beryllium hydride)

CO2 (carbon dioxide)

It releases hydroxide ions OH- into solution

It forms hydronium ion $H_3O^+$ and chloride ion $Cl^-$

It forms pure hydrogen gas bubbles

It produces multiple covalently bonded hydrogen molecules

It decreases both forward and reverse reaction rates equally with no net shift in position.

It shifts equilibrium toward products due to increased kinetic energy overcoming activation energy barriers more easily.

It increases both forward and reverse reaction rates equally with no net shift in position.

It shifts the equilibrium toward reactants because heat acts as a product.

HBr because it has a larger atomic radius.

HCl because it has a higher electronegativity difference.

They have equal hydrogen bonding capabilities due to their similar structures.

Neither; they do not form hydrogen bonds.

Forming hydronium ions ($H_{3}O^{+}$) after reacting with sulfur dioxide.

Breaking of hydrogen bonds between water molecules.

Formation of covalent bonds between water and nitrogen gas.

Ionization of water into hydroxide ions ($OH^{-}$) and isolated protons ($H^{+}$).