Acids and Bases

The equilibrium constant (K) value will increase.

The reaction rate of the forward reaction will increase.

The equilibrium will shift towards the reactants.

The pH of the solution will increase without affecting equilibrium.

7

1

0

14

0.1 M HCl

0.1 M NaOH

0.1 M Ca(OH)2

Pure water (H2O)

Water

Acid

Salt

Base

A donation of electron pairs

Neither an electron donor nor a proton acceptor

Both a proton donor and an electron acceptor

An acceptor of protons

Sodium bicarbonate and hydrochloric acid

Sodium chloride and water

Hydrogen gas and sodium chloride

Chlorine gas and sodium oxide

The equilibrium shifts toward reactants, producing fewer products.

The rate of both forward and reverse reactions increases equally.

There is no change in position as temperature does not affect neutralization reactions.

More products are formed as higher temperature favors formation of more stable compounds.

Bases donate H+ ion whereas acids accept it.

Acids donate H+ ion whereas bases accept it.

Acids and bases are determined by their pH values.

Acids decrease H+ ion while bases increase it.

They form coordinate covalent bonds.

They differ by a single proton (H+).

They act only as electron pair donors.

They share an equal number of electrons during reactions.

Vinegar

Baking soda

Tomato juice

Lemon juice