Equilibrium

The system must be open to the atmosphere

The system must be closed

The temperature must be changing

The pressure must be zero

$K_p = P_{solid}$

$K_p = P_{vapor}$

$K_p = P_{vapor} / P_{solid}$

$K_p = P_{vapor} + P_{solid}$

Chemical equilibrium

Physical equilibrium

Thermal equilibrium only

Unstable equilibrium

The concentration of the solution increases

The concentration of the solution decreases

The added salt remains undissolved and concentration stays the same

The solution becomes unsaturated

Continuous addition of reactants

Removal of products as they form

Constant temperature

An open container

Saturated

Unsaturated

Supersaturated

At equilibrium

$mol \\, L^{-1}$

$L \\, mol^{-1}$

$mol^2 \\, L^{-2}$

Unitless

Change in temperature

Change in concentration of reactants

The nature of the reaction

Stoichiometry of the reaction

$K_1 = K_2$

$K_1 \\times K_2 = 1$

$K_1 + K_2 = 1$

$K_1 / K_2 = 1$

Increasing the volume of the container

Adding more $CH_4$

Increasing the pressure

Removing $CO$ as it is formed

It allows the reaction to occur at a lower temperature with a reasonable rate

It shifts the equilibrium to favor ammonia

It increases the equilibrium constant $K_p$

It decreases the pressure needed for the reaction

Towards the products (Forward)

Towards the reactants (Backward)

It remains at equilibrium

The reaction stops

Pure water

$0.1\ M\ AgNO_3$

$0.01\ M\ KI$

$0.1\ M\ KI$

$10^{-12}\ M$

$10^{-2}\ M$

$12\ M$

$10^{12}\ M$

$HA \rightarrow H^+ + A^-$

$HA \rightleftharpoons H^+ + A^-$

$H^+ + A^- \rightarrow HA$

$HA + H_2O \rightarrow H_3O + A$

$H_2O$

$AlCl_3$

$NH_3$

$CH_4$

Weakly acidic

Strongly acidic

Weakly basic

Strongly basic

-5

5

10

1

1

2

3

4

$NH_3$

$NH_2^-$

$NH_5^{2+}$

$N_2$

Weak

Strong

Neutral

Unpredictable

$NH_4OH + NH_4Cl$

$H_2S + HCl$

$NaOH + NaCl$

$CH_3COOH + CH_3COONa$

Its $pH$ does not change on standing

Its $pH$ does not change on dilution

Its $pH$ changes drastically on adding a small amount of strong acid

It has a definite $pH$ value

To provide a high concentration of the conjugate base

To neutralize the weak acid

To make the solution acidic

To increase the $pKa$ of the acid

$Q_{sp} < K_{sp}$

$Q_{sp} > K_{sp}$

$Q_{sp} = K_{sp}$

The salt is highly soluble

$K_{sp} = 27s^4$

$K_{sp} = 3s^4$

$K_{sp} = s^4$

$K_{sp} = 9s^3$

$3.2 \times 10^{-11}$

$4 \times 10^{-8}$

$1.6 \times 10^{-11}$

$8 \times 10^{-12}$