Chemistry Equilibrium and Acid-Base Practice Flashcards

Vocabulary terms and definitions covering chemical equilibrium, Le Ch%telier's principle, and acid-base chemistry including pH, Ka/Kb, and salt properties.

Q < K

The reaction shifts right (toward products).

Q > K

The reaction shifts left (toward reactants).

Q = K

The reaction is at equilibrium.

K > 1

The side favored is the products.

K < 1

The side favored is the reactants.

Adding a reactant

Equilibrium shifts to the right.

Adding a product

Equilibrium shifts to the left.

Removing a reactant

Equilibrium shifts to the left.

Removing a product

Equilibrium shifts to the right.

Catalyst effect on equilibrium

Results in no shift.

Increasing pressure shift

Shifts equilibrium toward the side with fewer moles of gas.

Decreasing pressure shift

Shifts equilibrium toward the side with more moles of gas.

Arrhenius acid

Produces $H^+$ in water.

Arrhenius base

Produces $OH^-$ in water.

Br%nsted-Lowry acid

Proton donor.

Br%nsted-Lowry base

Proton acceptor.

Lewis acid

Electron pair acceptor.

Lewis base

Electron pair donor.

Acid-to-Conjugate Base Transition

Occurs when an acid loses $H^+$.

Base-to-Conjugate Acid Transition

Occurs when a base gains $H^+$.

Conjugate base of HCl

$$Cl^-$$

Conjugate acid of $NH_3$

$$NH_4^+$$

Kw at $25\,^{\circ}C$

$$1.0 \times 10^{-14}$$

pH Formula

$$pH = -\log[H_3O^+]$$

pOH Formula

$$pOH = -\log[OH^-]$$

Relationship between pH and pOH

$$pH + pOH = 14$$

Neutral solution pH

7

Acidic solution pH

Less than 7.

Basic solution pH

Greater than 7.

Large Ka

Indicates a stronger acid.

Small Ka

Indicates a weaker acid.

Large Kb

Indicates a stronger base.

pKa

A measure of acid strength where a smaller value indicates a stronger acid.

pKb

A measure of base strength where a smaller value indicates a stronger base.

Percent Ionization Formula

$$(\text{ionized amount} \div \text{initial concentration}) \times 100$$

Strong acid percent ionization

High.

Weak acid percent ionization

Low.

ARIO

Atom, Resonance, Induction, Orbital.

Charge resonance stability

A charge with resonance is more stable than one without resonance.

Conjugate base stability effect

A more stable conjugate base means a stronger acid.

Electron-withdrawing atoms effect

Atoms like F or Cl make an acid stronger.

Strong acid + strong base salt

Neutral salt.

Strong acid + weak base salt

Acidic salt.

Weak acid + strong base salt

Basic salt.

NaCl salinity property

Neutral.

NH₄Cl salinity property

Acidic.

NaF salinity property

Basic.

Polyprotic acid

An acid that can donate more than one proton ($H^+$).

Ka1 vs Ka2

$K_{a1}$ is usually the largest.

Lewis acid in $NH_3 + BF_3$

$$BF_3$$

Lewis base in $NH_3 + BF_3$

$$NH_3$$