Chem CH 15 Acids and Bases

Acid Properties

H, bonded to non metal, H+, positively charged

Base Properties

OH, H-, bonded to metal, negatively charged

Bronsted Lowry Base

proton acceptor

Bronsted Lowry Acid

proton donor

Conjugate acid-base pair

the resulting acid and anion that comes from the lost proton

Strong acids/bases

acids/bases that completely dissociate in water

Weak acids/bases

acids/bases that exist at equilibrium

Rules for Strong Acid

1. Completely dissociate in water

2. Produce H+ (or H3O+) ions

3. Common examples: HCl, HNO3, H2SO4

Rules for Strong Base

1. Completely dissociate in water

2. Produce OH- ions

3. Common examples: NaOH, KOH, Ca(OH)2

Percent ionization

way to determine the strength of an acid. (ionized acid concentration / initial concentration of acid ) x 100%

dissociation

To write the dissociation equation for an acid or base, follow these steps:

1. Identify if it's an acid or a base:

- Acids typically start with H (e.g., HCl, CH3COOH)

- Bases often end with OH (e.g., NaOH) or contain nitrogen (e.g., NH3)

2. For acids:

- Write the acid molecule on the left side

- Add H2O if it's a weak acid

- On the right side, show the acid splitting into H+ (or H3O+ if you included water) and the remaining ion

3. For bases:

- Write the base molecule on the left side

- Add H2O for weak bases

- On the right side, show the formation of OH- and the remaining ion

4. Use the correct arrow:

- For strong acids/bases, use a single arrow (→)

- For weak acids/bases, use a double arrow (⇌)

Examples:

1. Strong acid (HCl):

HCl → H+ + Cl-

or

HCl + H2O → H3O+ + Cl-

2. Weak acid (CH3COOH):

CH3COOH + H2O ⇌ H3O+ + CH3COO-

3. Strong base (NaOH):

NaOH → Na+ + OH-

4. Weak base (NH3):

NH3 + H2O ⇌ NH4+ + OH-

Remember, the dissociation equation is crucial for setting up ICE tables and solving equilibrium problems for acids and bases.

Citations:

[1] https://ppl-ai-file-upload.s3.amazonaws.com/web/direct-files/25647384/286ea4fe-eaac-4d2c-bd0d-6d3ee28a003c/Acids-and-Bases.pdf

bond stregth

(how many kJ it takes to break the bond)

Carboxylic acids

the most common organic acids

are three possible outcomes to the overall pH of the solution when salt is dissolved? (salt hydrolysis)

Nothing—these are neutral salts • Neutral salts are not exciting, they are the conjugate bases/acids of strong acids/bases (so sodium, chloride, nitrates, hydrogen sulfate etc.) • Basic salts—these increase the pH • Acidic salts—these decrease the pH

Lewis base

electron pair donor

Lewis acid

electron pair acceptor