IPS1- B4- Ionic Equilbria

Ionization

___- is a chemical process in which a neutral molecule forms new ions when dissolved in water.

Ionization

____ -

• is a chemical process is when the subtance was not made of ions originally but reacts with water to form ions.

  • New charged particles are produced

a. Ionization

HCl + H2O → H3O+ + Cl−

a. Ionization

b. Dissociation

a. Ionization

neutral substance + water = new ion (charge particle)

a. Ionization

b. Dissociation

a. Ionization

Common with acids and weak bases

a. Ionization

b. Dissociation

Dissociation

____ - is a physical process where an ionic compound separates into its pre-existing ions in solution

b. Dissociation

NaCl → Na+ + Cl−

a. Ionization

b. Dissociation

b. Dissociation

No new ions are formed, just a separation of existing ones.

a. Ionization

b. Dissociation

b. Dissociation

Common with salts and strong bases

a. Ionization

b. Dissociation

base

An acid must have a _____ present in order to function as an acid, and vice versa.

• Arrhenius

• Bronsted-Lowry

• Lewis

Acid Base Theories [3]

Arrhenius

[Acid Base Theories]

____-

• all bout H⁺ and OH

Bronsted Lowry

[Acid Base Theories]

____-

• about proton

Lewis

[Acid Base Theories]

___-

• about electron

• proton donor

• proton acceptor

►Bronsted Lowry acid is a ____ [proton donor/ proton acceptor]

►Bronsted Lowry base is a____ [proton donor/ proton acceptor]

• electron acceptor

• electron donor

►Lewis acid is a ____ [ electron donor/ proton acceptor]

►Lewis base is a____ [ electron donor/ proton acceptor]

Conjugate Acid and Base

partial ionization

Weak acid/Weak base = ____ [partial ionization / complete ionization] in water

complete ionization

Strong acid/Strong base = ____ [partial ionization / complete ionization] in water

• strong acid

• weak acid

►large Ka = ___ [weak/strong] acid

►small Ka= ___ [weak/strong] acid

1 × 10¹⁴

Acid dissociation constant of water (Kw) at 25 °C is ___ ?

autoprotolysis

___- is a process where water react with its own water molecule

autoprotolysis

____ - is a chemical process where a substance acts as both an acid and a base at the same time

autoprotolysis

Water undergoes _____ [what process] to produce ions

a. Monoprotic

one proton transfer

a. Monoprotic

b. Polyprotic

a. Monoprotic

Acetic acid (HAc) with one Ka

a. Monoprotic

b. Polyprotic

b. Polyprotic

Multiple protons

a. Monoprotic

b. Polyprotic

• Diprotic

• Triprotic

Types of Polyprotic [2]

a. Diprotic

Carbonic acid (H2CO3) is an example of what Type of Polyptoric electrolyte

a. Diprotic

b. Triprotic

a. Diprotic

Sulfuric acid (H₂SO₄) is an example of what Type of Polyptoric electrolyte

a. Diprotic

b. Triprotic

b. Triprotic

Phosphoric acid (H₃PO₄) has three Ka values is an example of what Type of Polyptoric electrolyte

a. Diprotic

b. Triprotic

• two Ka values

• three Ka values

• Carbonic acid (H₂CO₃) has ___ Ka values

• Phosphoric acid (H₃PO₄) has ___ Ka values

Ampholytes (Amphoteric electrolyte)

[KIND OF ELECTROLYTE] ____ - can function as an acid /base

Ampholytes

[KIND OF ELECTROLYTE] ____- are species that can functions either as an acid or as a base

True

[T/F] Ampholytes are amphoteric in nature

• Amino acid

• Proteins

Example of ampholytes [2]

a. Ampholyte

Amino acids and proteins are the classic example of

a. Ampholyte

b. Pedialyte

c. Ionization

d. hydrite

Zwitterion

[Kind of Ion] ____ - have both positive and negative charges

Amino acid

____ -

• is a zwitterion

• basic unit of protein

Sorensen

Ph scale is by ____ [who]?

• acidic

• neutral

• basic /alkaline

• pH <7 = ___ ?

• pH = 7 = ___ ?

• pH > 7 = ____ ?

a. 0-14

pH and pOH lie between ____?

a. 0-14

b. 0-12

c.1-5

d.2-20

• low pH

• higher pOH

• higher pOH

• Higher H = __ [high/low] Ph

• Higher H = __ [high/low] pOH

• Lower pH = Higher H = __ [high/low] pOH

the more acidic the substance is

• low pOH

• high pH

• high pH

• high OH = __ [high/low] pOH

• high OH = __ [high/low] pH

• low pOH = high OH = __ [high/low] pH

the more basic the substance is

• HI (Hydroiodic acid)

• HBr (Hydrobromic acid)

• HCl (Hydrochloric acid)

• HNO₃ (Nitric acid)

• HClO₄ (Perchloric acid)

• H₂SO₄ (Sulfuric acid, diprotic)

Strong acid [5]

• LiOH – Lithium hydroxide

• NaOH – Sodium hydroxide

• KOH – Potassium hydroxide

• Ca(OH)₂ – Calcium hydroxide

• CsOH – Cesium hydroxide

• RbOH – Rubidium hydroxide

• Sr(OH)₂ – Strontium hydroxide

• Ba(OH)₂ – Barium hydroxide

Strong bases [8]