IPS1 - B1-B3- Overview of dispersed system ➡️ Solubility Phenomena

Proverbs 16:3

System

____- is a bounded space of an exact quantity of a material

Dispersion

____ - consist of at least two phases with one or more dispersed phase (internal) contained in a single continuous (external) phase

• dispersed phase

• single continuous phase (dispersion medium)

Dispersion consists of at least two phases such as ___ [2]

internal phase

In Dispersion

• dispersed phase is our ____ [internal/extenal phase]

external phase

In Dispersion

• single continuous phase is our ____ [internal/extenal phase]

external or continuous phase

Dispesion medium is the ____ [internal/extenal phase]

Phase

____ - is a distinct homogenous part of a system

• Molecular dispersion

• Colloidal dipersion

• Coarse dispersion

Types of Dispersion [3]

Molecular dispersion

[Types of Dispersion]

____-

• A.k.a. True Solutions (one phase)

• is a HOMOGENEOUS SYSTEM

• Diameter of particles <1 nm

one phase

True solution have _____ [how many] phase ?

Colloidal dispersion

[Types of Dispersion]

____-

• Diameter of particles 1 to 500 nm

• is a HETEROGENEOUS SYSTEM

b.) Colloidal dispersion

Gelatin, milk is an example of what type of dispersion ?

a.) Molecular dispersion

b.) Colloidal dispersion

c.) Coarse dispersion

Coarse dispersion

[Types of Dispersion]

____-

• diameter of particles > 500 nm

c.) Coarse dispersion

emulsions and suspension is an example of what type of dispersion ?

a.) Molecular dispersion

b.) Colloidal dispersion

c.) Coarse dispersion

Molecular Dispersion

True solution is aka ___ ?

a.) True solution (Molecular Dispersion)

Binary Solution is what kind of solution?

a.) True solution

b.) Simple solution

Binary solutions

_____ - is a true solution (molecular dispersion) that is composed of only two substances

True solutions (Molecular dispersion)

____- is a mixture of two or more components that form a homogenous molecular dispersion or one-phase system

a.) < 1 nm

What is the particle size of true solution (molecular dispersion) ?

a.) < 1 nm

b.) 0.5 nm

c.) > 2nm

• Solute – lesser amount

• Solvent – greater amount

Components/Constituents of True Solution (Molecular Dispersion) such as ___ [2]

a.) Solute

Components/Constituents of True Solution that have lesser amt ?

a.) Solute

b.) Solvent

b.) Solvent

Components/Constituents of True Solution that have greater amt ?

a.) Solute

b.) Solvent

Example of Solute + Solvent = Product

ANALYZE MO LNG

b.) Nitrogen

What is the most abundant gas in air

a.) Oxygen

b.) Nitrogen

C. Carbon dioxide

• Non- electrolytes

• Electrolytes

Types of Solute [2]

b.) non electrolyte

[Classify the Type of Solute]

____ -

• Do not ionize in water

a.) electrolyte

b.) non electrolyte

a.) electrolyte

[Classify the Type of Solute]

• Ionize in water (form ions)

a.) electrolyte

b.) non electrolyte

b.) non electrolyte

[Classify the Type of Solute]

• Do not conduct electric current

a.) electrolyte

b.) non electrolyte

a.) electrolyte

[Classify the Type of Solute]

• Conduct electric current

a.) electrolyte

b.) non electrolyte

b.) non electrolyte

[Classify the Type of Solute]

• Sucrose, glycerin, naphthalene, urea

a.) electrolyte

b.) non electrolyte

a.) monoclinic

What is the shape of SUCROSE ?

a.) monoclinic

b.) tetragonal

c.) trigonal planar

b.) tetragonal

What is the shape of UREA ?

a.) monoclinic

b.) tetragonal

c.) trigonal planar

Alcohol ( specifically: Trihydric alcohol )

____ - is the functional group of GLYCERIN

a.) electrolyte

[Classify the Type of Solute]

• HCl, NaCl

a.) electrolyte

b.) non electrolyte

a.) electrolyte

[Classify the Type of Solute]

• Atropine, phenobarbital, sulfadiazine

a.) electrolyte

b.) non electrolyte

• Protophilic (Basic)

• Protogenic (Acidic)

• Amphiprotic

• Aprotic

Types of Solvent [4]

a.) Protophilic or Basic

[Classify the Type of Solvent]

• Proton-accepting

a.) Protophilic or Basic

b.) Protogenic or Acidic

c.) Amphiprotic

d.) Aprotic

a.) Protophilic or Basic

[Classify the Type of Solvent]

• Acetone, ether, and liquid ammonia

a.) Protophilic or Basic

b.) Protogenic or Acidic

c.) Amphiprotic

d.) Aprotic

b.) Protogenic or Acid

[Classify the Type of Solvent]

• Proton-donating

a.) Protophilic or Basic

b.) Protogenic or Acid

c.) Amphiprotic

d.) Aprotic

b.) Protogenic or Acid

[Classify the Type of Solvent]

• formic acid, acetic acid, sulfuric acid, liquid HCl, and liquid HF

a.) Protophilic or Basic

b.) Protogenic

c.) Amphiprotic

d.) Aprotic

c.) Amphiprotic

[Classify the Type of Solvent]

• Act as both acid and base

a.) Protophilic or Basic

b.) Protogenic or Acid

c.) Amphiprotic

d.) Aprotic

c.) Amphiprotic

[Classify the Type of Solvent]

• water and alcohol

a.) Protophilic or Basic

b.) Protogenic

c.) Amphiprotic

d.) Aprotic

d.) Aprotic

[Classify the Type of Solvent]

• Neither accept nor donate protons

• neutral

a.) Protophilic or Basic

b.) Protogenic

c.) Amphiprotic

d.) Aprotic

d.) Aprotic

[Classify the Type of Solvent]

• Hydrocarbon

a.) Protophilic or Basic

b.) Protogenic

c.) Amphiprotic

d.) Aprotic

Concentration Expressions

____- are expressions of

• quantity of solute/volume of solution

• quantity of solute/mass of solvent or solution

Normality (N)

____- is the gram-equivalent weight per liter of solution ( UNIT:mEq/mL or Eqwt / L )

Solubility

____ - quantitatively is the concentration of solute in saturated solution at a certain temperature

Solubility

____ - qualitatively is the spontaneous interaction of two or more substances to form homogenous molecular dispersion

• Saturated Solutions

• Unsaturated Solutions

• Supersaturated Solutions

Types of Solutions [3]

a. Saturated solution

[Classify the Types of Solution]

• Solute in a solution is in equilibrium with the solid phase

a. Saturated solution

b. Unsaturated solution

c. Supersaturated solution

b. Unsaturated solution

[Classify the Types of Solution]

• Solute concentration < saturation point

a. Saturated solution

b. Unsaturated solution

c. Supersaturated solution

c. Supersaturated solution

[Classify the Types of Solution]

• Solute concentration > saturation point

• Undissolved solutes are present

• is a HOMOGENEOUS SYSTEM

a. Saturated solution

b. Unsaturated solution

c. Supersaturated solution

Dissolution

____ - is the transfer of molecules / ions from a solid state into solution

Dissolution

____ - is when the solute dissolves in a solution

Solubility

_____- is the extent of dissolution

1g/mL of solute in solvent

What is the Part of Solvent Required for One part of solute?

a. 1g/mL of solute in solvent

b. 3g/mL of solute in solvent

c. 4g/mL of solute in solvent

d. 10g/mL of solute in solvent

mg/mL or g/L

Solubility Range units

True

[T/F] The greater the similarity between the solute and the solvent (similar physicalchemical properties), the greater the solubility.

Like dissolves like principle

According to ____ principle

• The greater the similarity between the solute and the solvent (similar physical/chemical properties), the greater the solubility

polarity of solvent (dipole moment)

Solubility of drug is due to the large measure to the _____ ?

• Dipole moment

• Form H-bond

• Short chain

• > 4C or 5C

• Increase Branching

Polarity involves [5]

a. Polar Solvent

Polar solvent + Ionic solute or Polar solutes

a. Polar Solvent

b. Non Polar Solvent

• Phenols

• Alcohols

• Aldehyde

• Amines

Except: ether and ketone

Functional Groups that forms H-bond [4]

Mnemonic : PAAA

a. Hydrogen Bond

Phenols , Alcohols , Aldehyde , Amines functional groups that forms

a. Hydrogen Bond

b. Ionic Bond

c. Covalent Bond

less water soluble

Longer Chain = ____ [more/less] water soluble

> 4C or 5C

Straight chain monohydroxy Alcohol (ROH), Aldehyde (RCHO), Carboxylic Acid (RCOOH) have ____ [how many] Carbons ?

slightly water soluble

> 4C or 5C = ____ [more/less/slightly] water soluble

more water soluble

Increase Branching = ____ [more/less] water soluble

b. Non Polar Solvent

Non-polar Solutes + Non-polar Solvents

a. Polar Solvent

b. Non Polar Solvent

b. Induce dipole

Non-polar Solvents is due to the ___ ?
a. Dipole moment

b. Induce dipole

• Benzene

• Carbon tetrachloride (CCI₄)

• Mineral Oil

Example of Nonpolar Solvents [3]

b. Non Polar Solvent

[Classify the Type of Solvent]

• Oils and Fats are soluble in Carbon tetrachloride (CCI₄), benzene, mineral oil

a. Polar Solvent

b. Non Polar Solvent

c. Semipolar Solvent

[Classify the Type of Solvent]

• Can induce a certain polarity in nonpolar solvents

a. Polar Solvent

b. Non Polar Solvent

c. Semipolar Solvent

• ketone (e.g. acetone)

• alcohol

Example of Semipolar Solvent [2]

c. Semipolar Solvent

[Classify the Type of Solvent]

• ketone and alcohol

a. Polar Solvent

b. Non Polar Solvent

c. Semipolar Solvent

c. Semipolar Solvent

[Classify the Type of Solvent]

• Can act as intermediate solvents

a. Polar Solvent

b. Non Polar Solvent

c. Semipolar Solvent

c. Semipolar Solvent

Acetone, Alcohol, Propylene glycol are Example

a. Polar Solvent

b. Non Polar Solvent

c. Semipolar Solvent

• Acetone

• Alcohol

• Propylene glycol

____ [3] can act as intermediate solvent

Acetone

[What Intermediate/Semi-Polar Solvent ]

• ___- increases the solubility of ether in water

Alcohol

[What Intermediate/Semi-Polar Solvent ]

• ___- increases miscibility of the water-castor oil mixture

Propylene glycol

[What Intermediate/Semi-Polar Solvent ]

• ___- increases miscibility of: ⏬

  • water and peppermint oil

  • water and benzyl benzoate

Propanol

____ - acts as a co-solvent of hexane and water

1. Dielectric constant

2. Presence of Salts

2. Effect of temperature

3. Effect of pH

5. Effect of Particle Size

Factors affecting solubility [5]

Dielectric constant

____- is a quantitiy measure the ability of substance to store electrical energy in electric field.

decrease polarity

Low dielectric constant = ___ [increase/decrease] polarity

decrease water solubility

Low dielectric constant = ___ [increase/decrease] water solubility

increase solubility

Increase Temperature = ____ [increase/decrease] solubility

increase KE

Increase Temperature ____ [increase/decrease] KE

increase solubility

Increase KE = ____[increase/decrease] solubility

a. Endothermic

Heat is absorbed

a. Endothermic

b. Exothermic

b. Exothermic

Heat is released

a. Endothermic

b. Exothermic

a. Endothermic

Potassium nitrate (KNO₃), Potassium chloride (KCl) are common example of what reaction ?

a. Endothermic

b. Exothermic

b. Exothermic

Sodium sulfate (Na₂SO₄₎ , Calcium hydroxide (Ca(OH)₂)are example of what reaction ?

a. Endothermic

b. Exothermic

Calcium Hydroxide (Ca(OH))

____- is the most common example of substance that undergo Exothermic Reaction

increase solubility

For endothermic substance

• increase temperature = ____[increase/decrease] solubility

decrease solubility

For exothermic substance:

• increase temperature = ____[increase/decrease] solubility

improve solubility

Acid + Basic = ___ [improve/reduce] solubility

decrease solubility

Acidic Drugs + Acid (low pH) = ____ [increase/decrease] solubility

decrease solubility

Basic Drugs + Base (high pH) = ____ [increase/decrease] solubility

soluble

Phenobarbital (weak acid) + high pH (base) = ____ [soluble / insoluble]