IN THE NAME OF ALLAH THE MOST GRACIOUS, THE MOST MERCIFUL

CHEM 122. LEVEL-2 LECTURE # 1 CHAPTER 8 - SOLUTIONS

RCDPRCDP

Chemistry by Timberlake Chemistry by Timberlake p.226p.226

Presented by:Presented by:

Department OfDepartment Of

ChemistryChemistry

• Types of mixtures

1- Solution2- Colloidal solution/dispersion3-Suspension

It is a homogeneous mixture of two or more substances.

One substance which is called the solute is uniformly dispersed in another substance called the solvent.

Every part of the solution possesses the same composition, density, viscosity.

Example: Sugar in water

1- True solution:

Solvent:The component present in larger amount in

solution. Solute:The component present in smaller amount

in solution (in lesser amount).

Solubility:Maximum amount of solute dissolved in a

fixed quantity of solvent ( 100g) at a given temperature to form a saturated solution.

TYPES of SOLUTIONS:Three States of matter :

GAS LIQUID

SOLID

Types of solutions (7):

1) A solution of gas in gas, example air (O2 gas in N2 gas)

2) A solution of gas in liquid, example aerated water such as soda water (CO2 in water)

3) A solution of gas in solid , example hydrogen in palladium (Pd)

4) A solution of liquid in liquid, example Benzene in toluene.

5) A solution of liquid in solid, example Amalgamated zinc (mercury in zinc)

6) A solution of solid in liquid, example seawater (NaCl in water).

7) A solution of solid in solid, Alloys, example Cu in Au (gold) and brass (zinc in copper).

Type of solution Example Components of solution

gas/gas air O2 gas and N2 gas

gas/liquid soda CO2 gas in water

solid/liquid seawater NaCl in water

solid/solid brass zinc and copper

It is a homogeneous mixture of two or more substances, where the solute,

1-May spread evenly throughout the solution.

2-Cannot be separated by filtration.

3-Can be separated by evaporation.

4-Is not visible, solution appears transparent

5-May give a color to the solution.

•Properties of solution :

Q1: Identify the element (1),

compound (2) or solution (3) :

A. water

B. sugar

C. salt water

D. air

E. tea

Q2- Identify the solute in each of the following solutions:

a) 2 g sugar + 100 mL water

b) 60.0 mL ethyl alcohol + 30.0 mL

of methyl alcohol

c) 55.0 mL water + 1.50 g NaCl

d) Air: 200 mL O2 + 800 mL N2

e) brass: 20 g zinc + 50 g copper

f) 100 g H2O + 5 g KCl

•Factors influencing solubility:

1-Temperature: (A) If the formation of solution is endothermic

then the solubility increases with the increase in temperature.heat + solute + solution (1) ⇌ solution (2)

(B) If the formation of solution is exothermic then solubility decreases with the increase in temperature. gas + solution (1) ⇌ solution (2) + heat

Example :Solubility of gases are exothermic. Gases are less soluble at higher temperatures

2-Pressure :Solubility of gases increases with increasing pressure.

Henry’s Law: The solubility of a gas in a liquid solution is directly proportional to the pressure of the gas above the solution.

3-Common ion effect:

Solubility of AgCl decreases in the solution of NaCl compared to the solubility of AgCl in pure water.

This is because of the chloride ion which is

a common ion.

Types of solutions according to solute concentration:

Saturated solution:Solution contains maximum amount of

solute at a given temperature and pressure

Unsaturated solution:Solution contains less than the maximum

quantity of solute, or if the solution is not saturated.

Dilute solution:Quantity of solute is very less in solution.

Types of mixtures(cont.)

2- Colloidal solutions/ dispersions: -These are heterogeneous (non-uniform

mixtures.)

-In colloidal dispersion, the size of the solute molecules are intermediate between the size of solute molecules in true solution and those in suspension.Range of size 1 to 1000nm Example, Milk, Butter in H2O

Properties of Colloids

Have medium size particles, that do not settle

out (separate).

Particles cannot be filtered (particles are

small enough to be pass through filters).

Can be separated with semi permeable

membranes (particles are too large to pass

through semi permeable membranes).

Scatter light (Tyndall effect)

Examples of Colloids

Fog, clouds (liquid in gas)

Whipped cream (gas in liquid)

Homogenized Milk (liquid in liquid)

Cheese (liquid in solid)

Blood plasma (solid in liquid)

Pearls (solid in solid)

3- SUSPENSIONS: These are heterogeneous non-uniform

mixtures.

Properties of Suspensions

Have very large particles (can be seen by eye)

Settle out

Can be filtered

Must be stirred to stay suspended

N.B:

It is important to “Shake well before using” before giving a suspension medication.

Examples of Suspensions

Blood platelets Muddy water Calamine lotion

(Homogeneous) (Heterogeneous) Solution Colloid Suspension - small particles - intermediate particles - large particles < 1 nm bet. 1-1000 nm >1000 nm - does not separate - does not separate - separates on standing over time over time

- cannot be filtered - cannot be filtered - can be filtered (can be separated with semi permeable membranes)

- no Tyndall Effect -Tyndall Effect present -Tyndall Effect present

- e.g.: salt/H20 - e.g.: milk, gel, smoke, - e.g.: clay/water , foam Italian salad dressing

Comparison:

Polar and non polar solvents:• Some substances are soluble in one

solvent but not in another solvent. • This is due to the polar and non polar

nature of solvent. • Example: Sugar is soluble in water but

not in petrol. • Alcohol and water are completely

miscible in each other, this is due to the hydrogen bonding.

• Two non polar substances are miscible

(Hexane in Carbon tetrachloride).

Miscible: Fluids that completely dissolve in each other.

Non-polar C6H14 will not dissolve in polar H2O. Non-polar C6H14 will dissolve in non-polar CCl4.

“ Like dissolves like ” General rule for solutions is “like dissolves like.”

Polar dissolves polar & non-polar dissolves non-polar.

Examples: I2 is soluble in CCl4 & relatively insoluble in

water NaCl is soluble in water but not in non polar

solvents. Polar molecule like CH3OH will dissolve as a

molecule in polar H2O. Ionic LiF will dissolve as ions in polar H2O.

Solvation and hydration: Polar solutes dissolve in polar solvents. Ionic substances furnish cations (+) and anions

( - ). These ions are surrounded by solvent molecules

this is known as solvation and if the solvent is water then it is called hydration. Example NaCl in water.

Cl-

Na+ Cl-Na+

H2O

H2O

Na+

Cl-

solute

Dissolvedsolute

Hydration

When NaCl(s) dissolves in water, the reaction can be written as

NaCl(s) H2O Na+ (aq)+Cl(aq) solid separation of ions in water

Q1: Solid LiCl is added to some water. It dissolves becauseA. The Li+ ions are attracted to the 1) oxygen atom(-) of water 2) hydrogen atom(+) of water

B. The Cl- ions are attracted to the 1) oxygen atom(-) of water 2) hydrogen atom(+) of water

Answer: Solid LiCl is added to some water.

It dissolves becauseA. The Li+ ions are attracted to the 1) oxygen atom(-) of water B. The Cl- ions are attracted to the 2) hydrogen atom(+) of water

Q2: Like dissolves like

A ____________ solvent such as water is

needed to dissolve polar solutes such as

sugar and ionic solutes such as NaCl.

A ___________solvent such as hexane

(C6H14) is needed to dissolve nonpolar

solutes such as oil or grease.

Q3:Which of the following solutes will dissolve in water? Why?

1) Na2SO4

2) gasoline

3) I2

4) HCl

Answer:

1) Na2SO4 Yes, polar

(ionic)

2) gasoline No, nonnpolar

3) I2 No, nonpolar

4) HCl Yes, Polar

Spectator ion:Two ionic compounds NaCl and AgNO3 in water exist as Na+, Cl- and Ag+, (NO3)

- ,ions

and react with each other Ag+

aq + NO3 aq + Na+aq + Cl-

aq → AgCl s↓ + Na+aq+ NO3 aq

This equation is called ionic equation.

In this reaction Na+ and NO3 ions do not change during a reaction are called spectator ions.They are the same before and after the reaction.

Ag+aq + NO3 aq + Na+

aq + Cl-aq → AgCl s↓ + Na+

aq+ NO3 aq

while writing an ionic equation we can omit the spectator ions.

This equation is known as net ionic equation

Ag+aq + NO3 aq + Na+

aq + Cl-aq → AgCl s↓ + Na+

aq+ NO3

aq

Ag+aq + Cl-aq → AgCl↓ ( net ionic equation )

Another example:Another example:

AgF AgF aq aq + KCl + KCl aq aq → AgCl → AgCl s s +KF +KF aqaq –– molecularmolecular equationequation

AgAg++aq + Faq + F--aq + Kaq + K++aq + Claq + Cl--aq → AgCl ↓ + Kaq → AgCl ↓ + K++ + + FF-- ------ionicionic equation equation

AgAg++aq + Claq + Cl--aq → AgCl ↓aq → AgCl ↓ ------net ionicnet ionic equationequation

PCDPR-CHEM.122 LEVEL 2MCQz

Q1. Indicate solution among the following:A). Water b) salt-water c) air d) both b & cQ2. Brass is an alloy of 20 g zinc + 50g

copper. Identify the solute:A). 20 g zinc b) 50g copper c) both a & b d) none of the aboveQ3. Identify solvent in 55ml water & 2g

NaClA). 55ml water b) 2g NaClc) both a & b d) none of the above

Q4.Solubility of gases increases with rise in:

A). Pressure b) temperature c) both a &b d) none of the above

Q5. The process in which water is taken as solvent is called:

A). solvation b) hydrationc) evaporation d) condensation

Q6. Iodine I2 is soluble in CCl4:A) True b) False

Q7.Polar or ionic solutes are dissolved in:A). Polar solvents b) non Polar solventsc) Polar solutes d) non Polar solutes

Q8. Which solute will dissolve in water?A) Na2SO4 b) gasoline c) I2 d) Hexane