Solutions Class 12th P.C Flashcards by Aishwarya Rathi

What is a solution?

A homogeneous mixture of two or more components.

How well did you know this?

Not at all

Perfectly

What are the components of a solution?

Solvent and Solute.

How well did you know this?

Not at all

Perfectly

Define solvent

Component present in larger amount.

How well did you know this?

Not at all

Perfectly

Define solute

Component present in smaller amount.

How well did you know this?

Not at all

Perfectly

Define solubility

Maximum amount of solute dissolved in given solvent at given temperature.

How well did you know this?

Not at all

Perfectly

What is a saturated solution?

Solution containing maximum solute dissolved at given temperature.

How well did you know this?

Not at all

Perfectly

What is an unsaturated solution?

Solution that can dissolve more solute.

How well did you know this?

Not at all

Perfectly

What is a supersaturated solution?

Solution containing more solute than saturated solution.

How well did you know this?

Not at all

Perfectly

Example of solid in solid solution?

Alloys like brass.

How well did you know this?

Not at all

Perfectly

Example of gas in liquid solution?

CO2 in soda water.

How well did you know this?

Not at all

Perfectly

Example of liquid in liquid solution?

Alcohol in water.

How well did you know this?

Not at all

Perfectly

Define concentration of solution

Amount of solute in given amount of solution.

How well did you know this?

Not at all

Perfectly

Mass percentage formula

(Mass of solute / Mass of solution) × 100

How well did you know this?

Not at all

Perfectly

Volume percentage formula

(Volume of solute / Volume of solution) × 100

How well did you know this?

Not at all

Perfectly

Mass by volume percentage

(Mass of solute / Volume of solution) × 100

How well did you know this?

Not at all

Perfectly

Define ppm

Parts per million concentration unit.

How well did you know this?

Not at all

Perfectly

ppm formula

(Mass of solute / Mass of solution) × 10^6

How well did you know this?

Not at all

Perfectly

Where ppm is used?

Very dilute solutions.

How well did you know this?

Not at all

Perfectly

Define mole fraction

Moles of component divided by total moles.

How well did you know this?

Not at all

Perfectly

Sum of mole fractions equals?

How well did you know this?

Not at all

Perfectly

Define molarity

Moles of solute per liter of solution.

How well did you know this?

Not at all

Perfectly

Molarity formula

M = n / V

How well did you know this?

Not at all

Perfectly

Define molality

Moles of solute per kg of solvent.

How well did you know this?

Not at all

Perfectly

Molality formula

m = n / mass of solvent in kg.

How well did you know this?

Not at all

Perfectly

Which concentration unit is temperature independent?

Molality.

Why molarity depends on temperature?

Volume changes with temperature.

Relation between molarity and molality?

Conversion requires density.

Define Henry's Law

Solubility of gas proportional to pressure.

Henry law formula

p = kH x

Effect of pressure on gas solubility?

Solubility increases.

Effect of temperature on gas solubility?

Solubility decreases.

Example of Henry law?

Cold drink bottles.

Define Raoult's Law

Partial pressure proportional to mole fraction.

Raoult law formula

PA = XA PA°

Total vapour pressure formula

Ptotal = XA PA° + XB PB°

Define ideal solution

Solution obeying Raoult law at all compositions.

Conditions for ideal solution

ΔHmix = 0 and ΔVmix = 0

Example ideal solution

Benzene and Toluene.

Define non-ideal solution

Solution not obeying Raoult law.

Positive deviation meaning

Higher vapour pressure than expected.

Negative deviation meaning

Lower vapour pressure than expected.

Cause of positive deviation

Weaker intermolecular forces.

Cause of negative deviation

Stronger intermolecular forces.

Example positive deviation

Ethanol + Acetone.

Example negative deviation

Acetone + Chloroform.

Define azeotrope

Constant boiling mixture.

Minimum boiling azeotrope example

Ethanol + Water.

Maximum boiling azeotrope example

Nitric acid + Water.

Define colligative properties

Depend only on number of particles.

Name colligative properties

RLVP Elevation BP Depression FP Osmotic pressure.

Relative lowering vapour pressure formula

(P° − P)/P° = Xsolute

Elevation of boiling point formula

ΔTb = Kb m

Depression of freezing point formula

ΔTf = Kf m

Osmotic pressure formula

π = CRT

Define osmosis

Flow of solvent through semipermeable membrane.

Define osmotic pressure

Pressure to stop osmosis.

Define reverse osmosis

Applying pressure to reverse osmosis.

Application reverse osmosis

Water purification.

Define van't Hoff factor

i = observed / calculated colligative property.

i greater than 1 indicates

Dissociation.

i less than 1 indicates

Association.

i for NaCl

i for CaCl2

i for AlCl3

Why abnormal molar mass occurs?

Association or dissociation.

Acetic acid in benzene shows what?

Association.

Relation molar mass and colligative property

Inverse relation.

Which property used for polymers?

Osmotic pressure.

Unit of Kb

K kg mol^-1

Unit of Kf

K kg mol^-1

Unit of osmotic pressure

atm or Pa.

Boiling point increases due to

Vapour pressure lowering.

Freezing point decreases due to

Solid formation hindered.

Electrolytes effect on colligative properties

Increase effect.

Non-electrolytes effect

Normal effect.

Semipermeable membrane example

Cell membrane.

Which solution has highest boiling point?

Highest molality.

Which solution has lowest freezing point?

Highest molality.

Raoult law valid for

Ideal and dilute solutions.

Henry law valid for

Gas in liquid dilute solution.

Mole fraction of solvent

n solvent / total moles.

Mole fraction of solute

n solute / total moles.

Density formula

Density = Mass / Volume.

Molality formula using mass

m = (w2 × 1000)/(M2 × w1)

Molarity formula using mass

M = (w2 × 1000)/(M2 × V)

Define vapour pressure

Pressure exerted by vapour in equilibrium.

RLVP proportional to

Mole fraction of solute.

If solute non volatile then

Vapour pressure decreases.

If solute volatile then

Total vapour pressure depends on both.

Boiling point defined as

Temperature when vapour pressure equals atmospheric.

Freezing point defined as

Temperature when liquid equals solid phase.

Colligative properties depend on

Number of particles.

Strong electrolyte example

NaCl.

Weak electrolyte example

CH3COOH.

Non electrolyte example

Glucose.

Osmotic pressure highest for

Maximum particles.

Which property independent of temperature

Molality.

Which property independent of pressure

Molality.

Van't Hoff factor formula

i = normal molar mass / abnormal molar mass.

Degree of dissociation formula

i = 1 + α(n − 1)

Degree of association formula

i = 1 − α(n − 1)

Relation ΔTb and molar mass

Inverse relation.

Relation ΔTf and molar mass

Inverse relation.

Osmotic pressure used for

Molar mass determination.

Why osmotic pressure preferred?

Works at room temperature.

Electrolytes dissociate into

More particles.

Association forms

Dimers or polymers.

Azeotropes cannot be separated by

Simple distillation.

Minimum boiling azeotrope shows

Positive deviation.

Maximum boiling azeotrope shows

Negative deviation.

Ideal solution intermolecular forces

A-A equals B-B equals A-B.

Positive deviation forces

A-B weaker.

Negative deviation forces

A-B stronger.

Henry constant increases means

Gas solubility decreases.

Colligative properties order

Osmotic pressure > BP elevation > FP depression > RLVP.

Most sensitive colligative property

Osmotic pressure.

RLVP used for

Molar mass determination.

Kb called

Ebullioscopic constant.

Kf called

Cryoscopic constant.

Molality used in

Colligative properties.

Molarity used in

Titrations.

ppm units mg per liter for

Aqueous solutions.

Freezing point depression proportional to

Molality.

Boiling point elevation proportional to

Molality.

Osmotic pressure proportional to

Molarity.

Raoult law for solvent

P = Xsolvent P°

RLVP equals

Mole fraction solute.

Semi permeable membrane allows

Only solvent molecules.

Reverse osmosis used in

Desalination.

Gas solubility decreases when

Temperature increases.

Gas solubility increases when

Pressure increases.

Electrolytes increase boiling point more because

More particles formed.

Association decreases colligative property because

Particles decrease.

Dissociation increases colligative property because

Particles increase.

van't Hoff factor for K2SO4

van't Hoff factor for Na2SO4

van't Hoff factor for MgCl2

van't Hoff factor for Al2(SO4)3

Ideal solution enthalpy change

Zero.

Ideal solution volume change

Zero.

Positive deviation enthalpy change

Positive.

Negative deviation enthalpy change

Negative.

Boiling point elevation constant depends on

Solvent.

Freezing point depression constant depends on

Solvent.

Colligative properties independent of

Nature of solute.

Colligative properties depend on

Number of particles.

Osmotic pressure symbol

Boiling elevation symbol

ΔTb

Freezing depression symbol

ΔTf

RLVP symbol

(P° − P)/P°

Mole fraction symbol

Molality symbol

Molarity symbol

Henry constant symbol

van't Hoff factor symbol

Kb relation

ΔTb / m

Kf relation

ΔTf / m

If solute volatile then

Raoult law applied to both components.

Total vapour pressure ideal solution

Sum of partial pressures.

Azeotrope composition

Vapour equals liquid.

Distillation fails for

Azeotropes.

Reverse osmosis pressure applied

Greater than osmotic pressure.

Semipermeable membrane example

Animal bladder.

Association example

Benzoic acid in benzene.

Dissociation example

NaCl in water.

Boiling point order depends on

Molality and i.

Freezing point order depends on

Molality and i.

Osmotic pressure order depends on

Molarity and i.

RLVP order depends on

Mole fraction solute and i.

Colligative properties formula include

i factor.

Density used for

Molarity molality conversion.

Mole fraction independent of

Temperature.

Molality independent of

Temperature.

Molarity dependent on

Temperature.

Henry law constant depends on

Temperature and gas nature.

Raoult law valid for

Ideal solutions.

Henry law for

Dilute gas solutions.

Electrolytes produce

Abnormal molar mass.

Non electrolytes produce

Normal molar mass.

Solutions Class 12th P.C Flashcards

(179 cards)