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Chemistry_NCERT > Solutions > Flashcards

Solutions Flashcards

1
Q

What is the Mass Percentage?

A

The mass percentage of a component in a given solution is the mass of the component per 100g of the solution.

Mass % of a component = Mass of the component in the solution/ Total mass of the solution × 100

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2
Q

What is the Volume Percentage?

A

The volume percentage is the volume of the component per 100 parts by volume of the solution.

Volume % of a component = Volume of the component/Total volume of solution × 100

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3
Q

What is Parts Per Million?

A

The number of parts by mass of solute per million parts by mass of the million.
ppm = Number of parts of the component/Total number of parts of all components in the solution × 10⁶

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4
Q

What is Mole Fraction?

A

The ratio of the number of one component to the total number of moles of all the components present in the solution.
Xₛₒₗᵤₜₑ = nₛₒₗᵤₜₑ / nₛₒₗᵤₜₑ + nₛₒₗᵥₑₙₜ

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5
Q

What is Molarity?

A

It is defined as the number of moles of solute dissolved in one liter.
Molarity = Number of moles of solute/Volume of solution (in liter)

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6
Q

What is Molality?

A

It is defined as the number of moles of solute dissolved in per kilogram of solvent.
Molalilty = Moles of solute/Mass of solvent (in kg)

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7
Q

What is Henry’s Law?

A

At constant temperature, the solubility of a gas in a liquid is directly proportional to the partial pressure of gas present above the surface of the liquid or solution.
P = Kₕ X

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8
Q

What is the significance of Henry’s law and Henry’s constant?

A

1) Different gases have different Kₕ values in the same solvent at the same temperature.
2) The value of Kₕ increases with an increase in temperature.
3) Higher the value of Kₕ at a particular pressure, the lower the solubility of the gas in the liquid.
4) It is applied to each gas independent of the presence of other gases.

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9
Q

What are the limitations of Henry’s law?

A

It is only applicable when
1) The pressure of the gas is not too high.
2) Temperature is not too low.
3) The gas should not go any chemical change.
4) The gas should not go association and disassociation in the solution.

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10
Q

What is Vapour Pressure?

A

The pressure exerted by the vapors above the liquid surface in equilibrium with the liquid at a given temperature.

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11
Q

What is the Raoult’s Law?

A

At a given temperature for a solution of volatile liquids, the partial vapor pressure of each component of the solution is directly proportional to its mole fraction present in the solution.
p = p₁ᵒ + (p₂ᵒ - p₁ᵒ) x₂

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12
Q

What are ideal solutions?

A

The solutions which obey the Raoult’s law over the entire range of concentration are known as ideal solutions.
• The enthalpy of mixing of the pure components to form the solution is zero.
• The volume of mixing is also zero.

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13
Q

What are non-ideal solutions?

A

Solutions which do not follow the Raoult’s law and show positive or negative deviation from the law are called non-ideal solutions.

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14
Q

How does a non-ideal solution show positive deviation from Raoult’s law?

A

When the intermolecular interactions are weaker than intramolecular interactions.
i.e. Iₐ₋ₓ < Iₐ₋ₐ and Iₓ₋ₓ
This means that molecules of A or X will find it easier to escape the solution, giving a positive deviation.

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15
Q

How does a non-ideal solution show negative deviation from Raoult’s law?

A

When the intermolecular interactions are stronger than intramolecular interactions.
i.e. Iₐ₋ₓ > Iₐ₋ₐ and Iₓ₋ₓ
This means that molecules of A or X will find it hard to escape the solution, giving a negative deviation as there is less vapor produced.

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16
Q

What are Azeotropes?

A

The binary liquid mixture having the same composition in liquid and vapour phase and that boil at constant temperature are called azeotropic mixtures.

17
Q

What are Minimum Boiling Azeotropes?

A

The non-ideal solutions which slow a large positive deviation from the Raoult’s law are called Minimum Boiling Azeotropes. In these solutions, there is one composition when the vapour pressure will be the highest and the boiling point the lowest.

18
Q

What are Maximum Boiling Azeotropes?

A

The non-ideal solutions which slow a large negative deviation from the Raoult’s law are called Maximum Boiling Azeotropes. In these solutions, there is one composition when the vapour pressure will be the lowest and the boiling point the highest.

19
Q

What are Colligative Properties?

A

Properties which only depend on the number of solute particles irrespective of their nature relative to the total number of particles present in the solution, are called Colligative Properties.

20
Q

What is Relative Lowering in Vapour Pressure?

A

The ratio of lowering of vapour pressure of a solution containing non-volatile solute to the vapour pressure of pure solvent is called relative lowering of vapour pressure.
X₂ = p₁° - p₁/p₁°
Where X₂ is the mole fraction of solute, p₁° is the vapour pressure of pure solute and p₁ of solvent in later phases.

21
Q

What is the Molar Mass in terms of Relative Lowering in Vapour Pressure?

A

M₂ = W₂M₁ / W₁(p₁° - p₁/p₁°)

22
Q

What is the Elevation in Boiling Point?

A

Boiling point elevation is the difference in temperature between the boiling point of a pure solvent and that of a solution when a non-volatile solute is added to a solvent.
ΔT = K (ebullioscopic constant) × m

23
Q

What is the Molar Mass in terms of Elevation in Boiling Point?

A

M₂ = Kb × W₂ × 1000/ΔTb × W₁

24
Q

What is Depression in Freezing Point?

A

The change in temperature of the freezing point of a solution after adding non-volatile solute into it is called Depression in Freezing point.
ΔT = K (cryoscopic constant) × m

25
Q

What is Osmosis?

A

The phenomenon of the flow of solvent through a semipermeable membrane from pure solvent to the solution is called osmosis.

26
Q

What is Osmotic Pressure (π)?

A

The excess pressure that must be applied to the solution side of the membrane to prevent osmosis is called osmotic pressure.
π = CRT

27
Q

What is the Molar Mass in terms of Osmotic Pressure?

A

M₂ = W₂ × RT/Vπ

28
Q

What is an Isotonic solution?

A

Two solutions having the same osmotic pressure at a given temperature is called isotonic solution.

29
Q

What is Hypertonic solution?

A

A solution having more osmotic pressure than the other solution is called hypertonic solution.

30
Q

What is Hypotonic Solution?

A

A solution having less osmotic pressure than the other solution is called Hypotonic Solution.

31
Q

What is Reverse Osmosis?

A

When a larger amount of pressure than the osmotic pressure is applied on the solution side is called Reverse Osmosis.

32
Q

What is Abnormal Molar Mass?

A

Molar masses that are either lower or higher than the expected or normal value are called abnormal molar masses. This happens due to association or dissociation or molecules.

33
Q

What is Association and Dissociation?

A

Association leads to decrease in the number of particles in a solution resulting in decreased value of Colligative property while Dissociation leads to increased number of particles in the solution resulting in increased value of Colligative property.

34
Q

What is Van’t Hoff Factor?

A

The ratio of the experimental value of the colligative property to the calculated value of the colligative property.
i = Observed Colligative property/Normal (calculated) Colligative property

35
Q

What is the Degree of Dissociation?

A

The fraction of the total substance that undergoes dissociation.
α (degree of dissociation) = (i – 1)/(n –1)

36
Q

What is the Degree of Association?

A

The fraction of the total substance that undergoes association.
α (degree of association) = (1- i)/(1 - 1/n)

Chemistry_NCERT (3 decks)

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