RBSE Class 12 Chemistry Notes Chapter 2 Solutions

These comprehensive RBSE Class 12 Chemistry Notes Chapter 2 Solutions will give a brief overview of all the concepts.

RBSE Class 12 Chemistry Chapter 2 Notes Solutions

→ Homogeneous solution: If the composition of solute and solvent in a solution is same throughout the solution or the distribution of each component is similar throughout the solution then it is called a homogeneous solution. Example: Solution of sugar in water.

→ Heterogeneous solution: When the composition of solute and solvent is not same througout the solution, then the solutionis called heterogeneous solution. Example: solution of carbon and sulphur.

→ Saturated solution: A solution in which no more solute can be dissolved at the same temperature and pressure is called a saturated solution.

→ Unsaturated solution: A solution in which more solute can be dissolved at the same temperature and pressure is called unsaturated solution.

 

→ Supersaturated solution: The solution that contains more of the dissolved material than could be dissolved by the solvent under normal conditions is called supersaturated solution.

→ Mass percentage: It is the number of parts of mass of one component per 100 parts by mass of the solution.

→ Volume percentage: It is the number of parts by volume of one component per 100 parts by volume of the solution.

→ Mass/volume percentage : The mass of the solute dissolved in 100 mL of the solution is called mass by volume percentage.

→ Parts per million (ppm): It is the number of parts by mass of a component per million parts by mass of the solution.

→ Mole fraction: It is the ratio of the number of moles of one component to the total number of moles of all the components present in the solution.

→ Molarity: It is the number of gram moles of solute dissolved per litre of the solution.

→ Molality: It is the number of gram moles of solute dissolved in 1 kg of solvent.

→ Nprmality: It is the number of gram equivalents of solute dissolved per litre of the solution.

→ Formality: It is the number of formula masses of the solute dissolved per litre of the solution.

→ Solubility : It is the amount of solute dissolved in 100 gram of solvent to make saturated solution at a particular temperature.

→ Lattice energy: It is the amount of energy released when 1 mole of ionic solid is formed from its constituent ion.

→ Hydration energy: It is the amount of energy released when 1 mole of solid is dissolved in water.

→ Transition Temperature: The temperature at which the solubility curve of two different crystalline forms meet with each other is known as transition temperature.

→ Absorption coefficient: The volume of gas at NTP which dissolves per unit volume of the solvent at the given temperature and under a pressure of one bar is absorption coefficient.

→ Henry's Law: The partial pressure of the gas in vapour phase is proportional to the mole fraction of the gas in the solution.

→ Anoxia: The people living at high altitudes or climbers have low concentration of oxygen in the blood. Low blood oxygen causes climbers to become weak and unable to think clearly. These symptoms are called anoxia.

→ Vapour pressure: The pressure exerted by the vapours of the liquid in equilibrium with the liquid at a given temperature is called vapour pressure.

→ Raoult's Law: For a solution of volatile liquids, the partial vapour pressure of each component in the solution is directly proportional to its mole fraction.

→ Ideal solution: The solutions which obey Raoult's law over the entire range of concentration and temperature are called ideal solutions.

→ Non-Ideal solution: The solutions which do not obey the Raoult's Law over the entire range of concentration are called non-ideal solution.

→ Azeotropes or Constant Boiling Mixture: The liquid mixtures having the same composition of liquid and vapour phase and boil at a constant temperature are called azeotropes are constant boiling mixture.

→ Minimum boiling azeotropes: The solutions which show a large positive deviation from Raoult's law form minimum boiling azeotropes at specific composition. Example: C2H5OH + H20.

→ Maximum boiling azeotropes: The solutions which show a negative deviation from Raoult's law form maximum boiling azeotropes at specific composition. Example: HC1 + H20.

→ Colligative property: The properties of the solutions which depend only on the numbers of solute particles or the number of moles of the solute but not on the nature and chemical properties of the solute are called colligative properties.

→ Relative lowering of vapour pressure: When a non-volatile solute is added to a solvent, the vapour pressure of the solution decreases. The relative lowering in vapour pressure of solution containing non-volatile solute is equal to the mole fraction of solute in solution.

→ Boiling point: The temperature at which the vapour pressure of a liquid becomes equal to the atmospheric pressure is called boiling point of that liquid.

→ Ebullioscopic constant: It is equal to the elevation in boiling point when 1 mole of solute is dissolved in 1000 g of the solvent. Its unit is K kg mol^-1.

→ Freezing point: The temperature at which the solid and the liquid phases of the substance have the same vapour pressure is called freezing point of that substance.

→ Cryoscopic constant: It is equal to the depression in freezing point, when 1 mole of solute is dissolved in 1000 g of the solvent. Its unit is K kg mol^-1.

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

→ Semipermeable membrane: The membrane made up of animal or vegetable origin and these occur naturally such as Pig's bladder of parchment or can be synthetic such as cellophane. It contains a network of submicroscopic holes or pores. Therefore, small solvent molecules like water can pass through the holes of semipermeable membrane but the passage Of bigger molecules like solute is hindered.

→ Osmotic Pressure: The extra pressure which must be applied on the solution to stop the flow of solvent, is called osmotic pressure.

→ Isotonic solutions: Two solutions having same osmotic pressure at a given temperature are called isotonic solutions.

→ Hypertonic solution: A solution having higher osmotic pressure than some other solution is called hypertonic solution.

→ Hypotonic solution: A solution having lower osmotic pressure than some other solution is called the hypotonic solution.

→ Hemolysis: The selling or repturing of cell is called Hemoloysis.

→ Plasmolysis: The shrinking of the cells is called plasmolysis.

→ Reverse Osmosis: The process of movement of solvent molecules from the solution to the pure solvent through the semipermeable membrane by applying extra pressure on the solution side is called reverse osmosis.

→ Van't Hoff factor: It is the ratio of the experimental or observed value of colligative property to the calculated or normal value of colligative property.

→ Mass%(w/W) = \(\frac{\text { Mass of solute in grams }}{\text { Mass of solution in grams }}\) × 100

→ Volume %(v/V) = \(\frac{\text { Volume of a component }}{\text { Total volume of solution }}\) × 100

→ Mass by volume %(w/W) = \(\frac{\text { Mass of solute in grams }}{\text { Volume of solution in } \mathrm{mL}}\) × 100

→ Parts per million(ppm) = \(\frac{\text { Mass of the component }}{\text { Total mass of solution }}\) × 10⁶

→ Mole fraction x_A = \(\frac{n_{\mathrm{A}}}{n_{\mathrm{A}}+n_{\mathrm{B}}}\)
= Mole fraction of component A
x_B = \(\frac{n_{\mathrm{B}}}{n_{\mathrm{A}}+n_{\mathrm{B}}}\)
= Mole fraction of component B
n_A = Moles of A
n_B = Moles of B, x_A + x_B = 1

→ Molarity (M) = \(\frac{W_{\mathrm{B}} \times 1000}{\mathrm{M}_{\mathrm{B}} \times \mathrm{V}_{(m \mathrm{~L})}}\)
Where, W_B = Mass of solute
M_B = Molar mass of solute
V(mL) = Volume of solution in mL

→ Molality (m) = \(\frac{W_B \times 1000}{M_B \times W_A}\)
W_A = Mass of solvent
W_B = Mass of solute
M_B = Molar mass of solute

→ Relation between molarity and molality Molarity × Molar mass of solute
= Normality × Equivalent mass of solute

→ Relation between molarity and mass percentage
M = \(\frac{p \times d \times 10}{\mathrm{M}_{\mathrm{B}}}\)
p = mass %,
d = density

→ Relation between molality and molarity
m = \(\frac{1000 \mathrm{M}}{(1000 d)-\left(\mathrm{M} \times \mathrm{M}_{\mathrm{B}}\right)}\)

→ Relation between molality and mole fraction
x_B = \(\frac{m \times \mathrm{M}_{\mathrm{A}}}{1000+m \times \mathrm{M}_{\mathrm{A}}}\)

→ Molarity equation M₁V₁ = M₂V₂

→ Molarity of mixture M = \(\frac{\mathrm{M}_1 \mathrm{~V}_1+\mathrm{M}_2 \mathrm{~V}_2}{\mathrm{~V}_1+\mathrm{V}_2}\)

→ Relation between molarity and mole fraction
Where x_B = \(\frac{\mathrm{M} \times \mathrm{M}_{\mathrm{A}}}{\mathrm{M}\left(\mathrm{M}_{\mathrm{A}}-\mathrm{M}_{\mathrm{B}}\right)+1000 d}\)
d = density
M_A = Molar mass of solvent
M_B = Molar mass of solute
M = Molarity of solution
x_B = Mole fraction of solute

→ Osmotic pressure π = \(\frac{\mathrm{W}_{\mathrm{B}} \times \mathrm{R} \times \mathrm{T}}{\mathrm{M}_{\mathrm{B}} \times \mathrm{V}}\)
Where,
T = Temperature in Kelvin
V = Volume of solution in litres
R = Gas constant

→ Equations for colligative properties modified by Van't Hoff factor
(a) \(\frac{p_{\mathrm{A}}^{\circ}-p_{\mathrm{A}}}{p_{\mathrm{A}}^{\circ}}\) = i × x_B
(b) ΔT_B = i × K_B × m
(c) ΔT_f = i × K_f × m
(d) πV = iCRT