2 Marks Questions

Question 12 Marks

Which method is most suitable to determine molecular mass of polymer ?

Answer

→ Measurement of osmotic pressure provides another method of determining molar masses
of solutes. This method is widely used to determine molar masses of proteins, polymers and other marco molecules.
→ The osmotic pressure method has the advantage over other methods as pressure measurement is around the room temperature and the molarity of the solution is used instead of molality.
→ As compared to other colligative properties, its magnitude is large even for very dilute solutions. The technique of osmotic pressure for determination of molar mass of solutes is particularly useful for biomolecules as they are generally not stable at higher temperatures and polymers have poor solubility.

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Question 22 Marks

Explain reverse osmosis for purification of water.

Answer

→ The direction of osmosis can be reversed if a pressure larger than the osmotic pressure is applied to the solution side. That is, now the pure solvent flows out of the solution through the semi permeable membrane. This phenomenon is called reverse osmosis.

→ Reverse osmosis is used in desalination of sea water.
→ When pressure is more than osmotic pressure is applied, pure water is squeezed out of the sea water through the membrane. A variety of polymer membranes are available for this purpose.
→ The pressure required for the reverse osmosis is quite high. A workable porous membrane is a film of cellulose acetate placed over a suitable support. Cellulose acetate is permeable to water but impermeable to impurities and ions present in sea water.
→ These days many countries use desalination plants to meet their potable water requirements.

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Question 32 Marks

What is semi permeable membrane ? Give examples.

Answer

→ The membrane which allows only the small molecule of solvent to pass but can not pass solute molecule is known as semi permeable membrane.
Example: Pig's bladder, parchment, cellophane
→ These membranes appear to be continuous sheets or films, yet they contain a network of submicroscopic holes or pores.

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Question 42 Marks

How to find out $K_b$ and $K_f$ ?

Answer

$\begin{aligned} →\ \ K _f & =\frac{ R \times M _1 \times T_f^2}{1000 \times \Delta_{ Fus } H } \\ K _{ b } & =\frac{ R \times M _1 \times T_{ b }^2}{1000 \times \Delta_{\text {vap }} H }\end{aligned}$
$\begin{aligned}Where\ \ \ R & =\text { gas constant }
\\ M _1 & =\text { Molar mass of solvent }
\\ T_f & =\text { Freezing point of pure solvent }
\\ T_{ b } & =\text { Boiling point of pure solvent. }
\\ \Delta_{\text {Fus }}^{ H } & =\text { Fusion enthalpy }
\\ \Delta_{\text {vap }}^{ H } & =\text { Vapourisation enthalpy }\end{aligned}$

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Question 52 Marks

What is colligative properties? Write colligative properties of solution.

Answer

→ "Colligative properties of solution depend on the number of solute particles and does not depend on the nature of solute."
→ There are 4 types of colligative properties.
(1) relative lowering of vapour pressure of the solvent
(2) depression of freezing point of the solvent
(3) elevation of boiling point of the solvent and
(4) osmotic pressure of the solution

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Question 62 Marks

Explain Raoult's Law as a special case of Henry's Law

Answer

→ According to Raoult's law, the vapour pressure of a volatile component in a given solution is given by
$p_1=p_1^0 \cdot x_1$
→ According to henry's Law solubility of gasous solute in liquid solvent is given by
$p= K _{ H } \cdot x$
→ If we compare the equations for Raoult's law and Henry's law, it can be seen that the partial pressure of the volatile component or gas is directly proportional to its mole fraction in solution.
→ Only the proportionality constant $K _{ H }$ differs from $p_1^0$.
→ Thus, Raoult's law becomes a special case of Henry's law in which $K _{ H }$ becomes equal to $p_1^0$.

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Question 72 Marks

Explain Parts per million (ppm) with examples.

Answer

→ "When a solute is present in trace quantities, it is convenient to express concentration in parts per million (ppm)"
→ Parts per million $=\frac{\text { Number of parts of the component }}{\text { Total number of parts of all components of the solution }} \times 10^6$
→ Parts per million can also be expressed as mass to mass, volume to volume and mass to volume.
→ A litre of sea water (which weighs 1030 g ) contains about $6 \times 10^{-3}$ of dissolved oxygen$\left( O _2\right)$. Such a small concentration is also expressed as 5.8 g per$10^6 g(5.8 ppm )$ of sea water.
→ The concentration of pollutants in water or atmosphere is often expressed in terms of$\mu g$$mL ^{-1}$ or ppm.

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Question 82 Marks

Explain (% W/V) Mass by volume Percentage with examples.

Answer

→ "The mass of Solute (g) dissolved in 100 ml Solution is called mass by Volume Percentage (% W/V)."
→ $\% W / V =\frac{\text { mass of solute } g \times 100}{\text { Volume of solution }( ml )}$
→ For example 5% W/V aqueous solution of sugar means 5 gram sugar is dissolved in 100 ml solution.

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Question 92 Marks

Explain (% V/V) Volume Percentage with examples.

Answer

→ "The volume of Solute (ml) dissolved in 100 ml solution is known as volume percentage (% V/V)."
→ Volume % of a component =
$\frac{\text { Volume of the component }( ml )}{\text { Total volume of solution }( ml )} \times 100$
→ For example, 10% ethanol solution in water means that 10 mL of ethanol is dissolved in water such that the total volume of the solution is 100 mL.
→ Solutions containing liquids are commonly expressed in this unit.
→ For example, a 35% (v/v) solution of ethylene glycol, an antifreeze, is used in cars for cooling the engine. At this concentration the antifreeze lowers the freezing point of water to 255.4K (-17.6°C).

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Question 102 Marks

What is Concentration of Solution?
Write down different Types of Units of Concentration?

Answer

→ "The amount of solute present in per unit volume of solution is known as Concentration."
→ There are 9 Types of Unit of Concentration:
(1) %/W/W (Mass Percentage)
(2) % V/V (Volume Percentage)
(3)% W/V (Mass by Volume Percentage)
(4) ppm (Parts Per million)
(5) Mole-Fraction (X)
(6) Molarity (M)
(7) Molality (m)
(8) Normality (N)
(9) Formality (F)

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