Azeotropic mixture Questions in English

(A) Fractional distillation is used to separate mixtures of miscible liquids that have a significant difference in their boiling points.
$A$. Benzene (boiling point $\approx 80.1 \ ^{\circ}C$) and Toluene (boiling point $\approx 110.6 \ ^{\circ}C$) form an ideal solution and can be separated by fractional distillation.
$B$,$C$,and $D$ form azeotropic mixtures (constant boiling mixtures) at certain compositions,which makes them difficult to separate into pure components by simple fractional distillation.

(D) An azeotropic mixture is a constant boiling mixture that behaves like a pure liquid.
Since it boils at a constant temperature without changing its composition,it is not possible to separate the components of an azeotropic mixture by simple distillation.
Therefore,neither $HCl$ nor $H_2O$ can be obtained in their pure states from this mixture.

(C) When a solution shows a positive deviation from Raoult's law,the intermolecular forces between the solute and solvent molecules are weaker than those present in the pure components.
This results in an increase in the total vapour pressure of the solution compared to the ideal solution.
Because the vapour pressure is higher,the solution reaches its boiling point at a lower temperature than either of the pure components. This is known as a minimum-boiling azeotrope.

(D) An azeotropic mixture is a mixture of two liquids that boils at one particular temperature like a pure liquid and distills over in the same composition.

(A) An azeotropic mixture is a liquid mixture that has a constant boiling point because the vapour phase has the same composition as the liquid phase. Thus,they boil at a constant temperature like a pure liquid.

(B) Some liquids,on mixing,form azeotropes,which are binary mixtures having the same composition in liquid and vapour phases and boil at a constant temperature.
In such cases,it is not possible to separate the components by fractional distillation.
This mixture is known as an Azeotropic mixture.

(D) The azeotropic mixture of $HCl$ and water is a constant boiling mixture that contains $20.2\%$ $HCl$ by mass.
Therefore,the correct option is $(D)$.

(D) Rectified spirit is an azeotropic mixture of $95.5 \%$ ethanol and $4.5 \%$ water.
Since this mixture boils at a constant temperature,it cannot be separated by simple fractional distillation.
Benzene is added to form a ternary azeotrope with water and ethanol,which has a lower boiling point $(64.9 \ ^{\circ}C)$ than the binary azeotrope of ethanol-water $(78.1 \ ^{\circ}C)$.
This ternary azeotrope distills off first,leaving behind pure (absolute) alcohol.

(C) The solution of ethanol and water forms an azeotropic mixture,which is a constant boiling point mixture.
In an azeotropic mixture,the liquid and vapor phases have the same composition,and therefore,their proportions cannot be altered or separated by simple fractional distillation.
Thus,absolute ethanol cannot be obtained by simple fractional distillation of the solution of ethanol and water because they form a constant boiling mixture.

(A) Rectified spirit is a mixture of approximately $95.6 \%$ ethanol and $4.4 \%$ water by mass.
This mixture forms a positive azeotrope,which means it boils at a constant temperature and has the same composition in both the liquid and vapor phases.
Because the composition of the vapor is identical to that of the liquid,fractional distillation cannot separate the components to obtain pure (absolute) alcohol.

(A) The mixture of ethanol and water forms an azeotropic mixture,which is a constant boiling point mixture.
In an azeotrope,the composition of the liquid phase and the vapor phase is identical at a specific temperature.
Therefore,the proportions of the components cannot be altered or changed by simple distillation.
Thus,absolute ethanol cannot be obtained from this mixture by simple distillation.

(C) Rectified spirit contains approximately $95.6\%$ ethanol and $4.4\%$ water by mass,which forms a constant boiling mixture known as an azeotrope.
Since simple fractional distillation cannot separate the components of an azeotrope,azeotropic distillation is used.
In this process,a third component like benzene is added to break the azeotrope,allowing the production of absolute alcohol ($100\%$ pure ethanol).

(A) Azeotropic distillation method:
Rectified spirit $+$ Benzene $+$ water
$\downarrow$ Fractional distillation
The first fraction obtained at $331.8 \ K$ is a ternary azeotrope consisting of $H_2O$ $(7.4 \%)$,Benzene $(74 \%)$,and alcohol $(18.5 \%)$.
The second fraction obtained at $341.2 \ K$ is a binary azeotrope consisting of Benzene $(67.7 \%)$ and alcohol $(32.2 \%)$.
The final fraction obtained at $351 \ K$ is absolute alcohol.

(D) An azeotropic mixture of $HCl$ and water is a constant boiling mixture that contains approximately $20.2\%$ $HCl$ by mass.

(D) An azeotropic mixture is a constant boiling mixture that distills at a constant temperature without change in composition.
Therefore,the components of an azeotropic mixture cannot be separated by simple distillation.

(D) Azeotropic mixtures are constant boiling mixtures.
Solutions that show a large positive deviation from Raoult's law form minimum boiling azeotropes at a specific composition.
In these mixtures,the intermolecular forces of attraction between the components are weaker than those in the pure components,leading to a higher vapor pressure and consequently a lower boiling point than either of the pure components.

(A) Rectified spirit is an azeotropic mixture of $95.87 \% \text{ ethyl alcohol}$ and $4.13 \% \text{ water}$ by mass.

(C) For an ideal solution,the intermolecular forces of attraction between $A-A$ and $B-B$ are equal to those between $A-B$. Thus,option $A$ is incorrect.
Henry's law relates the solubility of a gas in a liquid to the partial pressure of the gas,not directly to temperature. Thus,option $B$ is incorrect.
When a solution shows a negative deviation from Raoult's law,the intermolecular forces between $A$ and $B$ are stronger than those between $A-A$ and $B-B$. This leads to a decrease in vapor pressure and an increase in boiling point,resulting in a maximum boiling point azeotrope. Thus,option $C$ is correct.
The addition of a nonvolatile solute to a volatile solvent leads to an elevation in boiling point,not a decrease. Thus,option $D$ is incorrect.

(A) An azeotropic mixture with a boiling point higher than both individual components is known as a maximum boiling azeotrope.
This occurs due to strong attractive forces between the components,which leads to a decrease in vapor pressure.
According to Raoult's law,this behavior is classified as a negative deviation from ideal behavior.

(B) An azeotropic mixture that has a boiling point lower than both its components is known as a minimum boiling azeotrope. This occurs when the solution exhibits a large positive deviation from Raoult's law,where the intermolecular forces between the components are weaker than those in the pure components,leading to an increase in vapor pressure.

(B) An azeotropic mixture that has a boiling point lower than both its individual components is known as a minimum-boiling azeotrope.
This behavior is characteristic of solutions that exhibit positive deviations from Raoult's law.
In such cases:
$(I)$ The experimental vapor pressure of the mixture is higher than the calculated value.
$(II)$ The experimental boiling point of the mixture is lower than the calculated value.
$(III)$ The enthalpy of mixing is positive,$\Delta_{mix} H > 0$.
$(IV)$ The volume change upon mixing is positive,$\Delta V_{mix} > 0$.

(D) solution of $HCl$ in water containing $22\%$ by weight is an azeotropic mixture.
Because it forms an azeotropic mixture,$HCl$ cannot be concentrated beyond $22\%$ by boiling.

(C) low-boiling azeotrope is formed by solutions showing positive deviation from Raoult's Law.
These solutions have a vapor pressure higher than that of the pure components,resulting in a lower boiling point.
$CHCl_3 + CH_3COCH_3$ (acetone) is a classic example of a mixture that exhibits positive deviation from Raoult's Law due to the weakening of intermolecular forces (breaking of hydrogen bonds between chloroform and acetone).
Therefore,it forms a low-boiling azeotrope.

(B) Azeotropic mixtures that boil at a temperature lower than the boiling point of any of their components are known as minimum boiling azeotropes.
These mixtures are formed by solutions that show a large positive deviation from Raoult's law.
In such cases,the vapor pressure of the solution is higher than the vapor pressure of the individual components,leading to a lower boiling point.

(B) An azeotropic mixture that has a boiling point lower than both its individual components is known as a minimum-boiling azeotrope.
This occurs in solutions that exhibit a large positive deviation from Raoult's law.
In such cases,the intermolecular forces between the components are weaker than the forces between the pure components,leading to higher vapor pressure and consequently a lower boiling point.

(D) dilute solution of $HCl$ forms an azeotropic mixture with water at a concentration of approximately $22.2 \%$ by mass.
Because it is an azeotropic mixture,it boils at a constant temperature without changing its composition.
Therefore,it cannot be concentrated beyond this limit by simple boiling.

(A) Rectified spirit is a constant boiling mixture (azeotrope) of ethanol and water.
It contains approximately $95.87\%$ by mass of ethyl alcohol $(C_2H_5OH)$ and $4.13\%$ by mass of water.
This specific composition is obtained by the fractional distillation of fermented liquors.

(A) Maximum boiling azeotropes are formed by solutions that show large negative deviation from Raoult's law.
In these solutions,the solute-solvent interactions are stronger than the solute-solute and solvent-solvent interactions.
Water + Nitric acid $(H_2O + HNO_3)$ shows a large negative deviation from ideal behavior,resulting in a maximum boiling azeotrope.

(N/A) Azeotropes are binary mixtures that have the same composition in both liquid and vapour phases and boil at a constant temperature. In such cases,it is not possible to separate the components by fractional distillation.
There are two types of azeotropes: minimum boiling azeotrope and maximum boiling azeotrope.
$(i)$ Minimum boiling azeotrope: Solutions that show a large positive deviation from Raoult's law form a minimum boiling azeotrope at a specific composition. For example,an ethanol-water mixture on fractional distillation yields a solution containing approximately $95 \%$ by volume of ethanol. Once this composition is reached,the liquid and vapour have the same composition,and no further separation occurs.
$(ii)$ Maximum boiling azeotropes: Solutions that show a large negative deviation from Raoult's law form a maximum boiling azeotrope at a specific composition. For example,nitric acid and water form this class of azeotrope. This mixture has an approximate composition of $68 \%$ nitric acid and $32 \%$ water by mass,with a boiling point of $393.5 \ K$.

(N/A) When the composition of the liquid phase and the vapour phase becomes identical,the mixture is known as an azeotrope or a constant boiling mixture.
At this point,the mixture boils at a constant temperature without any change in composition.
Therefore,further separation by fractional distillation is not possible because the components cannot be separated based on their boiling points once the azeotropic composition is reached.

(N/A) Pure ethanol cannot be obtained by fractional distillation because it forms a constant-boiling mixture (azeotrope) with water at a concentration of approximately $95.4\%$ ethanol by mass.
This mixture boils at a constant temperature and cannot be separated into its pure components by simple distillation.
Such mixtures are generally called Azeotropes.
There are $2$ types of such mixtures:
$(i)$ Minimum boiling azeotropes
(ii) Maximum boiling azeotropes.

(A) Aqueous $HNO_3$ forms a constant boiling mixture (azeotrope) with water at a concentration of approximately $68\%$ by mass.
Distillation of dilute $HNO_3$ results in the concentration of the acid up to this limit,after which the composition of the vapor becomes identical to that of the liquid,preventing further concentration by simple distillation.

(A) In a fractional distillation column,the vapour of the component with the lower boiling point rises to the top of the column because it is more volatile.
Conversely,the component with the higher boiling point remains in the liquid phase or condenses more readily,concentrating at the lower part of the column.

(B) binary mixture of $C_6H_5OH$ and $C_6H_5NH_2$ shows a negative deviation from Raoult's law.
This occurs because the intermolecular hydrogen bonding between phenol and aniline is stronger than the interactions in the pure components.
As a result,the vapour pressure of the solution is lower than that of the pure components,which leads to a higher boiling point for the solution compared to the pure components.
Therefore,this mixture forms a maximum boiling azeotrope,not a minimum boiling azeotrope.

(A) Azeotropic mixtures are constant boiling mixtures that distill without change in composition. They are formed only by non-$ideal$ solutions because $ideal$ solutions do not show significant deviations from Raoult's Law to form azeotropes.
Positive deviations from Raoult's Law lead to minimum boiling azeotropes (boiling point less than both components),while negative deviations lead to maximum boiling azeotropes (boiling point greater than both components). Thus,the Assertion is true.
The definition of an azeotrope is a mixture that boils at a constant temperature and has the same composition in both the liquid and vapour phases. This property is the fundamental reason why they cannot be separated by fractional distillation. Thus,the Reason is true and correctly explains why such mixtures behave as a single component during distillation,which is the basis for the Assertion.

(A) Azeotropes are formed by non-ideal solutions that show significant positive or negative deviations from Raoult's law.
$CCl_4$ and $CHCl_3$ form a non-ideal solution showing positive deviation from Raoult's law,which can form a minimum boiling azeotrope at a specific composition.
$n-Hexane + n-heptane$,$C_2H_5Br + C_2H_5Cl$,and $Chlorobenzene + Bromobenzene$ form nearly ideal solutions and do not form azeotropes.

(B) Minimum boiling azeotropes are formed by non-ideal solutions that show a large positive deviation from Raoult's law.
In these solutions,the $A-B$ molecular interactions are weaker than the $A-A$ and $B-B$ interactions.
Due to these weaker interactions,the molecules escape more easily into the vapour phase,resulting in a total vapour pressure that is greater than that predicted by Raoult's law for an ideal solution.
Additionally,for such solutions,the enthalpy of mixing $(\Delta H_{mix})$ is positive and there is a slight increase in volume upon mixing.
Therefore,the correct statement is that the total vapour pressure of the mixture is greater than that corresponding to an ideal solution.

(A) Statement $(I)$: $1,2,3$-Trihydroxypropane (glycerol) has a very high boiling point $(563 \ K)$ compared to water $(373 \ K)$. Due to this significant difference in boiling points,they can be separated by simple distillation. Thus,Statement $(I)$ is true.
Statement $(II)$: Azeotropic mixtures are constant boiling mixtures that possess the same composition in both liquid and vapor phases. Because they boil at a constant temperature,their components cannot be separated by simple or fractional distillation. Thus,Statement $(II)$ is true.