Ideal and Non-Ideal Solutions

Calculate the b.pt. of $1$ molar aqueous solution of $\mathrm{KBr}.$ Given that the density of solution is $1.06 \mathrm{g} {\mathrm{mL}}^{-}, {\mathrm{K}}_{\mathrm{b}}$ for water is $0.52 \mathrm{K} \mathrm{kg}{ \mathrm{mol}}^{-}.$
[Atomic mass of $\mathrm{K}=39, \mathrm{Br}=80$]

Considering the formation, breaking and strength of hydrogen bond, predict which of the following mixtures will show a positive deviation from Raoult's law?

A solution obtained by dissolving $342 \mathrm{g}$ of sugar $\left({\mathrm{C}}_{12}{\mathrm{H}}_{22}{\mathrm{O}}_{11}\right)$ in $1000 \mathrm{g}$ water is_____molal.

Explain with the help of a diagram why some of the non-ideal solutions show positive deviations while some others show negative deviations.

What are ideal and non-ideal solutions? What type of non-idealities are exhibited by cyclohexane-ethanol and acetone-chloroform mixture? Give reasons for your answer.

What are the conditions necessary to show ideal behaviour of solution?

$\mathrm{A}$ and $\mathrm{B}$ liquids on mixing produced a warm solution. Which type of deviation is there and why?

Give reason when $30 \mathrm{mL}$ of ethyl alcohol and $30 \mathrm{mL}$ of water are mixed, the volume of resulting solution is more than $60 \mathrm{mL}.$

Vapour pressure of chloroform $\left({\mathrm{CHCl}}_3\right)$ and dichloromethane $\left({\mathrm{CH}}_2{\mathrm{Cl}}_2\right)$ at $298 \mathrm{K}$ are $200 \mathrm{mm} \mathrm{Hg}$ and $415 \mathrm{mm} \mathrm{Hg}$ respectively.
Calculate the vapour pressure of the solution prepared by mixing $25.5 \mathrm{g}$ of ${\mathrm{CHCl}}_3$ and $40 \mathrm{g}$ of ${\mathrm{CH}}_2{\mathrm{Cl}}_2$ at $298 \mathrm{K}$

Why does a solution of ethanol and cyclohexane shows positive deviations?

$10 \mathrm{mL}$ of a liquid A were mixed with $10 \mathrm{mL}$ of liquid $\mathrm{B}.$ The volume of resulting solution was found to be $19.9 \mathrm{mL}.$ What do you conclude?

What will be the nature of the solution when ethyl alcohol and water are mixed?

What is meant by positive and negative deviations from Raoult's law and how is the sign of ${\mathrm{\Delta }}_{\mathrm{sol}}\mathrm{H}$ related to positive and negative deviations from Raoult's law?

On mixing equal volumes of water and ethanol, what type of deviation would you expect from Raoult's law?

How does a non-ideal solution differ from an ideal solution? When does the positive deviations occur from ideality?

With the help of suitable diagrams, illustrate the two types of non-ideal solutions.

Give important differences between solutions showing positive and negative deviations.

Write two differences between ideal and non-ideal solutions.

Define azeotropic mixture.

State Raoult's law. Explain from it why the vapour pressure of a solution is always less than that of a pure solvent.