(a) Define the following terms :
`{:((i)"Ideal solution",(ii)"Osmotic pressure"):}`
(b) Calculate the boiling point elevation for a solution prepared by adding 10g `CaCl_(2)` to 200g of water, assuming that `CaCl_(2) `is completely dissociated.
`(K_(b)"for water"=0.512Kg mol^(-1),"Mole mass of "`CaCl_(2)=111g mol^(-1))`

Explanation

### Step-by-Step Solution

**(a) Definitions:**

(i) **Ideal Solution**: An ideal solution is a solution that obeys Raoult's law at all concentrations and temperatures. In an ideal solution, the interactions between the molecules of different components are similar to the interactions between the molecules of the same component. This means that the vapor pressure of each component in the solution is proportional to its mole fraction.

(ii) **Osmotic Pressure**: Osmotic pressure is the pressure that must be applied to a solution to prevent the flow of solvent into it through a semipermeable membrane. It is a measure of the tendency of a solvent to move into the solution by osmosis. The osmotic pressure can be calculated using the formula:
\[ \Pi = iCRT \]
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