Types Of Solutions

Moles of ethanol: Moles of water: Mole fraction of ethanol: Mole fraction of water:

- Specific resistance ( ): The resistance offered by a unit length and unit cross-sectional area of a material. It is given by: where is resistance, is cross-sectional area, and is the length. - Conductance ( ): The reciprocal of resistance. It is given by:

Moles of : Normality:

The solubility of gases in liquids is generally inversely proportional to temperature, meaning that as the temperature of the liquid increases, the solubility of the gas decreases. This can be explained through the following points: 1. Increased Kinetic Energy of Gas Molecules
As the temperature increases, the kinetic energy of the gas molecules also increases. The molecules move faster, and as a result, they are more likely to overcome the intermolecular forces that hold them in the liquid. This leads to a higher tendency for the gas molecules to escape from the liquid into the gas phase. Therefore, the gas becomes less soluble in the liquid.
2. Le Chatelier's Principle
Le Chatelier's principle states that if a system at equilibrium is disturbed, the equilibrium shifts in the direction that minimizes the effect of the disturbance. For gas solubility, when temperature increases, the equilibrium shifts in such a way that more gas molecules escape the liquid phase, reducing the solubility. This is because the dissolution of gas is an exothermic process, and according to Le Chatelier's principle, increasing the temperature causes the system to favor the gas phase, thus decreasing solubility.
3. Vapor Pressure of the Gas
At higher temperatures, the vapor pressure of the gas increases. This means that the gas is more likely to escape from the liquid to the surface and enter the gas phase. Thus, with an increase in temperature, the solubility of gases decreases because more gas molecules are found in the vapor phase. 4. Entropy Considerations
As temperature increases, the disorder or entropy of the system increases. At higher temperatures, the gas molecules have more freedom of motion and are less likely to stay dissolved in the liquid. This also leads to a decrease in solubility.
In conclusion, at higher temperatures, gas molecules gain enough energy to escape from the liquid, and the solubility decreases.

Definition:
Molality ( ) is defined as the number of moles of solute present in 1 kilogram of solvent.
Given:
Moles of solute = .
Mass of solvent = .

Step 1: Calculate molality.

A solid solution in which the solute is a gas typically refers to a gas dissolved in a solid (usually a metal). In this case, hydrogen gas can be absorbed by palladium metal to form a solid solution, called palladium hydride. This is a well-known example of a gas being absorbed into a metal to form a solid solution. Palladium is particularly known for its ability to absorb hydrogen gas into its structure at certain conditions, forming a hydrogen-rich alloy.
The other options are not examples of solid solutions involving a gas as the solute. For example:
- Oxygen dissolved in water is a gas dissolved in a liquid, not a solid solution.
- Solution of camphor in nitrogen is a liquid-solute in gas-solvent solution.
- Glucose dissolved in water is a solid dissolved in liquid, not a solid solution.
Thus, the correct answer is option (C) Solution of hydrogen in palladium.

A gaseous solution refers to a homogeneous mixture in which the solvent is a gas. The solute may be solid, liquid, or gas, but the solvent must be a gas.
Let us analyze the given options one by one:
1. Solution of camphor in nitrogen: Here nitrogen is the solvent (gas) and camphor particles get dispersed in it. This forms a gaseous solution. This is the correct example.
2. Solution of hydrogen in palladium: This represents a solid solution, since palladium is a metal and hydrogen gas occupies interstitial sites in its lattice. This is not a gaseous solution.
3. Amalgam of mercury with sodium: This is a solid–liquid type solution, where sodium dissolves in mercury to form an amalgam. It is not a gaseous solution.
4. Oxygen dissolved in water: This is a gas–liquid solution, not a gaseous solution.
Hence, the correct answer is option (A) Solution of camphor in nitrogen.

Step 1: Calculate molar mass of NaCl.
Molar mass of NaCl = Atomic mass of Na + Atomic mass of Cl
= 23 + 35.5 = 58.5 g/mol
Step 2: Calculate moles of NaCl.
Moles of NaCl =
=
Step 3: Convert volume of solution to liters.
200 ml =
Step 4: Calculate molarity.
Molarity
= Final Answer: