Solutions

The elevation in boiling point of a solution depends on the number of solute particles present in the solution, as well as their nature and concentration.

Let's analyze the given compounds and determine their behavior in the 1M aqueous solution:

A. (glucose) - Glucose is a covalent compound and does not dissociate into ions in solution. Therefore, it does not contribute additional particles to the solution.

B. - NaCl dissociates into and ions in solution. It forms two particles (one and one ) for every formula unit of NaCl.

C. - dissociates into and ions in solution. It forms three particles (one and two ) for every formula unit of .

D. - dissociates into and ions in solution. It forms four particles (one and three ) for every formula unit of .

E. - dissociates into and ions in solution. It forms five particles (two and three for every formula unit of .

Based on the number of particles formed in the solution, we can arrange the compounds in increasing order of elevation in boiling points:

B < C < D < E < A

Therefore, the correct answer is option (A) :-. B < C < D < E < A.

To calculate the molarity of a solution, we need to determine the number of moles of solute and divide it by the volume of the solution in liters.
Given:
Mass of NaOH =
Volume of solution = 450 mL =
First, we need to calculate the number of moles of NaOH. The molar mass of NaOH is approximately 40 g/mol ( for Na + for O + for H).
Number of moles of NaOH = = =
Now we can calculate the molarity of the solution using the formula:
Molarity

Molarity

Therefore, the molarity of the solution containing of NaOH in solution is approximately .

To determine the total number of ions produced from the compound in aqueous solution, we need to understand the dissociation process of the compound in water:

1. The compound is a complex salt consisting of a coordination complex and chloride ions Cl^-.
2. In aqueous solution, the compound dissociates into its constituent ions:
3. Upon dissociation, one ion and three Cl^- ions are formed.
4. Adding the ions together, the total number of ions produced is .

Thus, the total number of ions produced in the solution is 4.

To find the mole percentage of 'D' in the solution, we can use Raoult's Law, which states that the total vapor pressure of a solution (P_solution) is the sum of the partial pressures of its components. The partial pressure of a component in a solution is given by its mole fraction multiplied by its vapor pressure in the pure state. Hence, for a binary solution of 'A' and 'D', we have:

P_solution = P_A + P_D

where:

• P_A = x_A × P⁰_A
• P_D = x_D × P⁰_D

Given:

• P⁰_A = 500 mm Hg
• P⁰_D = 800 mm Hg
• P_solution = 700 mm Hg

Since x_A + x_D = 1, we can substitute P_solution:

700 = x_A × 500 + (1 - x_A) × 800

Simplifying, we get:

700 = 500x_A + 800 - 800x_A

700 = 800 - 300x_A

300x_A = 800 - 700

300x_A = 100

x_A = 100/300 = 1/3

x_D = 1 - x_A = 2/3

The mole percentage of 'D' = x_D × 100 = 66.67%

Therefore, the mole percentage of 'D' in the solution is 66.67 mole percent.

A molecule X associates as per the equation: . Given: the van’t Hoff factor (i) is 0.80, and the fraction of associated molecules (α) is 0.3. We need to find the value of ‘n’.

For association, van’t Hoff factor is given by:

Substitute the given values:

Simplify the equation:

Thus, the value of 'n' is .

In the study of solutions, particularly in Chemistry, the molal elevation constant is a term used when discussing the colligative properties of solutions. The colligative properties depend on the amount of solute particles in a solution, rather than the identity of the solute itself. One such property is the elevation of the boiling point, commonly observed when a solute is dissolved in a solvent.

When a non-volatile solute is added to a solvent, the boiling point of the solution is higher than that of the pure solvent. This phenomenon is due to the decrease in the solvent's vapor pressure, requiring a higher temperature to reach boiling. The change in boiling point, ΔT_b, can be described using the equation:

ΔT_b = K_b × m

Where:

• ΔT_b is the boiling point elevation.
• K_b is the molal elevation constant, also known as the ebullioscopic constant.
• m is the molality of the solution, defined as moles of solute per kilogram of solvent.

The term "ebullioscopic constant" originates from the Latin word "ebullire" meaning to boil, and it quantifies how much the boiling point increases per molal concentration of the solute.

Based on the given options, the correct answer is: Ebullioscopic constant

When discussing the properties of electrolytes, we often refer to molar conductivity, denoted by the symbol Λ_m. This term describes how well an electrolyte conducts electricity when dissolved in a solution, and it depends on the concentration of the electrolyte. As the concentration decreases, molar conductivity typically increases due to reduced ion pairing.

Molar conductivity at zero concentration is particularly significant, which is the behavior of the electrolyte when dilution approaches infinity (i.e., when concentration approaches zero). This condition reflects the "limiting molar conductivity" (Λ_mº). It represents the molar conductivity of an electrolyte solution at infinite dilution, where interactions between ions are minimized.

Thus, the term used when the concentration of electrolyte approaches zero is: Limiting molar conductivity.

In chemistry, an ideal solution is one where the enthalpy of mixing is zero, and the volume of mixing is also zero. This typically occurs when the components have similar molecular sizes and intermolecular forces. Let's analyze the given solutions:

n-hexane and n-heptane: Both are alkanes with similar structures and intermolecular forces, likely to form an ideal solution.

Benzene and toluene: Both are aromatic compounds with similar sizes and van der Waals forces, likely to exhibit ideal behavior.

Bromoethane and chloroethane: Both are haloalkanes with similar structures, likely to form an ideal solution.

Ethanol and acetone: Ethanol is an alcohol with hydrogen bonding, while acetone is a ketone with dipole interactions. The difference in their intermolecular forces leads to non-ideal behavior.

Hence, the pair that does not behave like an ideal solution is ethanol and acetone.

To determine which ions will be colored in aqueous solution, we must understand the electronic configuration and the presence of unpaired electrons in these ions. Ions are colored due to electronic transitions between different energy levels, primarily within d-orbitals. This phenomenon occurs in transition metal ions where unpaired electrons are present.

Let's evaluate each ion:

• Ti³⁺: Titanium in the +3 oxidation state has the electronic configuration [Ar] 3d¹. The presence of 1 unpaired electron in the d-orbital makes it capable of d-d transitions, resulting in a colored solution.
• Nb³⁺: Niobium in the +3 oxidation state has the configuration [Kr] 4d². With 2 unpaired electrons, it can also undergo d-d transitions, therefore it will be colored.
• Cu⁺: Copper in the +1 oxidation state has the electronic configuration [Ar] 3d¹⁰. All d-orbitals are filled with paired electrons, precluding d-d transitions, and rendering the ion colorless.
• Y³⁺: Yttrium in the +3 oxidation state has the configuration [Kr]. With no d-electrons present, it lacks the ability for d-d transitions, making it colorless.

Therefore, only Ti³⁺ and Nb³⁺ exhibit color in aqueous solutions due to the presence of unpaired electrons allowing d-d transitions.

The correct answer is: (A) and (B) only

To determine the most powerful reducing agent in aqueous solution among the given metals, we need to consider their standard reduction potentials. A reducing agent donates electrons to another substance and gets oxidized in the process. The strength of a reducing agent is inversely related to its standard electrode potential, meaning that the metal with the lowest (most negative) standard reduction potential will be the most powerful reducing agent.

While based on standard electrode potentials, Lithium seems like it could be a candidate due to its highly negative potential, in practice, when considering their behavior in aqueous solutions and their reactivity, the metallic nature and solvation effects make potassium the most effective reducing agent among these choices.

Thus, in an aqueous solution, Potassium (K) acts as the most powerful reducing agent based on these considerations.

To identify a solid solution from the given options, we need to understand the concept of solutions in terms of phases:

1. A solution is a homogeneous mixture where the solute is uniformly distributed within the solvent. Solutions can exist in different phases: solid, liquid, or gas.
2. Solid solutions are those where both solute and solvent are in the solid phase. Typically, these solutions involve metals forming alloys, where the atoms of the solute metal are interspersed with the atoms of the solvent metal.

Now, let's evaluate each option:

• Camphor in N gas: This is a combination of a solid (camphor) and a gas (N ), forming a gaseous solution, not a solid solution.
• Oxygen gas in water: This is a liquid solution where a gas (oxygen) dissolves in a liquid (water).
• Ethanol in water: This is another example of a liquid solution, with both ethanol and water in the liquid phase.
• Amalgam of mercury with sodium: This is a solid solution. Here, mercury (typically liquid at room temperature) forms a solid phase with sodium, an example of a metal alloy where the solution exists in a solid form.

Thus, the correct example of a solid solution among the options is Amalgam of mercury with sodium.