To find the concentration of a solution, we need to calculate the mass percentage of the solute in the solution. The mass percentage is defined as the mass of the solute divided by the total mass of the solution, multiplied by 100.
The total mass of the solution is the sum of the mass of the solute and the mass of the solvent.
\[ \text{Mass of solution} = \text{Mass of solute} + \text{Mass of solvent} \\ \text{Mass of solution} = 36 \text{ g} + 100 \text{ g} \\ \text{Mass of solution} = 136 \text{ g} \]The concentration in terms of mass percentage is given by the formula:
\[ \text{Concentration (mass %)} = \frac{\text{Mass of solute}}{\text{Mass of solution}} \times 100 \]Correct Option: D) 26.47% is the calculated concentration of the solution when 36 g of sodium chloride is dissolved in 100 g of water.
The question asks to identify which type of solution does NOT scatter light. This phenomenon is known as the Tyndall effect. We need to understand the characteristics of different types of mixtures (suspensions, colloids, and true solutions) and how their particle sizes relate to light scattering.
D) A true solution (e.g., salt water or sugar water)
True solutions have solute particles that are extremely small (less than 1 nm), typically individual molecules or ions. These particles are too small to scatter light effectively, so a beam of light passing through a true solution will not be visible. This is why salt water or sugar water appears clear and does not show the Tyndall effect.
The question asks for the definition and particle size range of a colloidal solution. We need to evaluate each option based on the characteristics of true solutions, colloids, and suspensions.
C) A heterogeneous mixture in which solute-like particles (1–100 nm) are distributed throughout the medium without settling — appears homogeneous but is actually heterogeneous. This option accurately describes a colloidal solution. It correctly identifies it as a heterogeneous mixture, specifies the particle size range (\(1\)-\(100 \text{ nm}\)), and notes that the particles do not settle, even though it may appear homogeneous.
The question asks to identify the correct list of colloids as mentioned in NCERT Class 9. To answer this, we need to recall the examples of colloids provided in the NCERT textbook and distinguish them from solutions and suspensions.
C) Milk, butter, foam, fog, smoke, clouds. This list exclusively contains examples of colloids as described and typically listed in the NCERT Class 9 Science textbook.
The question asks for the definition of the 'Tyndall Effect' in colloidal chemistry. We need to identify the option that correctly describes this phenomenon.
B) The scattering of a beam of light by the dispersed colloidal particles, making the path of light visible through the colloid
This option accurately describes the Tyndall Effect. When a beam of light passes through a colloidal solution, the dispersed colloidal particles scatter the light in all directions. This scattering makes the path of the light beam visible when viewed from the side. This phenomenon is named after John Tyndall, who extensively studied it.
The question asks for the technique used to separate components of a colloidal solution. We need to understand the properties of colloidal solutions and how different separation techniques work to identify the most suitable method.
Correct Option: D) Centrifugation is used to separate the components of a colloidal solution. The high centrifugal force causes the dispersed phase particles, which are larger than those in true solutions, to settle down, allowing for their separation from the dispersion medium.