The question asks for the key difference between homogeneous and heterogeneous mixtures. We need to recall the definitions and characteristics of these two types of mixtures to identify the correct distinguishing factor.
A) A homogeneous mixture has uniform composition throughout; a heterogeneous mixture has non-uniform composition with physically distinct parts — This statement accurately defines and differentiates homogeneous and heterogeneous mixtures based on their composition and physical appearance. A homogeneous mixture, like sugar dissolved in water, looks the same throughout. A heterogeneous mixture, like sand in water, clearly shows separate components.
The question asks for the correct definition of a 'solution' in chemistry. We need to evaluate each option based on the fundamental characteristics of solutions, mixtures, and their components.
D) A homogeneous mixture of two or more substances in which the solute is uniformly distributed throughout the solvent. This accurately describes a solution, highlighting its homogeneous nature and the uniform distribution of solute particles.
This question asks about the characteristic particle size of solute particles in a true solution. Understanding the classification of mixtures based on particle size is crucial here. Mixtures are broadly classified into true solutions, colloids, and suspensions, each defined by a specific range of particle sizes.
Correct Option: B) Less than 1 nm (1 nanometre = 10⁻⁹ m)
This option correctly identifies the particle size of solute particles in a true solution. True solutions are characterized by extremely small solute particles, typically individual atoms, ions, or small molecules, which are uniformly dispersed and have a diameter less than 1 nm. This small size allows them to form a homogeneous mixture that does not scatter light and cannot be separated by filtration.
The question asks to define the terms 'solvent' and 'solute' in the context of a solution. Understanding the basic definitions of these components is crucial for answering this question.
A) Solvent: the component present in larger quantity that dissolves the other; Solute: the component present in smaller quantity that is dissolved
This option accurately defines both the solvent and the solute. The solvent is the major component that dissolves the solute, which is the minor component being dissolved. For example, in a sugar solution, water is the solvent (larger quantity, dissolves sugar) and sugar is the solute (smaller quantity, gets dissolved).
The question asks for the definition of a 'saturated solution'. We need to understand the concept of solubility and saturation in chemistry to identify the correct option.
D) No more solute can be dissolved in the solvent at a given temperature — the solvent has reached its maximum dissolving capacity
This option perfectly describes a saturated solution. It highlights that the solution has reached its limit for dissolving solute at a specific temperature, which is a crucial condition for saturation.
To determine the correct formula for mass percentage concentration, we need to recall the definition of concentration, specifically mass percentage. Concentration expresses the amount of solute in a given amount of solvent or solution. Mass percentage specifically deals with the mass of the components.
Correct Option: C) Mass percentage = (Mass of solute / Mass of solution) × 100
This option correctly represents the definition of mass percentage concentration, which is the ratio of the mass of the solute to the mass of the entire solution, expressed as a percentage.
This formula represents volume percentage concentration, not mass percentage. Mass percentage specifically uses mass units for both solute and solution.
This formula mixes mass and volume units (mass of solute, volume of solution). While it is related to concentration (e.g., mass/volume percent), it is not the standard definition of mass percentage, which requires both numerator and denominator to be in mass units.
This formula incorrectly uses the mass of the solvent in the numerator and the mass of the solute in the denominator. The numerator should be the mass of the solute, and the denominator should be the mass of the solution (solute + solvent), not just the solute.