This question tests the skill of identifying solvent and solute in miscible liquid mixtures based on relative amounts. Acetic acid (5.0 mL) mixes completely with water (95.0 mL) to form a clear, homogeneous solution because both are polar and can form hydrogen bonds. Water is the solvent as it is present in much greater volume, while acetic acid is the solute. The resulting vinegar-like mixture is uniform, confirming miscibility. A tempting distractor is choice A, which reverses solvent and solute, based on the misconception that the added component is always the solvent regardless of quantity. In liquid-liquid mixtures, always designate the component in larger amount as the solvent and verify miscibility through polarity to ensure correct identification.

This question tests identification of solute and solvent when a gas dissolves in a liquid. When CO2 gas bubbles through water, some CO2 molecules dissolve in the water to form a homogeneous solution (carbonated water). In this solution, water is the solvent because it's the liquid medium doing the dissolving, while CO2 is the solute because it's the substance being dissolved. Choice D incorrectly claims gases cannot dissolve in liquids, when in fact many gases have measurable solubility in liquids (think of oxygen dissolved in water for fish to breathe). Remember that the physical state doesn't determine solvent/solute roles - the solvent is the dissolving medium (usually in greater amount) and the solute is what gets dissolved.

This question tests the application of "like dissolves like" for nonpolar substances. Iodine (I2) is a nonpolar molecular solid, and hexane (C6H14) is a nonpolar liquid solvent, so they are compatible and form a homogeneous solution. The nonpolar I2 molecules dissolve readily in hexane through London dispersion forces, creating a purple solution. Hexane is the solvent because it's the liquid medium present in larger amount (50 mL), while iodine is the solute being dissolved (1.0 g). Choice A incorrectly claims that molecular solutes don't dissolve in molecular solvents, when compatibility actually depends on matching polarities, not molecular versus ionic character. Remember that nonpolar solutes dissolve well in nonpolar solvents through dispersion forces.

This question tests the skill of identifying dissolution of ionic compounds in polar solvents and distinguishing solutions by uniformity. Potassium permanganate (KMnO4), an ionic solid, dissolves in water, a polar solvent, forming a uniformly purple homogeneous solution due to strong ion-dipole attractions. Water is the solvent as it is the large volume liquid in the beaker. The uniform color throughout confirms complete mixing at the molecular level. A tempting distractor is choice B, which claims a heterogeneous mixture because it's colored, stemming from the misconception that color indicates heterogeneity rather than dissolution. To classify colored mixtures, focus on uniformity and solubility principles, ignoring color as a factor for homogeneity.

This question tests the skill of recognizing solubility of polar covalent compounds in water and distinguishing solvent from solute. Sucrose, a polar covalent solid, dissolves completely in water, a polar solvent, forming a clear, uniform solution due to hydrogen bonding interactions between sucrose molecules and water. With 1.0 g of sucrose in 20 mL of water, water is the solvent as it is the abundant liquid component. The clarity and uniformity indicate a homogeneous solution. A tempting distractor is choice A, which names sucrose as the solvent, stemming from the misconception that the solid is always the solvent irrespective of quantity. To evaluate dissolution, consider molecular polarity and intermolecular forces, and designate the solvent as the component in greater amount for proper classification.

This question tests the skill of distinguishing between homogeneous solutions and heterogeneous mixtures, and identifying the solvent and solute in a solution. When 2.0 g of NaCl, an ionic solid, is added to 50 mL of water and stirred, it dissolves completely, forming a uniform mixture because NaCl is highly soluble in water due to ion-dipole interactions. In this homogeneous solution, water is the solvent as it is the component present in greater amount and the medium in which the solute dissolves. The mixture looks uniform with no visible particles, confirming it is a solution rather than a heterogeneous mixture. A tempting distractor is choice B, which incorrectly identifies NaCl as the solvent, stemming from the misconception that the solid component is always the solvent regardless of quantity. To identify solvents and solutes in mixtures, always consider the component in larger amount as the solvent and apply the principle that ionic compounds typically dissolve in polar solvents like water.

This question tests the skill of understanding solubility limits and identifying when a mixture remains heterogeneous due to insolubility. Calcium carbonate (CaCO3) has very low solubility in water, so even after stirring, a white solid remains at the bottom, indicating not all dissolves and forming a heterogeneous mixture. This is because the ionic compound does not sufficiently interact with water molecules to overcome lattice energy. The presence of undissolved solid confirms heterogeneity. A tempting distractor is choice B, which claims stirring always produces dissolution, based on the misconception that mechanical action alone determines solubility without considering chemical properties. When assessing solubility, evaluate the substance's inherent solubility product and observe for undissolved particles to differentiate between homogeneous and heterogeneous mixtures.

This question tests the skill of applying the 'like dissolves like' rule to predict solubility and identify solvents in nonpolar systems. Iodine, a nonpolar molecular solid, dissolves in hexane, a nonpolar solvent, forming a uniformly purple mixture because their similar nonpolar natures allow for dispersion forces to facilitate dissolution. In this homogeneous solution, hexane is the solvent as it is the liquid medium in larger amount. The uniform color without visible solids confirms complete dissolution. A tempting distractor is choice B, which identifies iodine as the solvent, based on the misconception that the colored or solid component dictates the solvent role. When dealing with nonpolar solutes and solvents, use the 'like dissolves like' principle and identify the solvent as the predominant liquid component to classify the mixture accurately.

This question tests the skill of recognizing gas solubility in liquids and identifying the solvent in gaseous solute systems. Carbon dioxide gas dissolves in water to form a clear, homogeneous solution, as CO2 molecules interact with water via dipole-induced dipole forces, and no bubbles are visible after shaking. In this solution, water is the solvent as it is the liquid medium containing the dissolved gas. The capped container and shaking enhance dissolution by increasing pressure and contact. A tempting distractor is choice B, which identifies CO2 as the solvent, arising from the misconception that the gaseous component acts as the solvent. To determine solution types with gases, consider the liquid as the solvent and check for uniformity and absence of phases to confirm homogeneity.

This question tests the skill of recognizing miscibility based on polarity and distinguishing homogeneous solutions from heterogeneous mixtures. Hexane, a nonpolar liquid, and water, a polar liquid, when mixed in equal volumes, form two distinct layers after settling because they are immiscible, following the 'like dissolves like' rule where polar substances mix with polar and nonpolar with nonpolar. This results in a heterogeneous mixture, as the components do not uniformly distribute. The observation of two layers confirms the lack of dissolution. A tempting distractor is choice A, which claims a homogeneous solution with hexane as solvent, based on the misconception that all liquids mix regardless of polarity. When evaluating mixtures of liquids, assess polarity compatibility and observe for phase separation to determine if the mixture is homogeneous or heterogeneous.