Solutions practice · Easy

The correct answer is A (Isohydric solutions) because isohydric solutions are defined as solutions having the same hydrogen ion concentration.

Potassium ferrocyanide, K4[Fe(CN)6], dissociates into the highest number of ions (5) in solution compared to the other options, resulting in the maximum van't Hoff factor, making option D the correct answer.

Option C (1 L of solution) is correct because molarity is defined as moles of solute per liter of solution.

Option B (The concentration of solute in the two liquids) is correct because the distribution law states that the ratio of solute concentrations in two immiscible liquids is constant.

Option C ($\Delta {S_{mix}} < 0$) is correct because for negative deviation, the entropy of mixing should be positive, not negative.

Option B ($0.1\;M$ sugar solution) is correct because sugar is a non-electrolyte, resulting in the smallest freezing point depression compared to the electrolyte solutions.

The correct answer is C (Temperature) because the vapor pressure of a liquid is directly related to its temperature.

Option D ($0.1\;m\;\mathrm{BaC}{\mathrm{l}_2}$) is correct because it has the highest van't Hoff factor, leading to the greatest lowering in vapor pressure.

Option B (83.5%) is correct because the degree of dissociation is calculated using the observed and calculated molecular weights and the van't Hoff factor.

Option B (Hypertonic solution) is correct because a hypertonic solution has a higher osmotic pressure compared to another solution.

Option A ($\frac{P}{5}$) is correct because the partial pressure of B is calculated based on its mole fraction in the mixture, considering the ratio of molecular weights.

Option B is correct because the freezing point is the temperature at which the vapor pressure of the liquid and solid phases are equal.

Option C is correct because the elevation in boiling point is calculated using the formula $\Delta T_b = K_b \times m$, where m is the molality of the solution.

Option D (All of these) is correct because the solubility of a gas in water depends on the nature of the gas, the temperature, and the pressure of the gas.

Option B (Freezing point will be highest for solution IV) is correct because the solution with the lowest total molality of ions will have the highest freezing point.

Option A ($6\mathrm{ }\;g\;\mathrm{ }of\;\;\mathrm{NaOH}/100$ $\mathrm{mL}$) is correct because it has the highest number of gram equivalents per liter of solution.

Option B (Nernst) is correct because Walther Nernst formulated the distribution law.

Potassium nitrate (KNO3) is a strong electrolyte and dissociates completely, while acetic acid (CH3COOH) is a weak electrolyte and only partially dissociates. Therefore, the osmotic pressure of KNO3 will be greater than that of CH3COOH, making option B the correct answer.

Option D (${P_B} + {X_A}\left( {{P_A} - {P_B}} \right)$) is correct because it correctly represents the total pressure of an ideal binary solution based on Raoult's law.

Option D is correct because $Na_3PO_4$ dissociates into the highest number of ions (4), leading to the greatest lowering of vapor pressure.

Option A ($CaC{l_2}$) is correct because it dissociates into three ions ($Ca^{2+}$ and $2Cl^−$), resulting in the highest van't Hoff factor and thus the highest osmotic pressure.

Option C (45.0 g conc. HNO3) is correct because it is calculated by determining the mass of HNO3 needed and then accounting for the concentration of the stock solution.

Parts per million (ppm) is the appropriate unit for expressing concentrations of solutes present in trace amounts, making option D the correct answer.

Option C (Associated) is correct because the depression in freezing point is half of what is expected, indicating that two molecules of B are associating into one particle.

Option C (Acetonitrile and acetone) is correct because both acetonitrile and acetone are polar molecules and exhibit dipole-dipole interactions as the major intermolecular force.

Option D (Both (1) and (3 )) is correct because the solvent is present in large excess and determines the physical state of the solution.

Option C (Assertion is true but Reason is false) is correct because osmotic pressure is a colligative property, and the osmotic pressure of 0.1 N urea is less than that of 0.1 M NaCl.

Option C (Molal ebullioscopic constant) is correct because it is the elevation in boiling point for a one molal solution.

Option D (The concentration of the solute in both the solvents must be kept high) is wrong because the distribution law is most accurate at low solute concentrations.

Option A (8) is correct because there are 8 possible combinations of dispersed phase (solid, liquid, gas) and dispersion medium (solid, liquid, gas), excluding gas in gas.