Solutions

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A solution is a homogeneous mixture of two or more components that has uniform composition and properties throughout. The component present in the largest quantity is the solvent, and components prese…

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The six types are: 1) Gas in gas (N₂ and O₂ mixture), 2) Gas in liquid (O₂ in water), 3) Liquid in liquid (ethanol in water), 4) Solid in liquid (glucose in water), 5) Liquid in solid (mercury in sodi…

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Mass % = (mass of solute / total mass of solution) × 100. Step 1: Total mass = 20g + 80g = 100g. Step 2: Mass % of glucose = (20g / 100g) × 100 = 20%. Step 3: Mass % of water = (80g / 100g) × 100 = 80…

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Mole fraction (x) = moles of component / total moles of all components. Step 1: Molar mass of C₂H₆O = 46 g/mol, H₂O = 18 g/mol. Step 2: Moles of ethanol = 46/46 = 1 mol. Step 3: Moles of water = 90/18…

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Molarity (M) = moles of solute / volume of solution in liters. Step 1: Moles of NaCl = 5.85g / 58.5 g/mol = 0.1 mol. Step 2: Volume = 500 mL = 0.5 L. Step 3: Molarity = 0.1 mol / 0.5 L = 0.2 M. Answer…

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Molality (m) = moles of solute / mass of solvent in kilograms. Step 1: Molar mass of C₂H₄O₂ = 60 g/mol. Step 2: Moles of acetic acid = 2.5g / 60 g/mol = 0.0417 mol. Step 3: Mass of benzene = 75g / 100…

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Henry's Law: The partial pressure of a gas in vapor phase is proportional to the mole fraction of the gas in the solution. Mathematical expression: p = K_H × x. Where: p = partial pressure of gas, K_H…

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Step 1: Apply Henry's Law: x(N₂) = p / K_H = 0.987 bar / 76,480 bar = 1.29 × 10⁻⁵. Step 2: For 1 litre of water, moles of water = 55.5 mol. Step 3: x(N₂) = n(N₂) / (n(N₂) + 55.5) ≈ n(N₂) / 55.5 (since…