Solutions

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A solution is a homogeneous mixture of two or more substances. Solvent is that component of a solution that has the same physical state as the solution itself (usually present in larger amount). Solut

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Molarity (M) is defined as the number of moles of solute dissolved per litre of solution. Formula: M = n/V, where n = moles of solute, V = volume of solution in litres. Molarity changes with temperatu

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Given: Mass of CH₃OH = 32.0 g, Volume = 200 mL = 0.2 L Molar mass of CH₃OH = 12 + 1×3 + 16 + 1 = 32 g mol⁻¹ Number of moles = 32/32 = 1 mol Molarity = n/V = 1/0.2 = 5 M

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Molality (m) is defined as the number of moles of solute dissolved per kilogram of solvent. Formula: m = (1000 × nB)/WA, where nB = moles of solute, WA = mass of solvent in grams. Unlike molarity, mol

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Normality (N) is defined as the number of gram equivalent weights of solute dissolved per litre of solution. Equivalent weight = Molecular weight/Valency. For acids: Eq. wt. = Mol. wt./Basicity. For b

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Mole fraction (X) is the ratio of moles of one component to total moles in solution. XA = nA/(nA + nB) Solution: Moles of H₂O = 36/18 = 2.0 mol, Moles of C₂H₅OH = 46/46 = 1.0 mol Total moles = 3.0 mol

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Henry's Law: The mass or mole fraction of a gas dissolved in a solvent is directly proportional to the partial pressure of the gas. Formula: x = Kp Conditions for validity: (1) Pressure is not too hig

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Vapour pressure is the pressure exerted by the vapour of a liquid when equilibrium is established between the liquid and vapour phases. At equilibrium, the rate of evaporation equals the rate of conde