B.Sc Chemistry Solutions — practice questions
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Practice B.Sc Chemistry Solutions in the app →Which statement correctly describes Raoult's law for an ideal solution of two volatile liquids A and B?Colligative properties of a dilute solution depend on:
The figure shows a non-ideal solution with *The molal boiling-point elevation constant of water is $K_b = 0.52$ K kg/mol. What is the boiling point of a s$36$ g of glucose ($M = 180$ g/mol) is dissolved in $200$ g of water. The molality of the solution is:The van't Hoff factor $i$ for a $0.01$ M aqueous solution of NaCl, assuming complete dissociation, is approximHenry's law for the solubility of a gas in a liquid is best stated as:Why are deep-sea divers given a breathing mixture of helium and oxygen instead of ordinary air?The mole fraction of urea ($M = 60\,\text{g/mol}$) in an aqueous solution containing $6\,\text{g}$ of urea in For an ideal solution containing two volatile liquids A and B, Raoult's law gives the total vapour pressure asFor a dilute solution of a non-volatile solute B in a solvent A, the relative lowering of vapour pressure equaThe elevation in boiling point of a solution is given by $\Delta T_b = K_b m$. The molal elevation constant $KThe freezing point of water is depressed when a non-volatile solute is added because:Osmotic pressure of a dilute solution is expressed by van't Hoff's equation as:Two solutions are said to be **isotonic** if they:If $\mathrm{NaCl}$ undergoes complete dissociation in water, the van't Hoff factor $i$ is:Benzoic acid associates in benzene to form dimers. The van't Hoff factor $i$ for benzoic acid in benzene (assuDesalination of sea water is best carried out by:A solution of glucose in water has a freezing point depression of $0.186\,\text{K}$. Given $K_f$ for water $= A solution showing positive deviation from Raoult's law has:Molarity M is defined as:Molality m is defined as:Mole fraction x_A is:Raoult's law for an ideal solution (one component A in solvent S) is:Henry's law for gas dissolution: solubility of a gas (mass m_gas per unit mass of solvent) is:Colligative properties depend on:What is the molarity of a solution containing 5.85 g of NaCl (M.W. = 58.5) in 250 mL of solution?Boiling point elevation: ΔT_b = K_b × m. For 1 molal aqueous urea (K_b = 0.52 K kg/mol), ΔT_b equals:Freezing point depression: ΔT_f = K_f × m. For 0.5 molal NaCl (assume full dissociation, K_f = 1.86), the deprVapour pressure of pure water at 25°C is 23.8 mm Hg. The vapour pressure of a solution with 18 g glucose (M.W.Osmotic pressure π = nRT/V (or CRT for molarity C). What is π for 0.1 M sugar solution at 27°C (R = 0.0821)?The van't Hoff factor i for a strong electrolyte like CaCl2 (full dissociation) is:In ideal solutions, ΔH_mix is:Mass percentage (w/w) of a solution: 12 g sugar in 100 g of solution is:Two solutions are isotonic if:For an azeotrope of HCl and water (boiling at 110°C with 20.2% HCl by mass), the composition and boiling pointMaximum boiling azeotropes are formed by mixtures with:Molality of a solution does not depend on:For 0.5 m solutions of NaCl, KCl, and BaCl2, which gives largest ΔT_f?Pure water boils at 100°C; pure ethanol at 78°C. A 0.5 mole fraction mixture under positive deviation will:Osmotic pressure of 0.1 M Glucose at 27°C is π_g. For 0.1 M NaCl at same T, the osmotic pressure is approximatThe pKa of a weak acid HA is 4.75. Find pH of an equimolar mixture of HA and A⁻:Solubility of N2 in water at 25°C is 6.8 × 10⁻⁴ mol/L at 1 atm partial pressure. By Henry's law, at 5 atm partTwo solutions A (0.1 M urea, π_A) and B (0.1 M NaCl, π_B). Water flows by osmosis:A solution boils at 100.5°C (water at 100). If K_b = 0.52, molality is:Mole fraction of solute in 18% glucose (180 g/mol) by mass in water:Vapour pressure of pure water is 100 (arbitrary units). Add 1 mole non-volatile solute to 9 moles water. New v