TS EAPCET (Engineering) Solutions — practice questions
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Practice TS EAPCET (Engineering) Solutions in the app →Colligative properties of a dilute solution depend on:$36$ 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 approximA solution is best defined as:In a salt-in-water solution, the solvent is:The empirical rule 'like dissolves like' predicts that:Which of the following is **not** a colligative property?When a non-volatile solute is dissolved in a volatile solvent, the vapour pressure of the solution:The boiling point elevation $\Delta T_b$ of a dilute solution is:For an **ideal** solution, the enthalpy of mixing $\Delta_{mix}H$ is:Raoult's law for a volatile component of a solution states $P_i$ equals:With increase in temperature, the solubility of most gases in water:If 18 g of glucose (M = 180 g/mol) is dissolved in 90 g of water (M = 18 g/mol), the mole fraction of glucose Which gas does **not** obey Henry's law in water, because it reacts chemically with the solvent?The relative lowering of vapour pressure of a dilute solution of a non-volatile solute equals:If $K_b$ for water is 0.512 K·kg/mol, the boiling point elevation of a 0.50 molal aqueous urea solution is:A solution that shows **positive** deviation from Raoult's law typically has:Solutions are homogeneous mixtures of two or more components. In a binary solution, the component present in tAn amalgam of mercury with sodium is an example of which type of solution?Which of the following concentration units is *temperature-dependent*?The sum of mole fractions of all components in a solution equals:Molality (m) is defined as:Calculate the molality of a solution prepared by dissolving 2.5 g of ethanoic acid (CH₃COOH, M = 60 g mol⁻¹) iThe molarity of a solution containing 5 g of NaOH (M = 40 g mol⁻¹) in 450 mL of solution is:The mole fraction of ethylene glycol (C₂H₆O₂, M = 62) in a 20% by mass aqueous solution is approximately:If sea water (density 1.03 g mL⁻¹) contains 5.8 g of dissolved O₂ per 10⁶ g of water, the concentration is bes'Like dissolves like' implies that:If dissolution of a solid in a liquid is endothermic (Δ_sol H > 0), the solubility will:Solubility of gases in liquids generally:To increase the solubility of CO₂ in soft drinks, manufacturers:Raoult's law for a solution of two volatile liquids states that the partial pressure of component 1 is:For a binary solution of volatile liquids, the total vapour pressure can be written as:Raoult's law in its general form, for the solvent in a solution of a non-volatile solute, gives the relative lFor an ideal solution, both the enthalpy of mixing and the volume of mixing are:Which of the following is an example of a near-ideal solution?Solutions showing large **positive deviation** from Raoult's law form which type of azeotrope?Ethanol–water mixture, on fractional distillation, gives an azeotrope at approximately:HNO₃–water mixture forms a *maximum* boiling azeotrope at composition:Which of the following is NOT a colligative property?The four colligative properties all originate from:Elevation of boiling point (ΔT_b) is related to molality (m) by:For water, K_b = 0.52 K kg mol⁻¹. What is the boiling point of a solution of 18 g glucose (M = 180) in 1 kg waDepression of freezing point (ΔT_f) is given by:45 g of ethylene glycol (M = 62) is dissolved in 600 g of water. K_f(water) = 1.86 K kg mol⁻¹. The depression The osmotic pressure (Π) of a dilute solution is given by:Two solutions are termed *isotonic* if they:Blood cells placed in a hypertonic solution (e.g., > 0.9% NaCl) will:Why do wilted flowers revive when placed in fresh water?The van't Hoff factor (i) for a solute that completely dissociates into n particles is:For benzoic acid dimerising in benzene (2 CH₃COOH ⇌ (CH₃COOH)₂), the van't Hoff factor approaches:Inclusion of the van't Hoff factor modifies the boiling point elevation formula to:Experimentally, a solute is found to have a molar mass *lower* than its formula mass. This indicates the solutIn an antifreeze formulation, 35% (v/v) ethylene glycol in water lowers the freezing point of water to about: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: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:Maximum 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?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 vA solution is:Mole fraction of solute x_B in a binary solution:Molarity M is defined as:Molality m is defined as:Henry's law states partial pressure of a gas above liquid is proportional to:Raoult's law for ideal solution states vapor pressure of solvent:For dilute solutions, lowering of vapor pressure of solvent ΔP / P°_A =Elevation in boiling point ΔT_b for solution of non-volatile solute:Depression in freezing point ΔT_f for non-electrolyte solute:Osmotic pressure π for dilute solution:For NaCl in water (assumes complete dissociation), van't Hoff factor i =For 0.1 M urea in water, freezing point depression (K_f = 1.86):Mass percent of solute = (mass of solute / mass of solution) × 100. For 5 g NaCl in 95 g water:Two volatile liquids A (P°_A = 100) and B (P°_B = 200) form ideal solution. For x_A = 0.4, total vapor pressurOsmotic pressure of 0.01 M sucrose solution at 27°C (R = 0.0821 L atm/mol K):For solution of urea (M_w = 60 g/mol) with 6 g in 100 g water, molality:For 0.1 M acetic acid (Ka = 1.8 × 10⁻⁵), van't Hoff factor i is:For salt CaCl₂ (assume full dissociation), i =For a 1 m glucose aqueous solution (i = 1), boiling point:Freezing-point depression and elevation are colligative properties: depend on:Which description correctly defines a solution in chemistry?Which component of a solution determines the physical state in which the solution exists?A solution of hydrogen in palladium belongs to which solute-in-solvent type?German silver is a mixture of which metals?Fluoride ions in drinking water at about which level cause teeth to become mottled?A solution labelled 10% glucose in water by mass is made from what?A solute present only in trace amounts is most conveniently expressed in which unit?31% ethylene glycol (62 g/mol) by mass in water: mole fraction of glycol?How is the molarity of a solution defined?Which of these concentration terms changes with temperature?Find the molality of a solution of 6.0 g of urea (60 g/mol) dissolved in 250 g of water.Naphthalene dissolves readily in which of these solvents?No more solute dissolves at this temperature. What is the solution called?If dissolving a solid in a nearly saturated solution is endothermic, raising temperature does what to solubiliWhy does pressure barely change the solubility of solids in liquids?At constant temperature, Henry's law links the solubility of a gas in a liquid to which quantity?At a given pressure, a gas with a larger Henry's law constant KH has what solubility?Why do aquatic species prefer cold water to warm water?Soda bottles are sealed under high pressure to do what?The painful condition called bends in scuba divers is caused by bubbles of which gas in blood?Weakness and confused thinking in climbers caused by low blood oxygen at high altitude is called what?Gas solubility in a liquid falls as temperature rises because gas dissolution is what?A gas has KH = 50 kbar in water. What mole fraction of it dissolves at a partial pressure of 1 bar?