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- What mass of a non-electrolyte solute is required, when mixed with 225 g H2O, to change the equilibrium vapor pressure of H2O from 1.013 x 105 Pa to 8.104 x104 Pa, at approximately 110 °C? The molar mass of the non-electrolyte solute is 62.07 g mol−1. Assume ideal behaviour for the solution.Consider a mixture of two liquids A and B (i.e., a solution of A+B). How many degrees of freedom are required to define a system where the solution is in equilibrium with both solids (solid A+ solid B)? What is/are the relevant intensive variable(s)?(3 is not the ansewer)A solution is prepared by dissolving 40.00 g of NaCl (f.w. = 58.44 g mol–1), a non-volatile solute, in enough water (m.w. = 18.02 g mol–1) to result in exactly 1 L of solution at 25 °C. Assume the density of the solution is that of pure water (dsolution = 1.000 g mL–1). The ebullioscopic constant (Kb) for water is 0.513 °C m–1. The cryoscopic constant (Kf) for water is 1.86 °C m–1. The vapor pressure of pure water is 0.0313 atm. Find the freezing point of the solution(in C to 2 decimal places)
- A solution is prepared by dissolving 40.00 g of NaCl (f.w. = 58.44 g mol–1), a non-volatile solute, in enough water (m.w. = 18.02 g mol–1) to result in exactly 1 L of solution at 25 °C. Assume the density of the solution is that of pure water (dsolution = 1.000 g mL–1). The ebullioscopic constant (Kb) for water is 0.513 °C m–1. The cryoscopic constant (Kf) for water is 1.86 °C m–1. The vapor pressure of pure water is 0.0313 atm. Find the vapor pressure of the solution to 3 decimal places in atm.A solution is prepared by dissolving 40.00 g of NaCl (f.w. = 58.44 g mol–1), a non-volatile solute, in enough water (m.w. = 18.02 g mol–1) to result in exactly 1 L of solution at 25 °C. Assume the density of the solution is that of pure water (dsolution = 1.000 g mL–1). The ebullioscopic constant (Kb) for water is 0.513 °C m–1. The cryoscopic constant (Kf) for water is 1.86 °C m–1. The vapor pressure of pure water is 0.0313 atm. Find the osmotic pressure in atm to three decimal placesA solution is prepared by dissolving 40.00 g of NaCl (f.w. = 58.44 g mol–1), a non-volatile solute, in enough water (m.w. = 18.02 g mol–1) to result in exactly 1 L of solution at 25 °C. Assume the density of the solution is that of pure water (dsolution = 1.000 g mL–1). The ebullioscopic constant (Kb) for water is 0.513 °C m–1. The cryoscopic constant (Kf) for water is 1.86 °C m–1. The vapor pressure of pure water is 0.0313 atm. Determine the boiling point of the solution(in C to 2 decimal places)
- A solution is prepared by dissolving 40.00 g of NaCl (f.w. = 58.44 g mol–1), a non-volatile solute, in enough water (m.w. = 18.02 g mol–1) to result in exactly 1 L of solution at 25 °C. Assume the density of the solution is that of pure water (dsolution = 1.000 g mL–1). The ebullioscopic constant (Kb) for water is 0.513 °C m–1. The cryoscopic constant (Kf) for water is 1.86 °C m–1. The vapor pressure of pure water is 0.0313 atm. Determine the following: Boiling point of solution (in °C to two decimal places) Freezing point of solution (in °C to two decimal places) Vapor pressure of the solution (in atm to three decimal places) Osmotic pressure (in atm to three decimal places)A saturated solution of copper (II) sulfate, with excess of the solid, is present in equilibrium with its vapor in a closed vessel. a) How many phases and components are present? b) How many degrees of freedom are available, and what are they? c) How would the degrees of freedom change if there was no excess of solid solute present?The osmotic pressure of an aqueous solution of a non-ionic solute is 120 kPa at 300 K. Assuming that the molarity and molality of the solution are essentially equal for dilute solutions, calculate the temps at which this solution freezes and boils. (Kf(H2O)= 1.86 °/m, and Kb(H2O)= 0.512 °/m)
- An excess amount of Ba(NO3)2 was added to 2 liters of water at 25 oC until the solution is saturated. Because Ba(NO3)2 is only slightly soluble in water, the excess Ba(NO3)2 was filtered out to get a solid-free mixture. The proponents of the experiment thought about using the concept of colligative properties, specifically boiling point elevation, to determine Ksp. It was observed in their experiments that the solution boils at 100.15 deg C. Kb of water = 0.51 K-kg/mol. Barium nitrate dissociates using: Solve the ff: a) Amount of Ba(NO3)2 dissolved in grams. MW of Ba(NO3)2 = 261.3 g/molb) Solubility product, Kspc) Vapor pressure of the solution in kPa(i) Gas (A) is more soluble in water than Gas(B) at the same temperature. Which one of the two gases will have the higher value of KH(Henry’s constant) and why?(ii) In non-ideal solution, what type of deviation shows the formation of maximum boiling azeotropes?Determine the vapor pressure of benzyl alcohol at 462.3 K in Pa.