P5B2 In a study of the properties of an aqueous solution of Th(NO3) by A. Apelblat, D. Azoulay, and A. Sahar (J. Chem. Soc. Faraday Trans., I, 1618, (1973)), a freezing-point depression of 0.0703 K was observed for an aqueous solution of molality 9.6 mmol kg ¹. What is the apparent number of ions per formula unit? 50 10.0 10.0 22.0 24.0 acid with PS te
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- P5B.1 Potassium fluoride is very soluble in glacial acetic acid (ethanoic acid) and the solutions have a number of unusual properties. In an attempt to understand them, freezing-point depression data were obtained by taking a solution of known molality and then diluting it several times (J. Emsley, J. Chem. Soc. A, 2702 (1971)). The following data were obtained: b/(mol kg") 0.015 0.037 0.077 0.295 0.602 ΔΤΙΚ 0.115 0.295 0.470 1.381 2.67 Calculate the apparent molar mass of the solute and suggest an interpretation. Use AfH= 11.4kJ mol™ and T;* = 290 K for glacial acetic acid. lusThe mean activity coefficients of HBr in three dilute aqueous solutions at 25° C are 0.930 (at 5.0 mmol kg-1), 0.907 (at 10.0 mmol kg-1), and 0.879 (at 20.0 mmol kg-1). Estimate the value of B in the extended Debye-Hückel law, with C = 0.Referring to Fig. 5.8, deduce the molar solubility of (i) NH4Cl, (ii) (NH4)2SO4 in water at 25 °C.
- The vapour pressure of water in a saturated solution of calcium nitrate at 20 °C is 1.381 kPa. The vapour pressure of pure water at that temperature is 2.3393 kPa. What is the activity of water in this solution?Describe the general features of the Debye-Huckel theory of electrolyte solutions. Which approximations limit its reliability to very low concentrations?(b) CMC of a surfactant in water at 25 °C is 0.5 g L-¹ and at 45 °C is 0.3 g L-1. The molar mass of the surfactant is 110 g mol-¹. (i) Calculate: The Gibbs energy of micellisation, AGO, of the surfactant at 25 °C and 45 °C, The fractions (%) of the surfactant molecules in free and in micellar states in 0.5 g L-¹ aqueous solution of the surfactant and temperature 45 °C. ● ● (ii) Calculate CMC for the surfactant in water at 55 °C.
- Calculate the molar solubility of methane at 1.0 bar in benzene at 25 °C.Explain the origin of osmosis in terms of the thermodynamic and molecular properties of a mixture.The solubility of alum in 25 mL 1.4 M KOH plus 10 mL 9 M H2SO4 (our solution) is approximately 1.0 g at 1.0 °C, and 1.7 g at 6.0 °C. Estimate the amount of alum left in the solution if the temperature of the solution at the time of filtration was 5.0oC
- The mean activity coefficients of KCl in three dilute aqueous solutions at 25 °C are 0.927 (at 5.00 mmol kg−1), 0.902 (at 10.0 mmol kg−1), and 0.816 (at 50.0 mmol kg−1). Estimate the value of B in the Davies equation.b) Determine the standard enthalpy change and std. Gibbs free energy change of reaction at 400 k for the reaction СO(g) +2H2(g) — CHОН (g) At 298.15 K, AH.co (0)= -26.41 kcal/mol, AH AG.co (9)= -32.8079 kcal/mol, AG cH,oh(9)= -38.69 kcal/mol, °.CH20H(9)= -48.08 kcal/mol, The standard heat capacity of various components is given by, CO = a + bT + cT² + dT³, where C, is in cal/mol-K and T is in K b x10² с х105 d x10° Соmponent CH3OH а 4.55 2.186 -0.291 -1.92 CO 6.726 0.04 0.1283 -0.5307 H2 6.952 -0.0457 0.09563 -0.2079The standard molar entropies of water ice, liquid, and vapour at 298 K are 37.99, 69.91, and 188.83 J K-1 mol-1, respectively. On a single graph, show how the Gibbs energies of each of these phases vary with temperature; assume that the entropies themselves vary negligibly with temperature.