For an ideal solution, which of the following is/are true? I. II. ΔΗ -0 AS = 0 III. Psolution =EPcomponents IV. AG = -R E (n¡ In x;) A. I and III only B. Il and IV only C. I, Il and III only D. III and IV only
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- The Henry’s law constant for CO2 in water at 25 °C is3.1x 10-2 M atm-1. (a) What is the solubility of CO2 inwater at this temperature if the solution is in contact withair at normal atmospheric pressure? (b) Assume that all ofthis CO2 is in the form of H2CO3 produced by the reactionbetween CO2 and H2O:CO2(aq) + H2O(l)------>H2CO3(aq)What is the pH of this solution?Please answer subparts d-e. Show solutions. ThanksThe freezing point of a 0.100 M acetic acid (CH3COOH) solution is determined to be-0.1878 C. Estimate the percent dissociation of acetic acid in this solution. Is it a strong orweak electrolyte? Note that acetic acid produces acetate (CH3COO-) and hydrogen (H+) ionswhen it is dissolved in water.
- Calculate the Gibbs free energy of the reaction from mixing 50 mL each of 0.50 M AgNO3(aq) solution and 1 M of NaCl(aq) to form AgCl(s) at 25°. The Ksp of AgCl is 6.0 × 10—11 at 25 °C.1.Calculate the normality of the solutions containing 5.267g/L K2Cr2O7 (the Cr is reduced to Cr3+).(FW=294.19 g/mol) 2.A and B react as follows: A + B 2C. The equilibrium constant is 5.0 x 106. If 0.40 mol of Aand 0.70 mol of B are mixed in 1L, what are the concentrations of A, B and C after reaction? 3. The following data is given at a certain temperature:(1) 2N2 (g) + O2 (g) 2N2O (g) K1 = 1.2 x 10-35(2) N2O4 (g) 2NO2 (g) K2 = 4.6 x 10-3(3) ½N2 (g) + O2 (g) NO2 (g) K3 = 4.1 x 10-9Calculate the molar equilibrium constant, K for the reaction:2N2O (g) + 3O2 (g) 2N2O4 (g)Calculate the Gibbs free energy of the reaction from mixing 50 mL each of 0.50 M Ag+(aq) solution and 1 M of NaCl(aq) to form AgCl(s) at 25°. The Ksp of AgCl is 6.0 × 10—11 at 25 °C.
- A public water supply was found to contain 0.8 partper billion (ppb) by mass of chloroform, .(a) How many molecules would be present in a350 mL glass of this water? (b) If the in part (a)could be isolated, would this quantity be detectable onan ordinary analytical balance that measures masswith a precision of g?30mL 0.9% v/v green food coloring. Transfer 2mL of of food coloring to flask, QS the flask to 100mL with DI water. What is the concentration of the standard?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)