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- A mixture combining 60 mL ethanol (C₂H6O) with 75 mL water (H₂O) is prepared at 280 K. The partial molar volumes of ethanol (E) and water (W) when mixed in these proportions (right column below) and in pure form (left column below) are ethanol water pure substance molar volume 58.2 mL/mol 18.00 mL/mol partial molar volume 55.3 mL/mol 17.7 mL/mol Determine the volume of the ethanol-water mixture. [Hint: You will need to determine the moles of each component.]A student determined the molar mass of an unknown ionic solid by the method used in this experiment. She found the equilibrium temperature of the ice water mixture (THE FREEZING POINT) to be 0.50°C on her thermometer. When she added 3.10 g of her solid to the mixture, the temperature fell to -4.30°C. She then poured off the solution into a beaker. The mass of the solution was 34.59 g. Kf = 1.86°C/m What was the freezing point depression ∆Tf (celsius) What was the molality of the unknown solution? How much water was in the solution? What did she find to be the observed molar mass of the ionic solid, assuming she made the calculation properly?The solubility of AgCl in water at 25 °C is measured to be 0.0019 Round your answer to 2 significant digits. x10 X 5 Use this information to calculate Ksp for AgCl.
- What is AG for the decomposition of CaCO3 at 298 K and a partial pressure of CO2 of 4.00x10-4 bar? CaCO3(s) → CaO(s) + CO2(g) AGrxn (298 K, Pco2 = 0.400 mbar) = ??? CO2(g) Compound AG°; (kJ mol·1) CACO3(s) СаО(s) -1129 -604 -394In the standardization of HCl using pure anhydrous sodium carbonate as the primarystandard for methyl orange as an indicator, 1.0 mL HCl was found to be equivalent to 0.05gof sodium carbonate (MW =106). The normality of HCl is:7. The solubility, C, of sucrose in water, expressed as grams of sucrose per 100 g of solvent, is given as below t/°C C/g 0 179.2 10 20 203.9 190.5 30 219.5 [ΔΗ (a) Draw an appropriate graph to determine the molar enthalpy of solution of sucrose in the temperature range 0 to 40°C. (b) 50mL of saturated solution of benzoic acid at 25°C requires 12.8 mL of 0.05 M NaOH to completely neutralize. What is the solubility of benzoic acid in g/L water at 25°C. so ln,m 40 238.1 = 4.96 kJ/mol, Cbenzoic acid = 1.56g/L]
- 4G 72% 4:37 = bartleby Q&A Science / Chemistry / Chemic... / 11th Ed... : A student determined the molar m... A A student determined the molar mass of an unknown non-dissociating liquid by the method described in this experiment. She found that the equilibrium temperature of a mixture of ice and pure water was indicated to be +0.4°C on her thermometer. When she added 9.9 g of her sample to the mixture, the temperature, after thorough stirring, fell to -3.7°C. She then poured off the solution through a screen into a beaker. The mass of the solution was 84.2 g. a. What was the freezing point depression? °C b. What was the molality of the unknown liquid? m c. What mass of unknown liquid was in the decanted solution? d. What mass of water was in the decanted solution?The amount of oil and grease from the rivers beside mining sites are quantified by solvent-solvent extraction. The dissolved oil and grease from the organic solvent will then be dried and weighed. What type of gravimetry is described by the statement? O precipitation gravimetry O physical gravimetry thermogravimetry electrogravimetry1.Define binary mixture 2. Define density 3. Give an abstract of determination of excess molar volume of binary mixtures of water and methanol by measuring density
- Pure potassium hydrogen phthalate is used for the standardization of the sodium hydroxide solution. Suppose that the potassium hydrogen phthalate is not completely dry. Will the reported molar concentration of the sodium hydroxide solution be too high, too low, or unaffected because of the moistness of the potassium hydrogen phthalate? Explain.(A) It is required to separate 1 mole of ethanol from ethanol-water mixture by using distillation Column at standard conditions. After 1 hour, it is found that the volume was double and the pressure increased to 152 kpa. Find the Temperature after 1 hour by using the ideal gas law: PV = nRT Given : R = 0.082 L.atm/mole.K (B) Calculate the capacity of a Base added to a solution contains 10 mole of ammonia (k, = 1.8x105) and 6 mole of ammonium chloride in 120 ml? Note: Atomic weight: H = 1, 0 = 16, C = 12, Ba = 137, Cl= 35 , N=14Calculate the following: (a) The bubble-point temperature of an equimolar mixture of liquid n-hexane and n-heptane at 1.0 atm and the composition (mole fractions) of the vapor in equilibrium with this mixture. (b) The dew-point temperature of a gas mixture with a molar composition of 30% n-hexane, 30% n-heptane, and 40% air at 1 atm and the composition (mole fractions) of the liquid in equilibrium with this mixture.