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- A beaker holds 48 mL of acetone (solute) and 111 mL of water (solvent). Calculate the v/v% of acetone in the solution. Report answer with correct sigfigs and units.State raoult's law for a non volatile solute in single volatile solvent?Which of the following statements is(are) true? Correct the falsestatements.a.The vapor pressure of a solution is directly related to the mole fractionof solute.b. When a solute is added to wate1 the water in solution has a lowervapor pressure than that of pure ice at 0°C.c. Colligative properties depend only on the identity of the solute and noton the number of solute particles present.d. When sugar is added to water, the boiling point of the solutionincreases above 100°c because sugar has a higher boiling point than water.
- 180.37 mL of 1.10 M organic salt was mixed with 185.23 mL of Ethanol (d= 0.789 g/mL, MW 46.07g/mole). Pure ethanol has a vapor pressure of 0.059 atm what will be the vapor pressure of the solution? (round your answer to 3 decimal places, no need to write the unit)How many mL of isopropyl alcohol are needed to make 292 mL of a 70 % (v/v) solution? Give answer as a whole number; no decimals. Round appropriately. Include appropriate unit.need this answer with explanation Considera mixture prepared by adding 0.1 moles of benzoic acid,and 1.5 moles of diethyl etherWhich of the following statements is false concerning the resulting mixture? A. The solution exhibits positive deviations from Raoult's law B. ∆H for the solution should be endothermic C. The intermolecular forces are stronger in solution than in either pure diethyl ether or pure benzoic acid. D. Molecules in the solution have a higher tendency to escape. E The solution with x =0.5 will have a lower boiling point than either pure diethyl ether or pure benzoic acid. need explanation for all Statements
- 1 kg solution of aqueous oxalic acid was made by dissolving 10g of C2H2O4 and is used as a disinfectant. The disinfectant was made at 30oC and is 3.5% dissociated. Determine: (a) Vapor pressure of solution (b) Boiling pt. of solution (c) Freezing point depression (d) Osmotic pressurea) What would you expect the magnitude and sign of ΔHSOLUTE, ΔHSOLVENT, and ΔHMIXING to be for CH2Cl2 as solute and acetone as solvent? Circle your choices below. Then, fill in the most important IM force that exists between solute molecules, between solvent molecules and between solute and solvent molecules. b) Based on this, what is the overall enthalpy change (HSOLUTION) for dissolving CH2Cl2 in acetone expected to be? (negative/positive/ near zero). Would you expect CH2Cl2 to dissolve in acetone? (yes/no). Explain your answers to both of the questions above. Consider the energy and entropyPlease indicate true (T) or false (F) as appropriate: Justify I) The vapor pressure of a solvent is reduced by the presence of a non-volatile solute II) In an ideal solution, the vapor pressure is increased by the presence of a solute Volatile. III) Sea water freezes at a lower temperature than sugar water. IV) In the laboratory, chemists use this effect to judge the purity of a component solid: if impurities are present, the freezing point of the compound is lower than the accepted value. A) TFTF B) TTFT C) FTFF D) TTTT
- 4.72 grams of an involatile nonelectrolyte with chemical formula C7H6O2 is dissolved in 35.5 grams of tert-butanol (C4H10O) to make a solution. If the boiling point of the pure tert-butanol is 80.1 °C, and tert-butanol has a molal boiling point elevation constant (Kb) of 1.11 °C*kg/mole, what is the boiling point of the solution?Two organic solvents (A and B) form an ideal solution when they mixed at 25 °C. The vaporpressures of A and B solvents at 25 °C are 500 and 180 mmHg, respectively. By mixing 30 mLof A (d=0.64 g/mL) with 48 mL B (d=0.67 g/mL), an ideal solution is prepared.(a) What is the vapor pressure of resulting ideal solution?(b) What is the composition by mole fraction of A in the vapor that is in equilibrium withthis solution? (Mw of A= 72.15 g/mol; Mw of B= 86.17 g/mol)Calculate the freezing point of a solution made by adding 18.59 g of a nonelectrolyte (115.4 g/mol) to 1 kg of solvent? The freezing point of the solvent is 3.36ºC and the freezing point depression constant of the solvent is 4.82 ºC/m. Report your answer to the hundreths place and do not include units.