Glycerol (C3H3O3), also called glycerine, is widely used in the food and pharmaceutical industries. Glycerol is polar and dissolves readily in water and polar organic solvents like ethanol. Calculate the mole fraction of the solvent in a solution that contains 1.31 g glycerol dissolved in 25.00 mL ethanol (CH3CH2OH; density = 0.7893 g/mL). Round to four significant digits. Nsolvent

Glycerol (C3H3O3), also called glycerine, is widely used in the food and pharmaceutical industries. Glycerol is polar and dissolves readily in water and polar organic solvents like ethanol. Calculate the mole fraction of the solvent in a solution that contains 1.31 g glycerol dissolved in 25.00 mL ethanol (CH3CH2OH; density = 0.7893 g/mL). Round to four significant digits. Nsolvent

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

See similar textbooks

Similar questions

A 690 g of 59% strontium bromide solution is cooled from 60 oC to a certain temperature. Upon addition of around 2 g of strontium bromide, excess solute above saturation started to crystallize. Total recovered crystals is 146.003 g. At what temperature is the solution cooled?
synthetic ion exchange resins. These resins are organic polymeric networks that contain functional groups that are permanently attached to the resin. One such functional group is sulfonic acid, -SO3H. When placed in water, the resin (being a large organic molecule) will not dissolve. However, the ionic functional groups become hydrated and the resin will swell as it takes up waters of hydration. The resin may then be thought of as a solid solution mixture with the functional groups being "dissolved" but the polymer remaining as a solid. The hydronium ion (H3O+) associated with acidic functional groups like sulfonic acid will dissociate just as it would if the acid were free of the resin. If other cations such as Cu2+ or Na+ are added to the resin, an ion-exchange reaction can occur: . Note that one H+ is released for each positive charge bound to the resin. Since the resin exchanges a hydrogen ion for a sodium ion in this reaction, sulfonic acid resins are called cation-exchange…
A polymer of large molar mass is dissolved in the organic solvent dimethylformamide (C3H7NO) at 25 °C, and the resulting solution rises to a final height of 10.8 cm above the level of the pure solvent, as solvent molecules pass through a semipermeable membrane into the solution. If the solution contains 3.80 g polymer per liter, calculate the molar mass of the polymer. Take the density of the solution to be 0.944 g cm-³. Molar mass polymer = g mol-1
C7H21O4NHCl(aq) + NaOH(aq) ---> C17H21O4N(aq) + H2O (l) + NaCl(aq) When a 25mL of aqueous solution that contains 62.50g of the salt is treated with NaOH, the salt is converted to pure cocaine. How much water in litres is needed additionally to dissolve the formed pure cocaine?
escriptionSolubility (soluble, insoluble, miscible & immiscible)25 mL of water and 1 g of salt—the resulting mixture is clear and colorless 25 mL of water and 1 g of solid silver chloride—the resulting mixture is cloudy and solid settles out. 25 mL of water and 5 mL of mineral oil—the resulting mixture is cloudy and gradually separates into two layers.
When the enthalpy of dissolution (Δ?°???) is positive, should solubility increase or decrease as the temperature is increased? Explain.
It is desired to prepare 2.5 m^3 of a 60 mol percent methanol - water solution. Determine the volumes of methanol and water required to be mixed at ambient temperature given that the partial molar volumes of methanol and water are 58.3x10^-6m^3/mol and 17.2 x 10 m^3/mol respectively. The density of the methanol is 782.51 kg/m^3. Do not use chatgpt. Thank you!
Hi there. Please help solve this. Thanks
You have two beakers. one contains pure water, the other contains pure methanol. The covalent bonds of methnol molecules are nonpolar. you pour crystals of stable salt into each beaker. Why will the table salt dissolve readily in water but will not dissolve in methanol?
In 200 words or less, give a real-world example of a colligative property of a solvent. How does mixing a solution with a solvent change the physical properties of that solvent. For example, salt is placed on ice on a snowy day to decrease the freezing point of the ice, preventing it from melting and becoming slick and causing accidents. The colligative property here is freezing point depression.
Based on the following data, determine the molecular weight of the unknown solute. Note the "initial freezing point" refers to the freezing point of the solvent as a pure substance while the "final freezing point" refers to the freezing point of the mixture. Mass Solvent: 15.000 g FPD Constant of Solvent: 4.9 Mass Solute 2.350 g Initial Freezing Point: 85.3oC Final Freezing Point: 82.4oC Your answer should follow the format: a) ΔT b) Molality of the Solution c) mols of solute d) Molecular weight of Solute
Consider a 250mL solution composed of 25% pentane by volume and 75%n-pentanol by volume. The following is a summary of the chemical and physical data for these two organic compounds. Pentane (CsH,12): bp = 36.1°C, MW = 72.15 g/mol, p = 0.626 g/mL n-Pentanol (CsH1,OH): bp = 138.5°C, MW = 88.15 g/mol, p = 0.814 g/mL %3D a) Can the components of the pentane/n- pentanol solution described above be effectively separated by simple distillation? No. A simple distillation cannot effectively separate these two components because simple distillations are only capable of separating liquid mixture when at least one of the components is water. No. A simple distillation cannot effectively separate these two components because their molecular weights are too similar Yes. A simple distillation can effectively separate these two components because their boiling points are sufficiently different. Yes. A simple distillation can effectively separate these two components because their densities are…