You have a 1.8M sodium phosphate solution , whose density is 1.13 g/ml. Calculate its: a) mol fraction. b) mass %. c) M...
1) Calculate the freezing point (°C) of a solution of 50 mL of acetone (CH3COCH3, Molar Mass = 58.08 g/mol, density 0.784 g/cm3) in 150g of CCl4, whose normal freezing point is -23.0 °C. Given: P = 1 atm, Kf CCl4 = 29.8 °C/m. Please show work. ------------------------------------------------------------------------------------------- 2) Calculate the boiling point (°C) at P = 1 atm of a solution of 25 g of acetone in 100 g of camphor whose normal boiling point is 204 °C. Kb...
Consider that you have 200.mL of 0.0500 M Na2SO4 solution in water. The density of the solution is 1.05 g/mL. a) What os the mass % of sodium sulfate in the solution? b) What is the ppm of the sodium sulfate in the solution? c) What is the molarity of ions in the solution assuming 100% dissociation? d) What is the molality of sodium sulfae in the solution? e) What is the molality of ions in the solution assuming 100%...
3. The density of a 4.53 M NH, solution is 0.9651 g/mL Calculate the molality 4. Calculate the freezing and boiling points of a solution made by mixing 10.5 g magnesium iodide with 150.0 g water. 5. A solution prepared by dissolving 0.56 g of a non-ionic solute in 25.0 g benzene freezes at 4.45°C. What is the molar mass of the solute?
Pure benzene, C6H6, has a molar mass of 78.114 g mol-1, a density of 0.8765 g mL-1, a freezing point of 5.45°C, and a boiling point of 80.2°C. Its freezing point depression and boiling point elevation constants are: Kf = 5.07°C m-1; Kb = 2.53oC m-1. A solution was made by taking 33.88 g of an unknown nonelectrolyte and dissolving it in 175.0 g of benzene. The measured freezing point of the solution was 1.65oC. Calculate the molar mass of...
Calculate the mole fraction of the solute of a 1.026 M aqueous solution of sodium phosphate with a density, ρ = 1.046 g/mL. Report your answer to THREE significant figures.
7. What is the mole fraction of urea, CH4N2O, in an aqueous solution that is 46% urea by mass? 8. What volume of a 0.850 M solution of CaCl2 contains 1.28 g of solute? 9. The volume of a 27.0% (by mass) solution is 162.9 mL. The density of the solution is 1.128 g/mL. What is the mass of solute in this solution? 10. Concentrated sodium hydroxide is 19.4 M and has a density of 1.54 g/mL. What is the...
29 You have a solution which is 43.4% by mass isopropyl alcohol (MM = 60.11 g/mol) in water. The density of this solution is 0.905 g/mL. a What is the molality of the isopropyl alcohol in the solution? > 1 point b What is the molarity of the isopropyl alcohol in the solution? > 1 point с What is the mole fraction of the isopropyl alcohol in the solution? > 1 point
The density of a 1.96 M solution of LiBr in acetonitrile (CH3CN) in 0.826 g/mL. Calculate the concentration of this solution in (a) molality, (b) mole fraction of LiBr, and (c) mass percent of CH3CN.
4a Calculate the molarity of an aqueous solution of sodium perchlorate with a solute mole fraction of 0.081 and a density, ρ = 1.078 g/mL. Report your answer to THREE significant figures. 4b Calculate the molarity of a 41.2% by mass aqueous solution of copper (I) sulfate with a density, ρ = 1.177 g/mL. Report your answer to THREE significant figures. 4c Calculate the mole fraction of the solute of a 4.211 m aqueous solution of cadmium (II) bromide with...
21. A sulphuric acid solution (H2SO4 : 98.09g/mol) is 5.83 M. This solution has a density of 1.329g/mL. Calculate the molality of the solution. 22. Calculate the freezing point and boiling point of the next solution: 0.35m glycerol (non-electrolyte) Kf-1.990C/m; TO S-114.6C; Kb0 x 1.220C/m; Tb0 x 78.4C.