Colligative properties, need to calculate the molar mass of the unknown substance:
Can you please show the work for this problem?
Thanks!
Colligative properties, need to calculate the molar mass of the unknown substance: Can you please show the work for this problem? Thanks! 13 A solution was prepared by dissolving 59.82 g of an unknow...
2. A solution of an unknown molecular substance is prepared by dissolving 0.50 g of the unknown in 8.0 g of benzene. The solution freezes at 3.9°C. Determine the molar mass of the unknown. (Benzene has a freezing point of 5.5°C and a Kfvalue of 5.12°C/m) 10
1. A solution was prepared by dissolving 2.20g of urea (H2NCONH2) in 50.00g of water. If for H2O Tb = 100C, Tf = 0C, Kb = 0.52C / m and Kf = 1.86C / m, determine the freezing and boiling point of the solution. 2. A solution is prepared by dissolving 17.41g of a substance X in 600g of benzene and the resulting solution is frozen at 4.00C. If the freezing point of pure benzene is 5.55C and its Kf...
Question 27 (1 point)B A solution is prepared by dissolving 4.12 grams of a nonelectrolyte in 60.0 grams of water. If the boiling point of this solution is 100.15°C, what is the molar mass of the unknown substance? 844 g/mol 851 g/mol 0.351 g/mol 1.28 g/mol 234 g/mol
A solution is prepared by dissolving 11.10 g of an unknown non-electrolyte solute in 78.64 g of cyclohexane. The freezing point of the solution is found to be 2.06 oC. What is the molar mass of the unknown solute in g/mol? Please report your answer with 3 significant figures. Answer g/mol
. 0.275 L of solution is prepared by dissolving 2.50 g of an unknown molecular compound in enough water. The osmotic pressure of this solution is 1.98 atm at 27 °C. (R = 0.08206 L·atm/mol·K) a) Determine the molar mass of the molecular compound. (7 pts) b) If you need to prepare 0.275 L of AlCl3 solution with the same osmotic pressure of the above solution, what mass of AlCl3 (MW = 133.33 g/mol) would you need to weigh out?
Colligative properties, determination of the freezing point of a nonelectrolyte, unknown solution. 1. What is the freezing point depression for the unknown, nonelectrolyte solution? 2. How do you determine the molar mass of the unknown, nonelectrolyte compound for each trial, and what is the average molar mass for the unknown compound? Please help me figure this out? We performed experiment with the solution in a tube suspended in a bath of ice water and mixed solution/observed for freezing. Here is...
A solution is prepared by dissolving 0.107 g of an unknown non-electrolyte in 88.1 g of camphor. The freezing point of the solution was measured to be 178.0�C. What is the molecular weight of the compound? (The freezing point of pure camphor is 179.5�C and kf= 40�C/m)?
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...
Problem # 3: what is the molar mass of 35.0 g of an unknown substance that depresses the freezing point of 0.350 kg of water 0.50 °C? K, for water is 1.86 °C/m. [10 points
A solution is prepared by dissolving 3.04 g of an unknown nonelectrolyte in 16.00 g of cylcohexane (tf = 6.6 oC and kf = 20.0 oC/m). What is the molar mass of the unknown compound if the solution has a freezing point of -6.7 oC? Please see https://youtu.be/lwWZ5hdB61M for assistance. Mm = g/mol