measurement of mass and mole fraction

5) The volume of several aqueous copper sulfate (CuSO4) solutions was precisely measured at SATP. All of the solutions were made by adding copper sulfate to 100.00 g of water. ncopper sulfate (mol) Vsolution (mL) 0 100.18 0.0330 100.16 0.0696 100.36 0.111 100.81 0.156 101.62 First, estimate the concentration-dependent partial molar volume of copper sulfate in water by taking finite differences. Second, fit the data to a hyperbola and take a derivative of the hyperbola to accurately calculate the partial molar volume of copper sulfate in water at each concentration. Interpret the partial molar volume at infinite dilution - what must copper sulfate be doing to the nearby water molecules?

Given these values, find the initial mole fraction and initial mass % of the solute (sucrose) Solvent (water) weight: 200g Solute (NaCl) weight: 232g Solute (NaCl) Molar mass=342.3 moles of solute (NaCl) = .678

A solution of hexane and heptane at 30 C with hexane mole fraction of 0.305 has a vapor pressure of 95.0 torr and a vapor-phase hexane mole fraction of 0.555.  Fine the vapor pressures of pure hexane and heptane at 30 C.

You create an aqueous solution containing an unknown solute. Measuring the  osmotic pressure, you find it is 0.2 bar. Which of the following data would you need in order to find the boiling temperature of the solvent at room temperature?a. The molecular weight of waterb. The mass of the solute in the solutionc. The ebullioscopic constant for water d. The cryoscopic constant for water e. No additional data is necessary.

Assume that when you were transferring the mass of sodium chloride you measured to Test Tube 2, a smalle amount remained on the weighing paper, so that actual mass of NaCl you added to the tube was a bit smaller that the mass you thought you trasnferred. Describe how this error would affect each of the following values. a. The freezing poing depression that you measured. b. The motality that you calculated from your measurement of the freezing point depression. c. The molar mass of NaCl that you calculated from the molairty that you determined.

The experimental data in the table was collected during a freezing point depression study where BHT (butylated hydroxytoluene) was the solvent. Mass of BHT Mass of unknown Freezing point of pure BHT Freezing point of BHT and unknown solution Kf for BHT 7.709 g7.709 g 1.252 g1.252 g 74.17 ∘C74.17 ∘C 70.91 ∘C70.91 ∘C 6.83 ∘C/?6.83 ∘C/m Use this data to calculate the molar mass of the unknown solute. molar mass =

Could you help me with #4? I included a picture of the phase diagram that was given.

We have a solution that is formed with two substances, A and B. Here's the data : Molar fraction in substance : 0,357 for A, unknown for B Vapor pressure of the substance in its PURE state (kPa) : 42,5 for A, 23,9 for B Calculate the composition of the vapor phase in the most volatile substance.The values of the vapor pressures of the pure substances should give you an idea of the most volatile substance.Give an answer in mole fraction to 3 significant figures.

Given these values, find the initial mole fraction and initial mass % of the solute (Sucrose) Solvent (water) weight: 329g Solute (sucrose) weight: 232g Solute (sucrose) Molar mass=342.3 moles of solute (sucrose) = .678