In an organic chemistry lab, some camphor crystals were synthesized but there were some traces of isoborneol also present in the crystals which lowered the melting point of the camphor crystals from 179 °C to 169 °C. Treating it as a solid-solid solution with isoborneol as the solute and camphor as the solvent, find the mass percentages of camphor and isoborneol in the solution. The freezing point depression constant for camphor is 40 °C kg mol1. The molecular weights of camphor and isoborneol are 152.2 g/mol and 154.3 g/mol respectively. A. 96.14 % and 3.86 % respectively B. 3.80 % and 96.20 % respectively C. 3.67 % and 96.33 % respectively D. 96.29 % and 3.71 % respectively E. 99.75 % and 0.25 % respectively

In an organic chemistry lab, some camphor crystals were synthesized but there were some traces of isoborneol also present in the crystals which lowered the melting point of the camphor crystals from 179 °C to 169 °C. Treating it as a solid-solid solution with isoborneol as the solute and camphor as the solvent, find the mass percentages of camphor and isoborneol in the solution. The freezing point depression constant for camphor is 40 °C kg mol1. The molecular weights of camphor and isoborneol are 152.2 g/mol and 154.3 g/mol respectively. A. 96.14 % and 3.86 % respectively B. 3.80 % and 96.20 % respectively C. 3.67 % and 96.33 % respectively D. 96.29 % and 3.71 % respectively E. 99.75 % and 0.25 % respectively

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 solution is prepared by dissolving 40.00 g of NaCl (f.w. = 58.44 g mol–1), a non-volatile solute, in enough water (m.w. = 18.02 g mol–1) to result in exactly 1 L of solution at 25 °C. Assume the density of the solution is that of pure water (dsolution = 1.000 g mL–1). The ebullioscopic constant (Kb) for water is 0.513 °C m–1. The cryoscopic constant (Kf) for water is 1.86 °C m–1. The vapor pressure of pure water is 0.0313 atm. Find the freezing point of the solution(in C to 2 decimal places)
Assuming 100% dissociation, calculate the freezing point (T) and boiling point (T) of 1.83 m K₂PO4(aq). Colligative constants can be found in the chempendix. Tf= Tb = °℃ °C
A solvent of Acetic Acid (CH3CO2H) is collected consisting of 0.4096 moles. The solute added consists of 0.18744g Ba(OH)2. Assume the change in temperature is 1.0°C. What is the freezing point depression constant (kf) of the solvent for this example. [CH3CO2H= 60.052 g/mol] [Ba(OH)2= 171.34 g/mol]
1-propanol and 2-propanol form an ideal solution at all concentrations at 25 °C. Letting the subscript 1 and 2 denote the 1- and 2- propanol, respectively, and given P1* = 20.9 torr and P2* =45.2 torr at 25 °C, calculate the mole fraction of 2-propanol in the vapor phase (y2) as a function of the mole fraction of 2- propanol in the liquid phase (x2). Plot y2 versus x2 for 0 < x2 < 1 (for plotting, increment x2 in steps or 0.05)
A solution of an unknown non-dissociating solute was prepared by dissolving0.300 g of the substance in 40.0 g of CCl4. The boiling point of the solution was0.357 °C higher than that of the pure solvent. Calculate the molar mass of thesolute. Kb=5.02 °C/m
8.71ml of a 4.00M HIO3(aq) solution is added to an ice-water mixture, and the freezing points were collected before and after addition of HIO3(aq). Once the temperature was stable after addition, the ice was separated from the solution and the mass of the beaker with solution was measured. The data below was recorded. Calculate the van't Hoff factor for HIO3. The freezing point depression constant for water is 1.86°C/m. Mass of beaker (g)l|Mass of beaker + solution (g T°f (°C)||Tf (°C) 87.438 176.179 0.305 ||-0.796
A solution made by dissolving 6.73 grams of an unknown organic acid in 110 grams of benzene. The normal freezing point of benzene is 5.45oC and the Kf = 5.07 oC/m. The solution had a final freezing point of 3.00 oC. Calculate the molecular weight of the solute.
1-propanol (n-propanol) and 2-propanol (isopropanol) form ideal solutions in all proportions. Calculate the partial pressure and the mole fraction (y) of the vapor phase of each component in equilibrium with each of the given solutions at 25 °C. Pprop=20.9 Torr and Piso = 45.2 Torr at 25 °C. A solution with a mole fraction of Xprop = 0.238. Pprop= Piso = yprop= Viso = A solution with a mole fraction of Xprop = 0.476. Pprop= Piso = yprop= Viso = A solution with a mole fraction of Xprop = 0.714. Pprop= Piso = yprop= Viso = Torr Torr Torr Torr Torr Torr
A polymer of large molar mass is dissolved in the organic solvent m-cresol (C7H8O) at 25 °C, and the resulting solution rises to a final height of 13.4 cm above the level of the pure solvent, as solvent molecules pass through a semipermeable membrane into the solution. If the solution contains 5.24 g polymer per liter, calculate the molar mass of the polymer. Take the density of the solution to be 1.03 g cm-3.