. Answer Only Refer to the following mixtures: Mixture A: Liquid and solid mixture Mixture B. Liquid mixture whose boiling points are similar. Mixture C. Liquid mixture with high boiling point. Mixture D. Heat sensitive liquid mixture. Which of the following distillation can be applied for Mixture D? vacuum distillation fractional distillation simple distillation none of these ———— This is defined as the temperature at which the vapor pressure of the liquid phase of a compound equals the external pressure acting on the surface of the liquid. solubility melting point boiling point flash point optical rotation —————— Predict the color change if 1% ferric chloride (yellowish solution) is added to a test tube containing a mixture of ethanol and pure acetyl salicylic acid. purple to yellow yellow to dark blue light blue to pink yellow to purple no color change

The strongest solute-solvent interaction that exists when calcium chloride dissolves in water is a(n)… a. dipole-dipole force b. dipole-induced dipole force c. dispersion force d. hydrogen bond e. ion-dipole force

Any additional information is attached

1.  A 4 M acetic acid (CH3COOH) solution lowers the freezing point by -8oC;    a 4 M KF solution yields a -15oC freezing point depression.  What can account for this difference?   2. Based on what you have studied about intermolecular forces, predict which of the following liquid has the highest boiling point and why. All three compounds have comparable molecular weights.   Butane, C4H10                          b.  Propanol, C3H7OH          c. Acetone, CH3COCH3

The boiling point of water is 100.0°C at 1 atmosphere. How many grams of silver acetate (166.9 g/mol), must be dissolved in 224.0 grams of water to raise the boiling point by 0.400 °C? mpor Refer to the table for the necessary boiling or freezing point constant. Solvent Kb (°C/m) Kf(°C/m) 0.512 1.22 Chloroform CHCl3 3.67 Benzene C6H6 2.53 Diethyl ether CH3 CH₂ OCH2 CH3 2.02 g silver acetate Water Ethanol Mass = this Formula H₂O CH3CH₂OH 1.86 1.99 5.12

Suppose that you have a 1:1 mixture of compounds that is comprised of compound X and compound Y. You desire pure compound X and are planning a recrystallization to enhance the purity. Which solvent below is optimal for your recrystallization?      Ethanol (boiling point = 78 °C)   Solubility At   0  °C 100  °C Compound X 0.05 g/mL 0.20 g/mL Compound Y 0.02 g/mL 0.40 g/mL           Water (boiling point = 100 °C)   Solubility At   0  °C 100  °C Compound X 0.02 g/mL 0.05 g/mL Compound Y 0.01 g/mL 0.10 g/mL           Methanol (boiling point = 65 °C)   Solubility At   0  °C 65  °C Compound X 0.04 g/mL 0.10 g/mL Compound Y 0.02 g/mL 0.30 g/mL         Acetone (boiling point = 56 °C)   Solubility At   0  °C 56  °C Compound X 0.10 g/mL 0.50 g/mL Compound Y 0.20 g/mL 0.50 g/mL         Ethyl Acetate (boiling point = 77 °C)   Solubility At   0  °C 77  °C Compound X 0.10 g/mL 0.60 g/mL Compound Y 0.30 g/mL 0.60…

Suppose you want to purchase a syrup containing water and sugar and you have two brands from which to choose. If you want to purchase on the basis of highest sugar content, which should you buy?  The syrup with the highest freezing point. The syrup with the highest boiling point. Why?

Determine the boiling point (in °C) of a solution that contains 45.5 g of MgCl2 dissolved in 685 mL of ethanol (density = 0.789 g/mL). Pure ethanol has a boiling point of 78.3°C and a Kp = 1.07°C/m. %3D

In the distillation of a pure substance ( e.g., water), why doesn't all the water vaporize when the boiling point is reached?

Can you please help me solve this problem?  I am having trouble figuring out the process to solve this.   Water has a molal freezing point constant of 1.86 degrees Celsius kg/mol.  Calculate the freezing point of 46.7 grams of Calcium chloride in 150.469 grams of water.  Assume complete disassociation.