1. Calculate the boiling point and freezing point of a solution containing 478 g of ethylene glycol (molar mass ethylene glycol 62.01 g/mol) in 3202 g of water. Kf = 1.86°C/m, %3D Kb = 0.52°C/m %3D

9. Calculate the boiling point of a solution of 500.0 g of ethylene glycol (C2H602) dissolved in 500.0 g of water. K/= 1.86°C/m and Kb = 0.512°C/m. Use 100°C as the boiling point of water.

The boiling point of water is 100.0°C at 1 atmosphere. How many grams of nickel(II) bromide (218.5 g/mol), must be dissolved in 275.0 grams of water to raise the boiling point by 0.400°C? Refer to the table for the necessary boiling or freezing point constant. Solvent Formula Kp (°C/m) Kf (°C/m) Water H20 0.512 1.86 Ethanol CH3CH,OH 1.22 1.99 Chloroform CHCI3 3.67 Benzene 2.53 5.12 Diethyl ether CH;CH,OCH2CH3 2.02 g nickel(II) bromide.

A solution is prepared disolving 2.00g of an substance in 10.0mL in water at 25°C. The freezing point of the substance is -0.350°C. Determine the molar mass of the substance. (Kf H2O=1.86°C) (Density H2O=0.9970g/mL)

Payal

What is the freezing point (in K) of a solution made by dissolving 19.543g of CCl4 in 130.0 g of benzene? Pure benzene has a freezing point of 5.5°C and a Kf = 5.12 °C/m.

-1 A certain liquid X has a normal freezing point of 5.90 °C and a freezing point depression constant K,=5.86 °C·kg•mol . Calculate the freezing point of a solution made of 20.1g of barium hydroxide (Ba(OH),) dissolved in 250. g of X. Round your answer to 3 significant digits. °C x10

The freezing point of water is 0.00°C at 1 atmosphere. How many grams of manganese(II) sulfate (151.0 g/mol), must be dissolved in 273.0 grams of water to reduce the freezing point by 0.350°C ? Refer to the table for the necessary boiling or freezing point constant. Solvent Formula Kp (°C/m) Kf(°C/m) Water H20 0.512 1.86 Ethanol CH3CH2OH 1.22 1.99 Chloroform CHC13 3.67 Benzene C6H6 2.53 5.12 Diethyl ether CH3CH2OCH,CH3 2.02 g manganese(II) sulfate.

16. Determine the cahnge in boiling point for 397.7 g of carbon disulfide (Kb= 2.34 degrees Celsius kg/mol) if 35.0 g of a nonvolatile, nonionizing compound is dissolved in it. The molar mass of the compound is 70.0 g/mol and the boiling point of the pure carbon disulfide is 46.2 degrees Celsius. a. 2.34 degrees Celsius  b. 5.88 degrees Celsius c. 24.8 degrees Celsius d. 2.94 degrees Celsius

A solution of 4.63 g of anhydrous aluminum chloride (AlCl3) in 59.08 g of water freezes at -4.37 degrees celsius. Kf (AlCl3) =1.86 degrees celsius/m part 1: calculate the molar mass of AlCl3 from the formula. Round the answer to the hundredths place. ___ g/mol Part 2: Calculate the molar mass from the freezing point depression, assuming AlCl3 does not dissociate in ions. Round to 3 Significant digits. Part 3: Comparing the two values, how many ions will AlCl3 form? Round the answer to the nearest whole number.