Question

1. Calculate the molar mass of an unknown solid (assume a non-electrolyte), if 1.35 grams of...

1. Calculate the molar mass of an unknown solid (assume a non-electrolyte), if 1.35 grams of the solid was dissolved in 15. grams of dodecanol and caused a freezing point depression of 2.34 degrees C. the freezing point constant, k_f_ is 2.9 degree C.

2. (use information from #1) Calculate the molar mass of this compound if it were actually an ionic compound that dissociates into two parts (i.e. BX->B^+ +X^-).

freezing point of dodecanol is 27.5 C

Homework Answers

Answer #1

1)

freezing point depression = 2.34 oC

Kf = 2.9

delta Tf = Kf x m

2.34 = 2.9 x m

m = 0.807 m

molality = 0.807 m

moles of solute / mass of solvent in kg = 0.807

n / 0.015 = 0.807

n = 0.0121

mass / molar mass = 0.0121

1.35 / M = 0.0121

molar mass = 111.5 g/mol

2)

delta Tf = i x Kf x m

2.34 = 2 x 2.9 x m

m = 0.403 m

molality = 0.403 m

moles of solute / mass of solvent in kg = 0.403

n / 0.015 = 0.403

n = 6.05 x 10^-3

mass / molar mass = 6.05 x 10^-3

1.35 / M =6.05 x 10^-3

molar mass = 223 g/mol

Know the answer?
Your Answer:

Post as a guest

Your Name:

What's your source?

Earn Coins

Coins can be redeemed for fabulous gifts.

Not the answer you're looking for?
Ask your own homework help question
Similar Questions
An aqueous solution containing 17.5 g of an unknown molecule (non electrolyte) compound in 100 g...
An aqueous solution containing 17.5 g of an unknown molecule (non electrolyte) compound in 100 g water has a freezing point of -1.8 degrees Celsius. Calculate the molar mass of the unknown compound
An aqueous solution containing 35.0 g of an unknown molecular (non-electrolyte) compound in 156.9 g of...
An aqueous solution containing 35.0 g of an unknown molecular (non-electrolyte) compound in 156.9 g of water was found to have a freezing point of -1.2 ∘C. Calculate the molar mass of the unknown compound. Calculate the molar mass of the unknown compound.
An aqueous solution containing 36.2 g of an unknown molecular (non-electrolyte) compound in 146.1 g of...
An aqueous solution containing 36.2 g of an unknown molecular (non-electrolyte) compound in 146.1 g of water was found to have a freezing point of -1.2 ∘C. Calculate the molar mass of the unknown compound.
An aqueous solution containing 36.2 g of an unknown molecular (non-electrolyte) compound in 152.4 g of...
An aqueous solution containing 36.2 g of an unknown molecular (non-electrolyte) compound in 152.4 g of water was found to have a freezing point of -1.4 ∘C. Calculate the molar mass of the unknown compound. Express your answer using two significant figures.
An aqueous solution containing 36.3 g of an unknown molecular (non-electrolyte) compound in 144.2 g of...
An aqueous solution containing 36.3 g of an unknown molecular (non-electrolyte) compound in 144.2 g of water was found to have a freezing point of -1.2 ∘C.Calculate the molar mass of the unknown compound.
a) When 1.13 g of an unknown non-electrolyte is dissolved in 50.0 g of carbon tetrachloride,...
a) When 1.13 g of an unknown non-electrolyte is dissolved in 50.0 g of carbon tetrachloride, the freezing point decreased by 5.46 degrees C. If the Kfp of the solvent is 29.8 K/m, calculate the molar mass of the unknown solute. b) How many moles of solute particles are present in 4.78 mL of 0.304 M (NH4)2SO4? c) A 0.97 mass % aqueous solution of urea (CO(NH2)2) has a density of 1.12 g/mL. Calculate the molarity of the solution. Give...
When 20.0 grams of an unknown nonelectrolyte (i=1) compound are dissolved in 500.0 grams of benzene,...
When 20.0 grams of an unknown nonelectrolyte (i=1) compound are dissolved in 500.0 grams of benzene, the freezing point of the resulting solution is 3.77 °C. The freezing point of pure benzene is 5.444 °C and the Kf for benzene is 5.12 °C/m. What is the molar mass of the unknown compound?
A solution was prepared by dissolving 1.000 g of an unknown non-electrolyte in 50.00 g of...
A solution was prepared by dissolving 1.000 g of an unknown non-electrolyte in 50.00 g of CCl4. The freezing point of the solution was found to be -28.4°C. What is the molar mass of this unknown solute? (The freezing point of pure CCl4 is -22.3°C, and Kf for CCl4 is 29.8°C.kg/mol.)
Molar Mass by Freezing Point Depression. What is the effect on your calculated molar mass if...
Molar Mass by Freezing Point Depression. What is the effect on your calculated molar mass if the following happened: a. 2.000g of an unknown solute was added to the solvent instead of 1.200g as directed, but 2.000g was used in the calculations. (All 2.000g dissolved in the solvent.) b. The unknown solute reacted with the t-butanol solvent and fragmented into two approximately equal sized molecules. c. Too much solid was put into the solvent- it dissolved when hot, but much...
Analysis of a non-electrolyte, unknown compound, X, reveals that it contains 32.3 percent by mass C,...
Analysis of a non-electrolyte, unknown compound, X, reveals that it contains 32.3 percent by mass C, 3.97 percent by mass H, and the balance is O. An aqueous solution of the unknown compound is prepared by dissolving 1.142 g of X in 11.230 g water and has a freezing point of -1.26oC. What is the molecular formula of the X?