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19 Nov 2019

A solution contains 11.35 g of unknown compound (non-electrolyte) dissolved in 50.0 mL of water. (Assume a density of 1.00 g/mL for water.) The freezing point of the solution is -3.57 ∘C. The mass percent composition of the compound is 60.98% C, 11.94% H, and the rest is O. What is the molecular formula of the compound?

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Nelly Stracke
Nelly StrackeLv2
19 Nov 2019

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Related questions

A solution contains 11.85g ofunknown compound dissolved in 50.0 mL of water.


(Assume a density of 1.00 g/mL forwater.)


The freezing point of the solution is -4.89?C.


The mass percent composition of the compound is53.31% C, 11.19% H, and the rest isO.


Q: What is the molecular formula ofthe compound?

A solution contains 11.00 g of unknown compound dissolved in 50.0mL of water. (Assume a density of 1.00 g/mL for water.) Thefreezing point of the solution is -6.59 *C. The mass percentcomposition of the compound is 38.70% C , 9.74% H , and the rest isO.

What is the molecular formula of the compound?
Express your answer as a molecular formula.

1- An aqueous solution containing 36.5 g of an unknown molecular (non-electrolyte) compound in 154.3 g of water was found to have a freezing point of -1.4 ∘C.

Calculate the molar mass of the unknown compound.

2-An aqueous KNO3 solution is made using 79.9 g of KNO3diluted to a total solution volume of 1.90 L .

Calculate the molality of the solution. (Assume a density of 1.05 g/mL for the solution.)

Calculate the mass percent of the solution. (Assume a density of 1.05 g/mL for the solution.)

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