A 12.0 g sample of a non-electrolyte is dissolved in 80.0 g of water. The solution freezes at . What is the molar mass of this solute? The freezing point depression constant of water is .
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Lysozyme is an enzyme that cleaves cell walls. A 0.100 L sample of a solution of lysozyme containing 0.0750 g of the enzyme exhibits an osmotic pressure of atm at . What is the molar mass of lysozyme?
A sample of an organic compound (a non-electrolyte) weighing 1.30 g lowered the freezing point of 10.0 g of benzene by . What is the molar mass of the compound?
When 5.00 g of a non-ionic compound is dissolved in 25.00 g of carbon tetrachloride (boiling point , , the boiling point of the solution at 1 atm is . Calculate the molar mass of the non-ionic compound.
A sample of sulfur weighing 0.201 g was dissolved in 17.8 g of carbon disulfide, . If the boiling point of the carbon disulfide was elevated by , what is the formula of a sulfur molecule in this solution?
A 2.43 mol/kg aqueous solution of glycerin was prepared by mixing glycerin with 0.500 kg of water.
What mass of glycerin was required?
What is the freezing point of this solution? The freezing point depression constant of water is 1.86 kg⋅K/mol.
When 6.29 g of a non-volatile solute is dissolved in 500 g of water, the freezing point of the resultant aqueous solution is lower than that of pure water. The cryoscopic constant for water is and the solute does not dissociate. Estimate the molar mass of the solute.