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An aqueous solution of isopropanol (mm = 60.10 g/mol) has a molality of 12.79 m and a density of 1.180 g/ml. what is the molarity of isopropanol in the solution?

Respuesta :

The molarity of an aqueous solution of isopropanol = 15.09 mol/L

Molality = 12.79 m

This gives that 12.79 moles of isopropanol is dissolved in 1000 grams of water.

Density = 1.180 g/mL

We know that,

Density= mass/volume

volume = mass/density

            = 1000/1.180

Volume = 847.46 ml

Molarity can be defined as the mass of solute per liter of the solution.

Molarity = moles × 1000/volume ------> (1)

The moles of isopropanol in 847.46 ml solution is 12.79.

On substituting in (1)

Molarity = 12.79 × 1000/847.46

Molarity= 15.09 mol/L

The molarity of aqueous solution of isopropanol is 15.09 mol/L

What is molality?

The number of moles of solute in a solution equal to 1 kg or 1000 g of solvent is referred to as its molality.

What is molarity?

  • The amount of a substance in a specific volume of solution is known as its molarity (M).
  • The number of moles of a solute per liter of a solution is known as molarity.
  • The molar concentration of a solution is another name for molarity.

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