Chapter 4.5 Concentrations of Solutions

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Chemistry

Concentrations

Molarity

Molality

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8 Terms

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ppb

mass of solute (μg) / total mass of solution (Kg)

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A) 43,01% B)XH2SO4= 0,122 C) 7,69 m D) 5,827 M

Bonus Example: A dissolution of sulfuric acid that contains 571,6 g of H2SO4 per liter of dissolution, has a density of 1,329 g/cm3. Calculate A) m/m% B) Molar Fraction C) Molality D) Molality

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ppm

mass of solute (mg) / total mass of solution (Kg)

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M

moles of solute / volume of solution in liters

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m

moles of solute / kg of solvent

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XX

moles of solute / total moles of solution

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m/m %

mass of solute / total mass of solution *100

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v/v%

volume of solute / total volume of solution *100