Examples of molality in the following topics:
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- A solution with a molality of 1 mol/kg is often described as "1 molal" or "1 m."
- The concentration, or molality, remains constant.
- Remember that molality is moles of solute/kg per solvent.
- The molality of our KCl and water solution is 1.3 m.
- In this lesson, you will learn how molarity and molality differ.
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- Solution concentration is expressed by a solution's molality, while electrolyte concentration is expressed in terms of milliequivalents per liter.
- On the other hand, a solution's molality is the number of moles of solute per kilogram of solvent.
- Molarity and molality represent solution concentration, but electrolyte concentrations are usually expressed in terms of milliequivalents per liter (mEq/L).
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- The two most common ways of expressing concentration are molarity and molality.
- The molal concentration (m) of a solution is defined as the number of moles of solute (n) per kilogram of solvent (i.e., the mass of the solvent, msolvent):
- Calculate concentrations of solutions in molarity, molality, mole fraction and percent by mass and volume.
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- It is directly proportional to the molal concentration of the solution.
- In this equation, $\Delta T_b$ is the boiling point elevation, $K_b$ is the boiling point elevation constant, and m is the molality of the solution.
- Calculate the boiling point of an aqueous solution where enough NaCl is added to make a 0.37 molal solution.
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- Mole fraction can also be calculated from molality.
- Since we are given molality, we can convert it to the equivalent mole fraction, which is already a mass ratio; remember that molality = moles solute/kg solvent.
- Given the definition of molality, we know that we have a solution with 1.62 moles of sugar and 1.00 kg (1000 g) of water.
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