Molality is moles of solute per kilogram of solvent. The term is deprecated by NIST, which prefers the less ambiguous "mol/kg".
The molality is 0,07.
The molality is 0,2.
This molality is 90,08 g/kg.
What is the molality of a solution of 75.2 g AgClO4 dissolved in 885 g C6H6?
4 mol/0.800 kg
The molality is 0,07.
The molality is 0,2.
This molality is 90,08 g/kg.
What is the molality of a solution of 75.2 g AgClO4 dissolved in 885 g C6H6?
4 mol/0.800 kg
The molality of ethanol will be 5,91.
The molality is 5,54.
Molality of a solution remains constant as mass of a solution independent of temperature.
The higher the molality the higher the boiling point and the lower the freezing point. Conversely, the lower the molality the lower the boiling point and the lower the freezing point. Now let's analyze the problem: The total molality of 0.10 m of NaCl is 0.20 m. This is based on the property of the ionic bond. Ionic bonds are salts and thus strong electrolytes, which means they break up into all of there constituents in solution. Since two substances make up sodium chloride (sodium and chlorine), that means you'll have two substances overall. Your total molality was .10, and you have two substances, which means you're left with 0.10 * 2 = 0.20 m. Glucose is made of covalent bonds which do NOT break up in solution. This means you are left with one substance, C6H12O6. So you have 0.10 * 1 = 0.10. You are left comparing 0.20m of NaCL and 0.10m of C6H12O6. The higher molality has the higher boiling point.
4 mol over 0.800 kg
2m
It is the number of moles of solute in 1 kg of solvent.