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Why does a 0.10 molality solution of NaCl have a higher boiling point and a lower freezing point than a 0.10 molality solution of C6H12O6?
Wiki User
∙ 11y ago
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.
Wiki User
∙ 11y ago
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Explain why molality is used for boiling point elevation and feezing point depression calculations and molarity is used for osmotic pressure calculations?
Molality is independent of temperature, so when you are trying to find changes in boiling and freezing points you need something that will stay constant regardless of the change in temperature. Molarity is temperature dependent and also is based on the volume of a solution, both of which are needed to calculate pressure using the ideal gas law, PV=nRT. Osmotic pressure is similar but we substitute the number of moles of the solution and the volume by using the molarity, you cannot do this with molality, since it is dependent on mass, not volume.
Is the boiling point of a 0.5 m aqueous solution of KOH higher than the boiling point of a .5m aqueous solution of KCL?
Colligative properties, such as boiling point elevation, depend on the molality of the solution and the number of "entities" (ions, in this case) per formula unit. For the solutions specified, these are identical, so the answer is no.
What is the freezing point of an aqueous solution if the boiling point of an aqueous solution is 101.34 degree Celsius?
nobody knows
Does salt affect the temperature of water -boiling point - freezing point?
i would opt for the Freezing point. salt decreases the freezing point of water. so if water would normally freeze at 0C, saltwater would freeze at -3C.
Compare the boiling and freezing points of 1m solution of glucose to a 1m solution of Cacl2. Why does CaCl2 have a higher boiling and a lower freezing Please explain not just say its 1m and then 3m?
Boiling and freezing points are colligative properties, meaning they depend on the number of solute particles dissolve in solution. Glucose is a molecular compound so it is one particle dissolved in solution. CaCl2 will dissociate into three particles in solution. There are three times as many particles present in solution when CaCl2 dissolves.
What is the effect of the boiling point and freezing point of a solution with electrolytes is caused?
it's a colligative property of solutions... when you add a higher boiling substance to a solution the boiling point increases and when you add anything that interferes with the intramolecular forces holding the solution together the freezing point decreases.
Explain why molality is used for boiling point elevation and feezing point depression calculations and molarity is used for osmotic pressure calculations?
Molality is independent of temperature, so when you are trying to find changes in boiling and freezing points you need something that will stay constant regardless of the change in temperature. Molarity is temperature dependent and also is based on the volume of a solution, both of which are needed to calculate pressure using the ideal gas law, PV=nRT. Osmotic pressure is similar but we substitute the number of moles of the solution and the volume by using the molarity, you cannot do this with molality, since it is dependent on mass, not volume.
What lowers the freezing point and raises the boiling point?
Yes, it is possible if the solution contain solutes.
What is the boiling point of a solution of 125.0 g of c6h12o6 in 350 g c2h5oh kb for c2h5oh is 1.19ºcm and the boiling point of c2h5oh is 78ºc?
88c
Is the boiling point of a 0.5 m aqueous solution of KOH higher than the boiling point of a .5m aqueous solution of KCL?
Colligative properties, such as boiling point elevation, depend on the molality of the solution and the number of "entities" (ions, in this case) per formula unit. For the solutions specified, these are identical, so the answer is no.
What is freezing point elevation?
This is not a common phenomenon. Usually it is boiling points that are elevated, and freezing points are depressed. It is possible that a freezing point could be raised (elevated) due to the presence of an impurity with a much higher freezing point.Changes in boiling and freezing points are typically due to impurities in compound.See the Related Questions to the left for more information about freezing point depression and boiling point elevation problems.
What occurs when NaCl is added to water?
The boiling point of the solution increases, and the freezing point of the solution decreases.
What does ethylene glycol do to the solution?
Raises the boiling point and lowers the freezing point.
At what temperature does brine freeze?
actually its freezing point depends on the molality of the brine. it is mathematically given as:- Δt=km, where Δt=change in freezing point k= cryoscopic constant m= molality of the substance the value of k for water(as a solvent)is= 1.86 Kg/mole therefore, t=273.15-(1.86*m) where t is the freezing point of brine note:- adding any solute always lower the boiling point of the solution. thnx for asking.
What is the boiling point of a solution of 125.0 g of c6h12o6 in 350 g c2h5oh kb for c2h5oh is 1.19ºc m and the boiling point of c2h5oh is 78ºc?
80c
What is the boiling point of a solution of 1250 g of c6h12o6 in 350 g c2h5oh kb for c2h5oh is 119cm and the boiling point of c2h5oh is 78c?
35 c
What is the freezing point of an aqueous solution if the boiling point of an aqueous solution is 101.34 degree Celsius?
nobody knows
