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Why does ethylene glycol increase the boiling point of water?
Ethylene glycol is a non-volatile solute that raises the boiling point of water through the phenomenon of boiling point elevation. When ethylene glycol is dissolved in water, it disrupts the hydrogen bonding between water molecules, making it harder for them to escape into the gas phase. This results in an increase in the boiling point of the solution compared to pure water.
How can the energy of the molecules of a solute and solvent be increased?
The energy of molecules in a solute and solvent can be increased by adding outside energy, say, heat, for instance.
Why moles solute before dilution equals moles solute after dilution?
This assumes you are using water (or whatever the original solvent is) to do the dilution so you are not adding more solute, only more solvent,
What effect does adding a solute to a solvent have on the freezing point of the solvent?
the temperature at which the solution freezes is lowered.
Can concentration of a solution be increased by constantly adding more material to the liquid?
Yes, adding more solute to a liquid will increase the concentration of the solution. By continually adding solute without adding more solvent, you are increasing the amount of solute particles in the same volume of solvent, thus increasing the concentration.
What is the solute and solvent of antifreeze?
water is solvent and ethylene glycol is solute
What is the solute of antifreeze?
The solute of antifreeze is ethylene glycol, the solvent is water. -Answered by Santa Claus HO HO HO
What is the solvent and solute in antifreeze?
Ethylene gkycol can be a solute; water is the solvent.
What are true the vapor pressure of 1 m ethylene glycol C2H6O2 is the same as the vapor pressure of 1 m kCI where the solvent is water is it true or false?
False. The vapor pressure of a solution is lower than that of the pure solvent in a colligative property called Raoult's law. The vapor pressure of a solution is directly proportional to the mole fraction of the solute present, so the presence of the solute (ethylene glycol or KCl) will lower the vapor pressure compared to pure water.
How is massed conserved when adding a solute to a solvent?
If you weigh the solute, and then weigh the solvent, and then add the solute to the solvent and weigh the solution, you will find that the sum of the weights of the solute and solvent is equal to the weight of the resulting solution. So mass is conserved.
Why does ethylene glycol increase the boiling point of water?
Ethylene glycol is a non-volatile solute that raises the boiling point of water through the phenomenon of boiling point elevation. When ethylene glycol is dissolved in water, it disrupts the hydrogen bonding between water molecules, making it harder for them to escape into the gas phase. This results in an increase in the boiling point of the solution compared to pure water.
What will adding solute to pure solvents cause?
Adding solute to pure solvents will cause the solute to dissolve in the solvent, forming a solution. This process can alter the properties of the solvent, such as its boiling point, freezing point, and osmotic pressure, depending on the amount and nature of the solute added.
How can the energy of the molecules of a solute and solvent be increased?
The energy of molecules in a solute and solvent can be increased by adding outside energy, say, heat, for instance.
What is the maximum amount of solute that can be dissolved in a solute at a particular temperature?
This is known as the solubility of the solute in the solvent. When you reach the maximum it is know as the saturation concentration. Adding any more solute will not dissolve in the solvent.
What is the process of mixing the solute with the solvent?
Dissolving
What are two ways you can change the concetration of a solution?
Adding more solute or adding more solvent
How does adding a solute affect the vapor pressure?
Adding a solute to a solvent lowers the vapor pressure of the solution compared to the pure solvent. This is due to the solute molecules occupying some of the surface area that would have been available for solvent molecules to evaporate. As a result, fewer solvent molecules are able to escape into the gas phase, leading to a decrease in vapor pressure.
