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Water is the solvent i don't the other one
chicken murderer
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What is a solvent?
A solvent is a liquid that dissolves a solute. The solvent is the component of a solution that is present in greater amount. Perhaps the most common solvent in everyday life is water. Many other solvents are organic compounds, such as benzene, tetrachloroethylene, or turpentine.
A solute makes the freezing point of a solution lower than the freezing point of the pure solvent because?
The phenomenon you're describing is generally referred to as freezing-point depression, the lowering of the freeze point of a liquid (or solvent) by adding another compound. Freezing point depression is a phenomenon driven by entropic changes in the system containing solvent and solute. As the system is frozen, the solvent forms crystals of high purity regardless of solute molecules being present while solvent crystallizes. Replacement of any solute in the crystal with a solvent molecule takes place spontaneously, since the inability of solute molecules to fit well into the ordered crystal makes the solute-solvent substitution thermodynamically favorable. As the freezing proceeds, solvent molecules continue to leave the liquid state and incorporate into the solid crystal, with each such occurrence leaving behind a smaller volume of liquid in which solute molecules can occupy. The shrinking of liquid volume occupied by a fixed number of solute molecules reduces the dispersion of solute molecules in the liquid, resulting in a reduction of entropy of the solute molecules. Thus, additional energy is required to match the reduced entropy of the solute molecules with that of the solid solvent crystal. The energy required (versus pure solvent) to gap the entropic difference (thus difference in chemical potential) to establish equilibrium but at a freezing temperature lower than that of the pure substance. Note that at low solute concentrations, freezing point depression is a property that depends solely of the number of solute particles and physical properties of the solute. Such properties are called colligative properties.
The solute molecules mixed with the solvent molecules in a solution cause the of a solution to be higher than it is for an equal volume of pure solvent?
Raoult's Law and Vapor Pressure LoweringWhen a nonvolatile solute is added to a liquid to form a solution, the vapor pressure above that solution decreases. To understand why that might occur, let's analyze the vaporization process of the pure solvent then do the same for a solution. Liquid molecules at the surface of a liquid can escape to the gas phase when they have a sufficient amount of energy to break free of the liquid's intermolecular forces. That vaporization process is reversible. Gaseous molecules coming into contact with the surface of a liquid can be trapped by intermolecular forces in the liquid. Eventually the rate of escape will equal the rate of capture to establish a constant, equilibrium vapor pressure above the pure liquid.If we add a nonvolatile solute to that liquid, the amount of surface area available for the escaping solvent molecules is reduced because some of that area is occupied by solute particles. Therefore, the solvent molecules will have a lower probability to escape the solution than the pure solvent. That fact is reflected in the lower vapor pressure for a solution relative to the pure solvent. That statement is only true if the solvent is nonvolatile. If the solute has its own vapor pressure, then the vapor pressure of the solution may be greater than the vapor pressure of the solvent.Note that we did not need to identify the nature of the solvent or the solute (except for its lack of volatility) to derive that the vapor pressure should be lower for a solution relative to the pure solvent. That is what makes vapor pressure lowering a colligative property--it only depends on the number of dissolved solute particles.summarizes our discussion so far. On the surface of the pure solvent (shown on the left) there are more solvent molecules at the surface than in the right-hand solution flask. Therefore, it is more likely that solvent molecules escape into the gas phase on the left than on the right. Therefore, the solution should have a lower vapor pressure than the pure solvent.Figure %: The Vapor Pressure of a Solution is Lower than that of the Pure Solvent
What will adding solute to pure solvents cause?
Adding a solute to a pure solvent will lower the freezing point, elevate the boiling point, and lower the vapor pressure.
What happens to a nonvolatile solute when added to water and the water raises?
Boiling-point elevation describes the phenomenon that the boiling point of a liquid (a solvent) will be higher when another compound is added, meaning that a solution has a higher boiling point than a pure solvent. This happens whenever a non-volatile solute, such as a salt, is added to a pure solvent, such as water. The boiling point can be measured accurately using an ebullioscope.
What is the solvent and solute in liquid nitrogen?
There is neither a solvent nor solute in liquid nitrogen as it is not a solution. Liquid nitrogen is pure elementalnitrogen in liquid form.
What is the differentiate of solution and a pure liquid?
A solution is a mixture of solvent which is larger in quantity and of one or more solute which is smaller in quantity like e.g. sugar or salt in water, where sugar or salt are solute and water is solvent and when they mix it form solution. A pure liquid is one which do not contain any other particle except itself like e.g. water without impurities or solute particles (known as distill water) is pure liquid
What is a solvent?
A solvent is a liquid that dissolves a solute. The solvent is the component of a solution that is present in greater amount. Perhaps the most common solvent in everyday life is water. Many other solvents are organic compounds, such as benzene, tetrachloroethylene, or turpentine.
Is oxygen a solvent or solution?
Oxygen is a solvent and if you want to know what a helium is then it is a solute.
A solute makes the freezing point of a solution lower than the freezing point of the pure solvent because?
The phenomenon you're describing is generally referred to as freezing-point depression, the lowering of the freeze point of a liquid (or solvent) by adding another compound. Freezing point depression is a phenomenon driven by entropic changes in the system containing solvent and solute. As the system is frozen, the solvent forms crystals of high purity regardless of solute molecules being present while solvent crystallizes. Replacement of any solute in the crystal with a solvent molecule takes place spontaneously, since the inability of solute molecules to fit well into the ordered crystal makes the solute-solvent substitution thermodynamically favorable. As the freezing proceeds, solvent molecules continue to leave the liquid state and incorporate into the solid crystal, with each such occurrence leaving behind a smaller volume of liquid in which solute molecules can occupy. The shrinking of liquid volume occupied by a fixed number of solute molecules reduces the dispersion of solute molecules in the liquid, resulting in a reduction of entropy of the solute molecules. Thus, additional energy is required to match the reduced entropy of the solute molecules with that of the solid solvent crystal. The energy required (versus pure solvent) to gap the entropic difference (thus difference in chemical potential) to establish equilibrium but at a freezing temperature lower than that of the pure substance. Note that at low solute concentrations, freezing point depression is a property that depends solely of the number of solute particles and physical properties of the solute. Such properties are called colligative properties.
The solute molecules mixed with the solvent molecules in a solution cause the of a solution to be higher than it is for an equal volume of pure solvent?
Raoult's Law and Vapor Pressure LoweringWhen a nonvolatile solute is added to a liquid to form a solution, the vapor pressure above that solution decreases. To understand why that might occur, let's analyze the vaporization process of the pure solvent then do the same for a solution. Liquid molecules at the surface of a liquid can escape to the gas phase when they have a sufficient amount of energy to break free of the liquid's intermolecular forces. That vaporization process is reversible. Gaseous molecules coming into contact with the surface of a liquid can be trapped by intermolecular forces in the liquid. Eventually the rate of escape will equal the rate of capture to establish a constant, equilibrium vapor pressure above the pure liquid.If we add a nonvolatile solute to that liquid, the amount of surface area available for the escaping solvent molecules is reduced because some of that area is occupied by solute particles. Therefore, the solvent molecules will have a lower probability to escape the solution than the pure solvent. That fact is reflected in the lower vapor pressure for a solution relative to the pure solvent. That statement is only true if the solvent is nonvolatile. If the solute has its own vapor pressure, then the vapor pressure of the solution may be greater than the vapor pressure of the solvent.Note that we did not need to identify the nature of the solvent or the solute (except for its lack of volatility) to derive that the vapor pressure should be lower for a solution relative to the pure solvent. That is what makes vapor pressure lowering a colligative property--it only depends on the number of dissolved solute particles.summarizes our discussion so far. On the surface of the pure solvent (shown on the left) there are more solvent molecules at the surface than in the right-hand solution flask. Therefore, it is more likely that solvent molecules escape into the gas phase on the left than on the right. Therefore, the solution should have a lower vapor pressure than the pure solvent.Figure %: The Vapor Pressure of a Solution is Lower than that of the Pure Solvent
Why is it when a solute is added to a pure liquid the boiling point increases and the freezing point decreases?
Boiling point is the temperature at which the vapor pressure of the liquid equals atmospheric pressure. The vapor pressure of solvent molecules is decreased when a solute is added, so a higher temperature is required to increase the number of solvent molecules in the gas phase above the liquid. At the freezing point, the vapor pressures of the solid and liquid are equal; a lower temperature is needed to reduce the number of solvent particles above the liquid.
How do you obtain a pure solvent from a solution by distillation?
By separating the mixture of solute and solvent based on their boiling points.
What is the molarity of pure liquid benzene?
Molarity is a concentration unit of solutions, pure benzene is not a solution so this term is meaningless for a pure liquid. In other words: Molarity of a solution is a numerical way of saying exactly how much solute is dissolved in a solvent .Molarity is equal to the moles of solute divided by the liters of solution. Molarity of a solution can be calculated by using the following formula: M= moles of solute/liters of solution
Is copper solute or solvent?
No. Copper is an element.
What will adding solute to pure solvents cause?
Adding a solute to a pure solvent will lower the freezing point, elevate the boiling point, and lower the vapor pressure.
What happens to a nonvolatile solute when added to water and the water raises?
Boiling-point elevation describes the phenomenon that the boiling point of a liquid (a solvent) will be higher when another compound is added, meaning that a solution has a higher boiling point than a pure solvent. This happens whenever a non-volatile solute, such as a salt, is added to a pure solvent, such as water. The boiling point can be measured accurately using an ebullioscope.
