ideal solution

(noun)

A solution with thermodynamic properties analogous to those of a mixture of ideal gases.

Related Terms

Examples of ideal solution in the following topics:

  • Vapor Pressure of Nonelectrolyte Solutions

    • The vapor pressure of a solution is directly influenced by the number of solute molecules present in a given amount of solvent.
    • The vapor pressure of a solvent is lowered by the addition of a non-volatile solute to form a solution.
    • In a solution, some spots on the surface are occupied by solute molecules, so there is less space occupied by solvent molecules.
    • Raoult's law states that the vapor pressure of an ideal solution is dependent on the vapor pressure of the pure solvent and the mole fraction of the component present in the solution.
    • For an ideal solution, equilibrium vapor pressure is given by Raoult's law:

  • Osmotic Pressure

    • A solution is defined as a homogeneous mixture of both a solute and solvent.
    • Solutions generally have different properties than the solvent and solute molecules that compose them.
    • Some special properties of solutions are dependent solely on the amount of dissolved solute molecules, regardless of what that solute is; these properties are known as colligative properties.
    • The osmotic pressure (II) of an ideal solution can be approximated by the Morse equation:
    • Discuss the effects of a solute on the osmotic pressure of a solution

  • Solutions and Entropy Changes

    • In a similar manner entropy plays an important role in solution formation.
    • All these factors increase the entropy of the solute.
    • This is the same as saying that the entropy of the solute increases.
    • Since the Hsolution for this process is approximately zero (an ideal solution), the only thermodynamic factor driving the mixing is the entropy term.
    • When food dye is added to water, a solution is formed.

  • Mole Fraction and Mole Percent

    • In a mixture of ideal gases, the mole fraction can be expressed as the ratio of partial pressure to total pressure of the mixture.
    • Mole fraction can also be applied in the case of solutions.
    • $x = (\frac {1.62 \text{ moles sugar}}{57.1 \text{ moles solution}})= 0.0284 $
    • With the mole fraction of 0.0284, we see that we have a 2.84% solution of sugar in water.
    • $x = (\frac {.388 \text{ moles cinnamic acid}}{1.22 \text{ moles solution}})= 0.318$

  • Density Calculations

    • A reformulation of the Ideal Gas Equation involving density allows us to evaluate the behaviors of ideal gases of unknown quantity.
    • The Ideal Gas Equation in the form $PV=nRT$ is an excellent tool for understanding the relationship between the pressure, volume, amount, and temperature of an ideal gas in a defined environment that can be controlled for constant volume.
    • We know the Ideal Gas Equation in the form $PV=nRT$.
    • The term $\frac{m}{V}$ appears on the right-hand side of the above rearranged Ideal Gas Law.
    • Atmospheric science offers one plausible real-life application of the density form of the ideal gas equation.

  • Using Molarity in Calculations of Solutions

    • In chemistry, molar concentration, or molarity, is defined as moles of solute per total liters of solution.
    • What is the molarity of a solution containing 0.32 moles of NaCl in 3.4 liters of solution?
    • Molarity is a measurement of concentration, with units of mol solute per liter solution.
    • Also, molarity is a ratio that describes the moles of solute per liter of solution.
    • Translate between molarity, grams of solute in solution, and volume of solution.

  • Standard States and Standard Enthalpy Changes

    • In chemistry, the standard state of a material, be it a pure substance, mixture, or solution, is a reference point used to calculate its properties under different conditions.
    • Strictly speaking, temperature is not part of the definition of a standard state; the standard state of a gas is conventionally chosen to be 1 bar for an ideal gas, regardless of the temperature.
    • The standard state should not be confused with standard temperature and pressure (STP) for gases, or with the standard solutions used in analytical chemistry.

  • The Effect of the Finite Volume

    • Real gases deviate from the ideal gas law due to the finite volume occupied by individual gas particles.
    • The ideal gas law is commonly used to model the behavior of gas-phase reactions.
    • It is important to note that this equation applies to ideal gases as well.
    • Ideal gases are assumed to be composed of point masses that interact via elastic collisions.
    • Demonstrate an understanding of the van der Waals equation for non-ideal gases.

  • Vapor Pressure of Electrolyte Solutions

    • The vapor pressure of an electrolytic solution is dependent on the ratio of solute to solvent molecules in a solution.
    • Nonelectrolyte solutions are those in which the solute does not dissociate into ions when dissolved; sugar does not dissociate, for example.
    • To better visualize the effect of solute on the vapor pressure of a solution, consider a pure solvent.
    • Now consider a solution composed of both solvent and solute.
    • In an electrolyte solution, the number of dissolved particles is larger because the solute breaks apart into ions.

  • Medical Solutions: Colligative Properties

    • These electrolytic solutions share the same colligative properties as chemical solutions.
    • One class of medical solutions is known as saline solutions.
    • These solutions are composed of water and sodium chloride.
    • Saline solutions can vary in their concentrations.
    • The saline solution is expected to restore the salinity levels in the blood.