solute

Examples of solute in the following topics:

• 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.

• 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.
  • If a solution consisting of both solute and solvent molecules is placed on one side of a membrane and pure solvent is placed on the other side, there is a net flow of solvent into the solution side of the membrane.
  • Discuss the effects of a solute on the osmotic pressure of a solution

• 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.

• Intermolecular Forces and Solutions

  • To form a solution, molecules of solute and solvent must be more attracted to each other than themselves.
  • In order to form a solution, the solute must be surrounded, or solvated, by the solvent.
  • Solutes successfully dissolve into solvents when solute-solvent bonds are stronger than either solute-solute bonds or solvent-solvent bonds.
  • If the solute binds to other solute (X-X bond) more strongly than the solute binds to the solvent (X-Y bond), then the dissolution is not energetically favorable.
  • Recall the two conceptual steps necessary to dissolve a solute and form a solution

• Electrolyte and Nonelectrolyte Solutions

  • An electrolyte is any salt or ionizable molecule that, when dissolved in solution, will give that solution the ability to conduct electricity.
  • The resulting solution will conduct electricity because it contains ions.
  • As mentioned above, when an ionizable solute dissociates, the resulting solution can conduct electricity.
  • A strong electrolyte will completely dissociate into its component ions in solution; a weak electrolyte, on the other hand, will remain mostly undissociated in solution.
  • Nonelectrolytes are compounds that do not ionize at all in solution.

• Heat of Solution

  • Heat of solution refers to the change in enthalpy when a solute is dissolved into a solvent.
  • The heat of solution, also referred to the enthalpy of solution or enthalpy of dissolution, is the enthalpy change associated with the dissolution of a solute in a solvent at constant pressure, resulting in infinite dilution.
  • The heat of solution can be regarded as the sum of the enthalpy changes of three intermediate steps:
  • The value of the overall heat of solution, $\Delta H^\circ_{sol}$, is the sum of these individual steps.
  • This depends entirely on if more energy was used to break the solute-solute and solvent-solvent bonds, or if more energy was released when solute-solvent bonds were formed.

• Dilutions of Solutions

  • This process keeps the amount of solute constant, but increases the total amount of solution, thereby decreasing its final concentration.
  • Dilution can also be achieved by mixing a solution of higher concentration with an identical solution of lesser concentration.
  • Diluting solutions is a necessary process in the laboratory, as stock solutions are often purchased and stored in very concentrated forms.
  • M1 denotes the concentration of the original solution, and V1 denotes the volume of the original solution; M2 represents the concentration of the diluted solution, and V2 represents the final volume of the diluted solution.
  • What is the final concentration of the diluted solution?

• Molality

  • Molality is a property of a solution that indicates the moles of solute per kilogram of solvent.
  • Molality is an intensive property of solutions, and it is calculated as the moles of a solute divided by the kilograms of the solvent.
  • It is easy to calculate molality if we know the mass of solute and solvent in a solution.
  • With this information, we can divide the moles of solute by the kg of solvent to find the molality of the solution:
  • Since the solution is very dilute, the molality is almost identical to the molarity of the solution, which is 1.3 M.

• Molarity

  • Molarity is defined as the moles of a solute per volume of total solution.
  • In chemistry, concentration of a solution is often measured in molarity (M), which is the number of moles of solute per liter of solution.
  • A solution that contains 1 mole of solute per 1 liter of solution (1 mol/L) is called "one Molar" or 1 M.
  • To calculate the molarity of a solution, the number of moles of solute must be divided by the total liters of solution produced.
  • If there are 10.0 grams of NaCl (the solute) dissolved in water (the solvent) to produce 2.0 L of solution, what is the molarity of this solution?