In the first week of class we learned that a homogeneous mixture of two or more substances is called a solution. If one of the substances is present in much greater quantities than all the other substances then it is called the solvent. The other substances in solution are known as solutes. For example, when a small amount of NH4Cl is dissolved in a large quantity of water we refer to water as the solvent and NH4Cl as the solute. Another example is Napthalene (used in mothballs) can be dissolved in benzene. In this example benzene is the solvent and napthalene is the solute.
Solutes dissolved in water (solvent) are called aqueous solutions. Not all substances are soluble in water. Why do some substances dissolve in water and others don't? It has to do with the structure of the water molecule.
Oxygen has a greater attraction for electrons, so the shared electrons (bonding electrons) spend more time close to oxygen then to either of the hydrogens. This gives oxygen a slightly excess negative charge and hydrogen a slightly more positive charge.
This unequal charge distribution makes water a polar molecule, and gives water its ability to dissolve compounds. When an ionic solid dissolves in water, the positive ends of the water molecule are attracted to the negatively charged anions and the negative ends of the water molecule are attracted to the positively charged cations. For example, when NaCl is dissolved in water we find
So when an ionic substance (salt) dissolves in water, it is broken up into individual cations and anions which are surrounded by water molecules. For example, when NH4 NO3 is dissolved in water it breaks up into separate ions.
NH4+ and NO3- ions are floating around in H2O essentially independent of each other.
Water also dissolves non-ionic substances. For example, C2H5OH (ethanol) is very soluble in H2O. This is because C2H5OH has a polar OH bond that the water molecules like to hang around.
Many substances do not dissolve in water and that is because they are non-polar and do not interact well with water molecules. A common example is oil and water. Oil contains molecules that are non-polar, thus they do not dissolve in water.
How do we know that ionic solids dissolve in water and form cations and anions that float around separately? One clue comes from conductivity experiments. Anions and Cations should act as charge carriers in solution. Therefore a solution with dissolved ions should conduct electricity. Let's look at a few examples. Pure (distilled) water contains no dissolved ions. Therefore pure water will not conduct electricity. In a simple conductivity experiment as shown below we would not expect the light to be on.
An aqueous NaCl solution, however, will have dissolved ions present and therefore will conduct electricity. Therefore the light in our conductivity experiment will be on if dipped in an aqueous NaCl solution.
NaCl ionizes completely when dissolved in water. It's helpful to think of this process as two steps:
Substances that exist in solution almost completely as ions are called strong electrolytes.
Substances that do not form ions when they dissolve in water are called non-electrolytes. And example of a non-electrolyte is sugar. Sugar will readily dissolve in water but doesn't form cations and anions in solution. That is, there are no charge carriers formed.
Substances that only partially ionize into ions when dissolved in water are called weak electrolytes. For example, Acetic Acid (HC2H3O2) dissolves in water, but only partially dissociates into ions.
Be careful not to confuse how soluble a substance is in water with whether it is a weak, strong, or non-electrolyte. For example, sugar dissolves completely in water but it is a non-electrolyte. Another example are salts that can be very insoluble in water but the small amount of salt that does dissolve in water is a strong electrolyte.
Chemisty, The Central Science, 10th Ed.
4.1, 4.3, 4.5, 4.7, 4.9, 4.11, 4.13, 4.15, 4.17, 4.33, 4.35, 4.37,