Introduction This lab introduces you to the properties of strong and weak electrolytes and non-electrolyte solutions. An electrolyte is a material that dissolves in water to give a solution that conducts an electric current. To carry this current, an electrolyte breaks up into its ions and the ions carry the current to complete the circuit. A strong electrolyte produces a large number of ions giving high conductivity values. Basically electrolytes will conduct, non-electrolyte won't Example: H3PO4-->3 H+ + PO4-3 |
*Introduction This lab introduces you to the properties of strong and weak electrolytes and non-electrolyte solutions. An electrolyte is a material that dissolves in water to give a solution that conducts an electric current. To carry this current, an electrolyte breaks up into its ions and the ions carry the current to complete the circuit. Basically electrolytes will conduct, non-electrolyte won't. A strong electrolyte produces a large number of ions giving high conductivity values. Example: H3PO4-->3 H+ + PO4-3 |
Example: CH3OH(l) --> CH3OH(aq) Procedures See lab Tips You don't need a lot of the solution, just enough to cover the probe |
Example: CH3OH(l) --> CH3OH(aq) *Procedures See lab *Tips You don't need a lot of the solution, just enough to cover the probe *Questions # Separate the above solutions into ionic compounds, molecular compounds, and acids. # Why would you expect ionic cpds to conduct and molecular cpds to not conduct? (use chemical reactions) # Why do HCl and H3PO4 conduct more than HC2H3O2? # Explain the difference in the conductivity values between the distilled and tap waters. |