Editing Properties Of Solutions Electrolytes And Non - Electrolytes
ApchemWiki
|
RecentChanges
|
Preferences
*<b>Introduction</b><br> 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. <br> <br><i>Basically electrolytes will conduct, non-electrolyte won't.</i><br><br> A strong electrolyte produces a large number of ions giving high conductivity values.<br> Example: H<sub>3</sub>PO<sub>4</sub>-->3 H<sup>+</sup> + PO<sub>4</sub><sup>-3</sup><br><br> A non- electrolyte does not break up into ions.<br> Example: CH<sub>3</sub>OH<sub>(l)</sub> --> CH<sub>3</sub>OH<sub>(aq)</sub><br><br> *<b>Procedures</b><br> See lab<br><br> *<b>Tips</b><br> You don't need a lot of the solution, just enough to cover the probe<br><br> *<b>Questions</b><br> # Separate the above solutions into ionic compounds, molecular compounds, and acids.<br> # Why would you expect ionic cpds to conduct and molecular cpds to not conduct? (use chemical reactions)<br> # Why do HCl and H<sub>3</sub>PO<sub>4</sub> conduct more than HC<sub>2</sub>H<sub>3</sub>O<sub>2</sub>? # Explain the difference in the conductivity values between the distilled and tap waters.
View other revisions
ApchemWiki
|
RecentChanges
|
Preferences