- To start this activity, click this link for Names and Formulas of Ionic Compounds. The lab will load in a new tab. Click back to this tab to read further instructions and complete the questions below.
- Drag a test tube from the box and place it in the clamp on the ring stand (or you can double click a tube to move it). You can then click on the bottle of Ag+ ion solution on the shelf to add it to the test tube.
- Click on the Divide button (the test tube next to the hotplate on the front of the lab bench) four times to make four additional test tubes containing Ag+. With one test tube in the clamp and four others in the blue rack, click on the Na2S bottle located on the lab bench. You will be able to observe what happens in the Live Data display. Record your observation in the table below and write a correct chemical formula and name for the product of the reaction. If the solution remains clear, record NR, for no reaction. Drag this test tube to the red disposal bucket on the right. (*See instructions below step 5 for additional explanation of what to record in the table.)
- Place a second tube from the blue rack (containing Ag+) in the clamp on the ring stand. Add NaCl. Record your observations and discard the tube. Use the next tube but add Na2SO4, and record your observations. Use the next tube but add NaOH, and record your observations. With the last tube add Na2CO3 and record your observations. When you are completely finished, click on the red disposal bucket to clear the lab.
- Repeat steps 2-4 for Pb2+, Ca2+, Fe3+, and Cu2+. Complete the table.
Each cell should include a description of what you observed when the reagents were mixed and a correct chemical formula (eg: NaCl, not Na+Cl–) and name for all solutions that turned cloudy and NR for all solutions that did not react or remained clear. If there is no visible reaction, put NR in the boxes for Observations, Name and Formula. Remember to include roman numerals where appropriate.
You will find that a few of these formulas may not be what you’d expect from the solubility tables in your textbook. Some of the variations are due to the fact that these are low concentration prepared solutions that include water. Acidity, temperature and speed of reaction all affect the results you see. These are all actual images taken under identical conditions in our labs.
You can enter subscripts and superscripts in the chemical formulas using the _ and ^ symbols respectively. For example: A_2B^3 will give you A2B3. The Preview button will help you make sure your formula looks right.
Question
- Did you notice any patterns? Explain the patterns you noticed.
