Our lab consisted of combining small amounts of aqueous solutions in order to observe their soluble nature (or lack thereof). The key concept that was involved in this lab was the concept of solubility, the ability of a substance (the solute) to dissolve in a solvent rather than to form a solid precipitate. Through this lab, we were attempting to determine the solubility of the solutions as well as observe how the solutions interact with each other -- if they form a precipitate once combined or remain aqueous. Our results reflected the rules of solubility (go more in depth about the rules). Also, there were some more directly beneficial results due to the lab. We now have more knowledge and have gained a deeper understanding of solubility and how different compounds interact. An example of a realistic application for density could be a (add). Experimental
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Solutions should be the cations of cupric nitrate, ammonium nitrate, zinc nitrate, calcium nitrate, aluminum nitrate, silver nitrate, ferric nitrate, and plumbous nitrate. The other seven solutions should be the anions of sodium hydroxide, sodium carbonate, potassium sulfate, sodium iodide, sodium phosphate, sodium chloride, and sodium chromate.
Divide students into groups of two.
Provide a bin of paper towels for the students to empty their well plates.
Students:
Obtain a pair of safety goggles from the goggle cabinet, a plastic reaction well plate for your group, two 250 mL beakers from station drawer to share with another group, 15 pipettes (each pipette labeled with the name of one aqueous solution) to share with another group, one glass stirring rod from the station drawers for you and your partner, a paper copy of the periodic table for your pair, a bottle of deionized water for the table of two groups to share, paper towels, soap, and one test tube brush from the station drawers for your own
Solutions should be the cations of cupric nitrate, ammonium nitrate, zinc nitrate, calcium nitrate, aluminum nitrate, silver nitrate, ferric nitrate, and plumbous nitrate. The other seven solutions should be the anions of sodium hydroxide, sodium carbonate, potassium sulfate, sodium iodide, sodium phosphate, sodium chloride, and sodium chromate.
Divide students into groups of two.
Provide a bin of paper towels for the students to empty their well plates.
Students:
Obtain a pair of safety goggles from the goggle cabinet, a plastic reaction well plate for your group, two 250 mL beakers from station drawer to share with another group, 15 pipettes (each pipette labeled with the name of one aqueous solution) to share with another group, one glass stirring rod from the station drawers for you and your partner, a paper copy of the periodic table for your pair, a bottle of deionized water for the table of two groups to share, paper towels, soap, and one test tube brush from the station drawers for your own