Chemical Reaction Lab

At the beginning of yesterday's class we turned in our separating mixtures lab. Then we proceeded to our lab desks to complete our chemical reaction lab. We had started Part A yesterday, but I'll give a brief summary of part A just to review. We used a Bearal-pipet to fill 6 rows of the well plate with HCl. We were to record both temperature of the HCl and the initial appearance in our data table. This was helpful because after the experiment was over, we could look compare the before and after data.

PART A:

• The first well we tested was A1. Groups were to put a piece of blue litmus paper in the HCl and record their initial observations, including appearance and temperature change. Next, we added 1 mL of sodium hydroxide solution and noted any temperature change. We waited a minute and tested the solution again with a piece of litmus paper. This was to test the pH of HCl, and to see if the pH would change because of the sodium hydroxide solution.
• Next, well A2. Groups added solid sodium bicarbonate to the HCl, and were to observe all changes including temperature. Once the reaction had settled down, groups were to add 2 more portions of sodium bicarbonate.
• For well A3 groups were to use a Beral-type pipet to add 1 mL of silver nitrate solution. Again, we used the date table to record observations.
• For well A4, groups added a small piece of mossy zinc to the HCl and recorded observations.
• For well A5, groups were to use the forceps to add one piece of aluminum to well A5, and accord observations in the data table.
• Lastly, well A6. In A6 we added one piece of magnesium ribbon, and recorded our observations.
• After part A was completed, groups were to remove unreacted metals from well A4-A6 and rinse the metals with water and throw away.
• Picture shows the general setup for the wells.

This is the data that I collected for the temperature/appearance changes in Part A.

(sorry if you cant read it)

PART B:

• Part B was pretty similar to part A, except with cupric chloride instead of HCl.
• To start off, we added 1 mL of cupric chloride to well B1-B6.
• Next we placed various items into each well and recorded all observations.
• For well B1-one piece of aluminum shot was added, B2-aluminum foil, B3-zinc, B4-1 mL ammonium hydroxide solution, B5-1 mL sodium carbonate solution, B6- 1 mL silver nitrate solution.
• After that, we used forcepes to remove any pieces of unreacted metals from well A4-A6, rinse the metals with water, and dispose.
• Picture on right shows how some of the metals corroded because of the cupric chloride

Here is my data table for Part B. Sorry again if you can't read it.

PART C:

• In Part C we used a graduated cylinder to add 10 mL of cupric chloride into a flask.
• Next, we rinsed the graduated cylinder and added 3 mL of silver nitrate solution to a small test tube.
• After that, we placed the test tube in the flask, capped the flask with a rubber stopper, and recorded the mass.
• We inverted the flask several times so the contents of the flask and test tube would mix. We measured the mass again and recorded it.
• The two masses should be the same.

Here are some things you might want to take a look at:

• Chemical reaction lab, incase you forgot it/lost it
• Chemical reaction data: 
• Mr Lieberman's notes:

Tonight's homework:

1. Study for tomorrows quiz (previous webassigns, chemthink, worksheets, notes, labs etc.)
2. Complete the lab

The next scribe is Stephanie K.

-Rachel M