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Salt Crystals Experiment

We did this experiment to be able to find out and observe what happens when you mix acids and alkalis together. This experiments were design to see the crystals formed, (since mixing acids and bases create salt) and then to be able to calculate the percentage yield.

Question:

What are the results when acids and bases react together?

Hypothesis:

I believe that the percentage yield will be lower than 100% because I think that there will be some human mistakes, and as we are going to heat our solution, I also believe that the solution makes water, that will then be evaporating. As well as that, in class we have learned that when you mix a alkali and an acid they form cubic crystals (salt).

List of Materials

Experiment 1:

-Hydrochloric Acid
-Sodium Hydroxide Solution
-Universal Indicator
-Charcoal Powder
-Two Flasks
-Pipette
-Beaker
-Filter
-Funnel Paper
-Bunsen Burner

Experiment 2:

-Hydrochloric Acid
-Copper Carbonate
-Beaker
-Spatula
-Glass Rod
-Filter
-Funnel Paper
-Bunsen Burner

Method

Experiment 1:

1. Put 10ml of hydrochloric acid into a beaker.
2. Add 5 drops of universal indicator.
3. Add 9ml of sodium hydroxide.
4. Use a dropper to add sodium hydroxide one drop at a time, swirling the flask after each drop.
5. Stop when the solution turns green.
6. Add a spatula of charcoal powder to the flask and swirl it.
7. Filter the solution.
8. Heat the new solution onto a Bunsen burner until it is almost empty.
9. Leave the solution for a few days so that it will form crystals.

Experiment 2:

1. Put 25ml of hydrochloric acid into a small beaker.
2. Add a spatula of copper carbonate and stir.
3. Add more copper carbonate one spatula at a time until it stops fizzing.
4. Filter the unreacted copper carbonate.
5. Heat the new solution onto a Bunsen burner until it is almost empty.
6. Leave the solution for a few days so that it will form crystals.

Table of Results

Experiment # Weight of solution Weight of crystals Percentage Yield
Experiment 1 21.44g 0.78g 133.4 percent
Experiment 2 96.99g 1.27g 75.5 percent

The crystals formed in the first experiment had a cubic structure.
The weight of the empty flask was 117.14g

Experiment 1:

Weight of flask with sodium solution: 138.58g
Weight of hydrochloric acid and sodium hydroxide: 21.44g

Theoretical mass
NaOH + HCL > NaCl + H2O
1M 1M
10ml 10ml

n=CxV n= 1 x 10/1000 n= 0.01

moles NaCl= 0.01 mass NaCl= 0.01 x Mr mass NaCl= 0.01 x 58.5 mass NaCl= 0.585g

Experimental mass (mass of crystals): 0.78g

Percentage yield
0.78/0.585 x 100= 133.4 percent

Experiment 2:

Theoretical Mass
2HCl + CuCO3 > CO2 + CuCl2 + H2O moles= 0.025 x 1 moles= 0.025

2/0.025 = 1/x x = 0.025 x 1 / 2

mass= 0.025/2 x 134.5 mass= 1.68g

Experimental mass: 1.27

Percentage yield
1.27/1.68 x 100 = 75.5 percent

Conclusion

Experiment 1:

Overall our experiment went as planned, after heating up the hydrochloric acid and the sodium hydroxide mixture (which is now neutralized), we ended up with cubic crystals (salt).

As we can see in the results in the first experiment the percentage yield we have found is higher than 100%. The only reason I can think of is that when we had to heat our solution, we maybe did not let it evaporate enough, and as we saw during our second lesson doing the experiment, our crystals were not dry. So this basically means that there was more substance than what we predicted.
The other option and reason why the percentage yield is more than 100% might be because there were some impurities.

Experiment 2:

Overall this experiment went well, just like the first one, things went like planned. When we made the solution evaporate to dry and make the crystals there was no problems.

As we can see in the results in our second experiment, the percentage yield was lower than 100%. For this, I could find many reasons why that happened: First of all we interrupted the reaction between the substances, we might have lost some solutions while we poured it into other containers, and finally we could have measured the amounts wrong.

Evaluation

Overall even though we faced some complications in the measurements, the experiments went well.
If we had to do this experiment again we would be much more carful while measuring our solutions, and also we should have been much more carful when it came to put the five drops of indicator. Then being more carful when we had to filter our solutions because I think that we lost some of the solutions.
We also took the beaker off the heat to early and that might have also affected our results because our crystals were not fully dry.

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