Top-Rated Free Essay
Preview

Percent Yield of Calcium Carbonate

Good Essays
1338 Words
Grammar
Grammar
Plagiarism
Plagiarism
Writing
Writing
Score
Score
Percent Yield of Calcium Carbonate
SCH 3U0
May 7th 2013

Percent Yield of Calcium Carbonate
Introduction:

The purpose of this experiment is to examine the percent yield of a precipitate in a double displacement reaction. A solution of calcium citrate and sodium carbonate were mixed together, then the products were filtered out as so only the precipitate remained. The filtered paper was then dried and the mass of the precipitate in the experiment divided by the theoretical mass of the precipitate from the calculated gave the percent yield. The percent yield that was acquired is about 69.1%.

The chemical reaction that took place was that sodium displaced calcium in a solution of calcium nitrate, and that calcium displaced sodium in a solution of sodium carbonate. The resulting products were solid calcium carbonate and aqueous sodium nitrate (equation 1).

To calculate the theoretical yield, the moles of sodium carbonate and calcium nitrate were calculated to find the limiting reagent. Then the moles of the limiting reagent (calcium nitrate) were used in ratio with the precipitate ( 1:1), calcium carbonate, to find how many moles of the solid were produced, then to conclude the mass of the precipitate (equation 2).

The percent yield was calculated by taking the mass of the precipitate that was observed in the reaction(actual yield), divided by the mass of the precipitate that was hypothesized in the calculations (theoretical yield). This number was multiplied by a hundred to determine the percent yield (equation 4).

Equation 1:

Na2CO3 (aq) + Ca(NO3)2 (aq) CaCO3 (s) + 2NaNO3 (aq)

Equation 2:

n = OR mole =

Equation 3:

Percent Yield = × 100

Hypothesis:

The law of conservation of mass states that the mass of the reactants must be equal to the mass of the products; no mass can be created or destroyed. In relation to this experiment, the theoretical yield is the calculated mass based on if the result has a percent yield of 100%. The theoretical yield of the precipitate is mass of approximately 0.695 g (appendix A). Therefore if the percent yield is close to 100% (an actual yield ≈ 0.694), then less experimental errors occurred and the more accurate the result.

Procedure:

1. To ensure safety, goggles were worn.
2. A 150ml beaker with a mass of 68.2g was filled with sodium carbonate until the total mass was 69.08g. The mass of the sodium carbonate contained was calculated and recorded to be 0.88g.
3. Another 150ml beaker with a mass of 72g was filled with calcium nitrate until the total mass was 73.14g. The mass of the calcium nitrate contained was calculated and recorded to be 1.14g .
4. Using a graduated cylinder, 50ml of distilled water was added to each of the beakers
5. A different stirring rod was used to dissolve each of the solids in the beakers.
6. Then the calcium nitrate solution beaker was poured into the other beaker that contained the sodium carbonate solution and mixed thoroughly with a stirring rod.
7. A filter paper, massed to be 0.75g, was subsequently set up (diagram 1)
8. The filter paper was placed inside a funnel and the funnel was placed into a clean 250ml flask.
9. The products of the mixed solutions were slowly and hesitantly poured into the funnel, until nothing remained in the beaker (diagram 2)
10. Then the funnel paper was removed and set to dry
11. The day after, the funnel paper with the precipitate was weighed to be 1.25g and subtracted from the mass of the funnel paper by itself to get an actual yield of 0.48g of precipitate.

Diagram1 : Fold at the dotted line. Open with three folds on one side and place in the funnel with a few drop of water so it sticks to the funnel.

Observations:

Table 1: The recorded masses of materials and results in the experiment
Material
Mass
Beaker 1
68.2g
Beaker 1 with sodium carbonate
69.08g
Sodium carbonate
0.88g
Beaker 2
72g
Beaker 2 with calcium nitrate
73.14g
Calcium nitrate
1.14g
Funnel paper
0.75g
Dried precipitate with funnel paper
1.25
Calcium carbonate precipitate
0.48g

Analysis:

The percent yield was calculated to be approximately 69.1%. This was concluded by dividing the mass of the mass observed in the reaction divided by the mass calculated that was theoretically supposed to be produced; actual yield divided by theoretical yield (appendix A).

Conclusion:

The percent yield of the calcium carbonate is 69.1%. This means that less precipitate than was expected was produced due to systematic errors that occurred, causing deviation and a result that is inaccurate.

A systematic error that is hypothesized to have occurred is that some of the precipitate made it through the filter. When the two solutions were mixed, a precipitate of calcium carbonate was formed. The precipitate with the products when filtered through the filter funnel must not have had enough time for the reaction to reach its completion. The observation that the flask with the filtered products was foggy only helps to confirm the point that some of the precipitate made it through the filter. This causing a decrease in the actual yield, consequently leading to a decrease in the percent yield. A solution to this error for future reference would be to use a catalyst to speed up the reaction, or by simply giving the reaction more time so that the net ionic equation of the reactants could form into a precipitate completely .

Another systematic error that may have occurred is loss of material during transfer. In many instances, substances had to moved from one container to another, stored, poured, and all these transfers are imperfect. Substances could have stuck to the sides of the beakers, to the stirring rods, to the tissue paper under the drying filter paper and precipitate. This excessive loss of matter causes a decrease in the actual yield of the precipitate, and coherently leading to a decrease in the percent yield, lowering the accuracy of the experiment. For this problem to be avoided, using more advanced tools and being more careful when transferring products would be helpful.

A third systematic error may be due to the result of evaporation. When the two solutions of sodium carbonate and calcium nitrate were mixed, it is not ensured that all of the reactants that could be produced (according to the limiting reagent) were reacted. Some of the mass could have been lost and evaporated due the warm temperature in the room due to the season, and the energy produced from the large mass of people in the room and their friction. This causes a mass of the precipitate to be less than expected and therfore decreasing the percent yield accuracy. To avoid this, covering the reactant beakers would create an equilibrium, causing the amount of reactant that is evaporating equal to the amount of reactant that is condensing back in (figure 1), or by decreasing the temperature from the thermostat in the room so that the room temperature is below the boiling point of the solutions.

Applications to Real World:

Percent yield is essential the chemical manufacturing and engineering business. When the reactants are loaded into the reactor processor, the actual yield is taken and divided by the theoretical yield. In terms of benefits to the company and their economic status, having a higher percent yield would be a plus for the company, saving the company valuable money on reactants and resulting in a higher net profit; the highest amount of products produced , in the least amount of money.

It also would be more environmentally advantageous to them because less fuel and materials are being wasted, which could be used as an advertising strategy as using their products would be environmentally friendly in the eyes of the consumer . Therefore, it would be considered the chemist's job to improve the percent yield of his or her company, similarly to how this experiment was conducted, and how underlying errors were identified to improve future results.

Appendix A
Calculating Percent Yield

Limiting Reagent:
Na2CO3 (aq) + Ca(NO3)2 (aq) CaCO3 (s) + 2NaNO3 (aq)

n (Na2CO3) =

= = 8.303 × 10-3 mol of sodium carbonate

n (Ca[NO3]2) =

= = 6.948 × 10-3 mol of calcium nitrate

Theoretical Yield: =

moles of CaCO3 =0.0069478 =

Theoretical yield of CaCO3 = 6.95 × 10-1g

Percent Yield

Percent Yield = × 100 Percent Yield of Calcium Carbonate = ×100
= 69.1%

You May Also Find These Documents Helpful

  • Better Essays

    Abstract: Using hypochlorous acid to convert secondary alcohol called cyclododecanol to the corresponding ketone which is cyclododecanone by oxidation.…

    • 708 Words
    • 3 Pages
    Better Essays
  • Powerful Essays

    Abstract: The objective of this lab is to calculate the theoretical, actual, and percent yield of the product from a precipitation reaction. It is also to learn concepts of solubility and the formation of a precipitate.…

    • 597 Words
    • 3 Pages
    Powerful Essays
  • Good Essays

    Experiment 9 okiemute

    • 589 Words
    • 3 Pages

    The objectives of this experiment are to predict the amount of product produced in a precipitation reaction using stoichiometry, to accurately measure the reactants and products of the reaction, to determine the actual yield vs. the theoretical yield and to calculate the percent yield. A Precipitation reaction begins by combining two aqueous solutions to form a precipitate, an insoluble product that is also a solid. With my knowledge of the measuring scale, I was able to use the scale with no problem throughout the whole experiment. The mass of the weighing dish was 0.5 grams.…

    • 589 Words
    • 3 Pages
    Good Essays
  • Satisfactory Essays

    Stoichiometry Lab Report

    • 783 Words
    • 4 Pages

    Purpose: The purpose of this lab is to find the limiting reactant, also to find the percentage yield and percentage purity of the reaction that happens between Calcium Chloride and Sodium Carbonate. The other purpose was to know how the reaction can be balanced and created.…

    • 783 Words
    • 4 Pages
    Satisfactory Essays
  • Powerful Essays

    Conclusion: The objective of the experiment is to predict the amount of product produced in a precipitation reaction using stoichiometry. Secondly, the experiment accurately measures the reactants and products of a reaction. Also, the experiment is to determine actual yield vs. theoretical yield and to calculate the percent yield. For example in this experiment, we were able to predict that we need 0.72g of Na-2CO3 to fully react with 1g of CaCl2-.2H2O. Another example is that, we calculate the amount of…

    • 567 Words
    • 3 Pages
    Powerful Essays
  • Powerful Essays

    Chem Ia Lead

    • 990 Words
    • 4 Pages

    The qualitative data taken was that the compound created was a yellow precipitate, and when the water was poured through the funnel in order to strain the precipitate, it retained much of it, making the ending mass of the precipitate far more than the Theoretical yield (4.60 g, which is a percent error of about 259%). The two substances mixed together (Pb(NO3)2 and KI) were white in color, and resembled a sort of powdery substance.…

    • 990 Words
    • 4 Pages
    Powerful Essays
  • Good Essays

    I will have the same mass of the different types of metal carbonates. To control this I will weigh the carbonates and make sure its the same mass for each time when we heat it.…

    • 1178 Words
    • 5 Pages
    Good Essays
  • Good Essays

    Lab 3 no name

    • 1348 Words
    • 5 Pages

    Experiment and Observations: As I performed the lab, I had to retrieve all my equipment’s from my labpaq. As I started to setup, I had to weigh out 1.0 gram of CaCl2*2H2O on the digital scale. After it was weighed, it was added to the 100 mL beaker and 25 mL of distilled was added and stirred. Next, I had to figure out the amount of the second reactant, so that it can be added to the solution. I had to perform stoichiometry to figure out the amount of Na2CO3 is needed to make a precipitate of calcium carbonate. After the calculations, I arrived at .72 grams of Na2CO3 and rounded to the nearest tenth to mix with 25 mL of distilled water. After both of the reactants were mixed separately with distilled water, they both were clear color. As soon as you added the solution of Na2CO3 to CaCl2*2H2O the color of solution changed to a cloud white color. When both solutions are mixed, the paper filter that was provided with the lab must be weighed and recorded. Then you pour the solution into the paper filter to filter out the precipitate and dry the filter to weigh the mass of the precipitate when it dries. After it dried, it was weighed and stoichiometry was performed to see what the…

    • 1348 Words
    • 5 Pages
    Good Essays
  • Good Essays

    The purpose of this experiment is to demonstrate a precipitation reaction combined with stoichiometry. The experiment also provided a method to improve substance measurement with utilizing measuring tools e.g. digital scales, beakers, and cylinders.…

    • 578 Words
    • 3 Pages
    Good Essays
  • Better Essays

    Honors Chemistry 1 Notes

    • 1026 Words
    • 4 Pages

    -The mass put into the reaction will be the same as the mass put out of the reaction.…

    • 1026 Words
    • 4 Pages
    Better Essays
  • Good Essays

    A Paper

    • 1140 Words
    • 5 Pages

    The precipitated calcium carbonate is then filtered, dried, and weighed. The moles of calcium carbonate, CaCO3, are equal to the moles of Group 1 metal carbonate, M2CO3, added to the original solution. Dividing the mass of the unknown carbonate by the moles of calcium carbonate yields the formula weight, and thus the identity, of the Group 1 metal carbonate.…

    • 1140 Words
    • 5 Pages
    Good Essays
  • Satisfactory Essays

    4.08 Percent Yield

    • 231 Words
    • 2 Pages

    The product’s mass would be greater making the calculations adjust. If my actual yield is…

    • 231 Words
    • 2 Pages
    Satisfactory Essays
  • Powerful Essays

    Chemistry Test

    • 792 Words
    • 4 Pages

    16) What is the law of conservation of mass? The mass of products has to _____ the mass of reactants.…

    • 792 Words
    • 4 Pages
    Powerful Essays
  • Powerful Essays

    The crystallinity, morphology, structure, shape and molecule size of precipitated calcium carbonate were directly influenced by the stirring action during the carbonation process. As depicted in the Fig. 1, SEM images of nano CaCO3 precipitated at different stirring rate varied from 700, 800, 900, 1000, 1100 and 1200 rpm had shown significant differences in morphology structure influenced by agitation rate, respectively. Results revealed that in Fig. 1 (a) and (b) the particle morphology was tended to rhombic-calcite. Meanwhile, Fig. 1 (c) and (d) showed structured more likely to needlelike-aragonite and Fig. 1 (e) and (f) were indicating to spherical-vaterite. This can be explicated from the perspective of the co-effects of micro-macro mixing and mass transfer theory. At low multiple impeller stirring rotation speed, the level of supersaturation had a wide variety of different local areas in the interface region between particle and agitation medium. Meanwhile, when the multiple impeller stirring rotation speed was excessively high, the micro-macro mixing was significantly increased, and the CO2 transfer coefficient was additionally intensified into the system. Higher multiple impeller stirring rotation speed also will provide a better homogeneity and heterogeneity of nucleation of nano-precipitated CaCO3. This finding was supported by previous researchers' work such as M. Wang et. al., Laifeng et. al. and Martin Back et. al. which described and discussed deeply about the transformation of CaCO3 morphology, influenced by numerous parameters…

    • 2090 Words
    • 9 Pages
    Powerful Essays