Takaguchi, Y. Calculating the theoretical yield of the precipitate CaCO3 : In the reaction that occurred, calcium chloride was found to be the limiting reactant.
This would have increased the percent yield of the three trials and made the experiment more accurate. This means that once all of the CaCl2 has reacted, no more of the products will form.
Colloid Interf. Nikos, Analyst Deng, J. Using this value for the number of moles of solute present, and the measured volume of solution, concentration can be determined as such: Nadkarni 3!
Google Scholar Also in Trial 3, a qualitative observation was that I noticed an unwanted speck of dust on the filter paper after I took it out of the overnight drying location.
Cacl2 + na2so4
According to this balanced chemical equation representing the double displacement reaction that occurs, the ideal stoichiometric ratio of reactants CaCl2 and Na2CO3 is 1 mole CaCl2 to 1 mole Na2CO3. A possible solution for such a condition could have been to use larger filter papers if available, seeing as even if an erroneous fold did occur in the paper, it would not allow solution to go through without filtration. Press, Beijing, Sakuda, and H. Kato, Adv. CrossRef Google Scholar 9. At this point I could not extract it from the dry precipitate sample, because that would risk extracting some of the precipitate as well and would cause an even larger random error in the mass readings. Distilled water was used to run any extra NaCl that might have been caught in the filter; however, a better process of separation might have helped. Growth , This would have increased the percent yield of the three trials and made the experiment more accurate. Kato, A.
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