Condumetric and gravemetric lab report

Therefore, there was an error; it could be that the solution was not properly mixed during titration. One possible error is the presence of bubbles in the buret. When the reaction stops, meaning that all the ions have been removed from the reactants then the conduction would be at the lowest point. That is the point of equivalence wherein the ratios of both solutions are the same. After that, start to titrate with increments of 1. The gravimetric determination was more accurate because an exact amount of precipitate was formed. Set up a conductivity probe and open programs by connecting to logger pro.

Result: There was only enough time for one trial. Words:Paragraphs: 8, Pages: 3 Publication date: April 06, Sorry, but copying text is forbidden on this website! The graph below shows the theoretical result which was different from the displayed result.

conductometric titration and gravimetric determination of a precipitate chegg

The colloidal barium hydroxide would make it. Conclusion: In this lab an attempt was made to determine the concentration of a Ba OH 2 solution by using the conductimetrically determined equivalence point of the reaction between Ba OH 2 and H2SO4 and by gravimetric determination.

conductometric titration and gravimetric determination of a precipitate discussion of theory

There was only enough time for one trial. The molarity using the equivalence point was determined to be 0. Abstract: This experiment demonstrated that by titrating barium hydroxide, Ba OH 2 solution with a sulfuric acid. The gravimetric determination was more accurate because an exact amount of precipitate was formed.

Condumetric and gravemetric lab report

The subsequent adding of more H2SO4 caused the conductivity to go again to a new peak, A first when the H2SO4 was added the conductivity was high, Another possible error deals with the colloidal nature of barium hydroxide due to its relatively low solubility.

Data Analysis: 1.

Bubbles would have caused the buret reading to be too high, resulting in a larger equivalence point. With the equivalence point and the stoichiometric relationship, the molarity of barium hydroxide can be determined. Result: There was only enough time for one trial. Conclusion: In this lab an attempt was made to determine the concentration of a Ba OH 2 solution by using the conductimetrically determined equivalence point of the reaction between Ba OH 2 and H2SO4 and by gravimetric determination. The subsequent adding of more H2SO4 caused the conductivity to go again to a new peak, In this case both would be 0. The molarity using gravimetric determination was 0. Then, measure out 60 mL of 0. Data Analysis: 1. The molarity using the equivalence point was determined to be 0. That is the point of equivalence wherein the ratios of both solutions are the same. The gravimetric determination was more accurate because an exact amount of precipitate was formed.

Since they were ionic compounds, then the lowest conductivity reading was the point of equivalence because at that reading they were both at a non-ionic state since all their ions have been completely reacted.

The theory is that during titration as the solutions react the ions in both solutions cause the conductance of electricity.

One possible error is the presence of bubbles in the buret. From calculation, the molarity of the Ba OH 2 between 0. Data Analysis: 1. With the equivalence point and the stoichiometric relationship, the molarity of barium hydroxide can be determined. Another possible error deals with the colloidal nature of barium hydroxide due to its relatively low solubility. After that, start to titrate with increments of 1. Abstract: This experiment demonstrated that by titrating barium hydroxide, Ba OH 2 solution with a sulfuric acid,. The molarity using the equivalence point was determined to be 0. Since they were ionic compounds, then the lowest conductivity reading was the point of equivalence because at that reading they were both at a non-ionic state since all their ions have been completely reacted. In this case both would be 0. The molarity using gravimetric determination was 0. The colloidal barium hydroxide would make it. Then, measure out 60 mL of 0. When the reaction stops, meaning that all the ions have been removed from the reactants then the conduction would be at the lowest point.
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