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1. How Did The Final Naoh Molarities Compare For Each Trial?

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Conclusion: Based on the results of molarity from Trials 1, 2, and 3, it is concluded that our experimental for each trial is .410M NaOH, .410M NaOH, and .450M NaOH. The actual molarity of the NaOH concentration used was found to be 1.5M NaOH. The percent error of the results resulted in 72%. The large error may have occurred due to over titration of the NaOH, as the color of the solution in the flask was a darker pink in comparison for the needed faint pink. Discussion of Theory: Titration is the basis of the Titration Lab because the goal of the lab was to titrate. Titration is determining the concentration of a solution by neutralizing it with another known concentration. We titrated the NaOH in the HCl. The titration caused a …show more content…

How did the final NaOH molarities compare for each trial? Were they similar? The results of the trials were reproducible in the sense that they all showed consistency in molarities. 2) Why were you able to pour the products down the sink for this lab? What were your two products of this reaction? The two products formed from the titration were table salt and water, both of which could be dumped into the sink without any harm being caused. 3) What is the balanced chemical equation for this titration? NaOH + HCl → NaCl + H2O 4) Define: Standard Solution: Titration: A lab procedure used to determine the concentration of a solution by neutralizing it with a solution of another known concentration. Endpoint: pH at which indicator changes color and titrating is stopped. Volumetric Analysis: A measurement of volume of a solution of a known concentration which is used to determine the analyte’s concentration. Gravimetric Analysis: A technique to determine the analyte based on its measured mass. Equivalence Point: pH at which the moles of H3O¬+ equal the moles of OH- and solution is neutralized. Indicator: A weak acid or base and its conjugate ion whose color changes as pH

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