Titration Lab Essay

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The purpose of this lab was to perform a titration on 10.000 mL of sodium hydroxide solution with 0.10 mol/L sulfuric acid solution. In this lab we performed numerous trials to find the amount of sulfuric acid solution that would neutralize 10.0 mL of sodium hydroxide solution and averaged the trials to find the amount; this data could then be used to find the concentration of the sodium hydroxide solution through solution stoichiometry. To do this we used a burette with the capacity of 50.00 mL with an uncertainty of 0.04 mL, a pipette of 10.000 mL with an uncertainty of 0.015 mL, a clamp stand, a titration flask(an Erlenmeyer flask) and bromothymol blue indicator. The apparatus was set up like so; 0.00mL (graduation at top) Burette contains 0.10M H2SO4(aq) 50.00mL (graduation at bottom) Erlenmeyer flask contains 10.000mL of NaOH (aq) as well as bromothymol blue indicator (10.000mL was measured with a pipette) Evidence Table 1: Raw Data collected from the Titration Lab showing the initial and final burette readings of the titrant of 0.10M ± 0.005M H2SO4(aq) Qualitative Observations Before any sulfuric acid was added, the solution was colourless and clear. After adding three drops of brymothymol blue indicator, the solution was now a clear blue colour. In the first and fourth trial, the bromothymol blue indicator caused the solution in the Erlenmeyer flask to turn a pale yellow colour from the blue colour that the solution already was after the 10.00mL of acid was added. This indicates that the solution was now acidic. In the second, third and fifth trial, the bromothymol blue indicator caused the solution in the Erlenmeyer flask to turn a pale green colour from the blue colour that the solution already was after the respective amounts of acid was added to the solution. This indicates that the solution was now neutral, or close to a pH of 7.

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