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    Chemis Report

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    sanjesh_baskaran
    The document describes an experiment to determine the concentration of sulfuric acid using a standard sodium hydroxide solution. 25cm3 of sulfuric acid was titrated with sodium hydroxide until the first permanent pink color was observed, which indicated the reaction was complete. This procedure was repeated 3 times and the results were averaged. The average titration showed that 27.80cm3 of sodium hydroxide solution was required to neutralize the 25cm3 sulfuric acid sample. Calculations were shown to determine the molarity of the sulfuric acid from these results.

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    Chemis Report

    Uploaded by

    sanjesh_baskaran
    8 views2 pages
    The document describes an experiment to determine the concentration of sulfuric acid using a standard sodium hydroxide solution. 25cm3 of sulfuric acid was titrated with sodium hydroxide until the first permanent pink color was observed, which indicated the reaction was complete. This procedure was repeated 3 times and the results were averaged. The average titration showed that 27.80cm3 of sodium hydroxide solution was required to neutralize the 25cm3 sulfuric acid sample. Calculations were shown to determine the molarity of the sulfuric acid from these results.

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    The document describes an experiment to determine the concentration of sulfuric acid using a standard sodium hydroxide solution. 25cm3 of sulfuric acid was titrated with sodium hydroxide until the first permanent pink color was observed, which indicated the reaction was complete. This procedure was repeated 3 times and the results were averaged. The average titration showed that 27.80cm3 of sodium hydroxide solution was required to neutralize the 25cm3 sulfuric acid sample. Calculations were shown to determine the molarity of the sulfuric acid from these results.

    Copyright:

    Attribution Non-Commercial (BY-NC)
    Download as DOCX, PDF, TXT or read online from Scribd
    Download as docx, pdf, or txt
    8 views2 pages

    Chemis Report

    Uploaded by

    sanjesh_baskaran
    The document describes an experiment to determine the concentration of sulfuric acid using a standard sodium hydroxide solution. 25cm3 of sulfuric acid was titrated with sodium hydroxide until the first permanent pink color was observed, which indicated the reaction was complete. This procedure was repeated 3 times and the results were averaged. The average titration showed that 27.80cm3 of sodium hydroxide solution was required to neutralize the 25cm3 sulfuric acid sample. Calculations were shown to determine the molarity of the sulfuric acid from these results.

    Copyright:

    Attribution Non-Commercial (BY-NC)
    Download as DOCX, PDF, TXT or read online from Scribd
    Download as docx, pdf, or txt
    of 2

    Name Exp No Title

    : : : 1 Determine the concentration of sulphuric acid using standard hydroxide solution. 1) 25.00cm3 of sulphuric acid was pipetted into a conical flask. 2) 2-3 drops of phenolphthalein is added and the solution with the standard NaOH was pipetted until the first permanent pink colour was observed. 3) The procedure was repeated for consistent results.

    Procedure

    Results : Burette readings Titration No Rough


    3

    Average 1 9.00 cm3 37.40 cm3 28.40 cm3 2 5.00 cm3 32.50 cm3 27.50 cm3 3 7.00 cm3 34.50 cm3 27.50 cm3

    Initial Reading Final Reading Volume of NaOH used/cm3

    4.00 cm

    33.00 cm3 29.00 cm3

    Discussion :

    Carefully use sodium hydroxide to titrate sulphuric acid so that volume of sodium hydroxide used is not in excess. First permanent pink colour is observed when the reaction between sulphuric acid and sodium hydroxide is completed. Procedure is repeated for 3 times and calculate the average results to get a more accurate results.

    Conclusion :

    25.00cm3 of sulphuric acid required 27.80cm3 of the sodium hydroxide solution for complete reaction.

    Calculations :

    1.

    Use the values for the averaged total volume of NaOH added and the NaOH concentration to calculate the moles of NaOH used. Average total volume of NaOH = (28.40 + 27.50 + 27.50)cm3 3 = 27.80 cm3 Concentration of NaOH = 4.0gdm-3 Mass of NaOH = 4.0gdm-3 x (27.80 cm3 1000) = 0.1112g
    n

    ( NaOH) = mass molar mass = 0.1112g (23 + 16 + 1) = 2.78 x 10-3 mol

    2.

    Write and balance an equation to show how H2SO4 reacts with NaOH in a neutralization equation. H2SO4 + 2NaOH Na2SO4 + 2H2O

    3.

    Calculate the moles of H2SO4 used in the reaction, using the moles of NaOH calculated in (1) and the balanced equation in (2). 1 mol H2SO4 2 mol NaOH X 2.78 x 10-3 mol NaOH X = 2.78 x 10-3 mol 2 = 1.39 x 10-3 mol

    4.

    Calculate the molarity of the H2SO4 , using the moles of H2SO4 calculated in (3) and the volume of H2SO4 recorded in your table. Molarity of H2SO4 = 1.39 x 10-3 mol 0.025dm3 = 0.0556 moldm-3

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