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ACID-BASE titration

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Introduction

Chemistry Lab Report Acid- Base Titration Using a pH Meter Acid- Base Titration Using a pH Meter Data Collection: Strong acid- Strong base titration: Both NaOH (Strong base) and HCl (Strong acid) are colorless. NaOH was placed in a burette to titrate 25.00 cm� of 0.1 moldm?� HCl that is poured into a conical flask. A pH electrode was used to measure the pH. During titration there was no color change, neither change in temperature nor smell. Table1: The volume of NaOH added from the burette to HCl in the flask and pH of the resulting solution. # Volume of 0.1moldm?� NaOH /cm��0.05 cm� pH / �0.1 0 0.00 1.2 1 2.00 1.1 2 4.00 1.2 3 8.00 1.1 4 10.00 1.2 5 12.00 1.2 6 14.00 1.4 7 15.00 1.4 8 16.00 1.6 9 17.00 1.8 10 18.00 1.7 11 18.50 1.8 12 19.00 1.8 13 19.50 1.8 14 20.00 2.1 15 20.50 2.2 16 20.70 2.3 17 20.90 2.5 18 21.10 2.8 19 21.20 2.9 20 21.50 3.6 21 21.60 4.7 22 21.80 5.7 23 21.90 5.7 24 22.00 6.1 25 ...read more.

Middle

# Volume of 0.1moldm?� NaOH /cm��0.05 cm� pH / �0.1 0 0.00 2.4 1 2.00 3.1 2 4.00 3.4 3 6.00 3.7 4 8.00 3.9 5 10.00 4.1 6 12.00 4.4 7 14.00 4.6 8 15.00 4.6 9 16.00 4.8 10 17.00 4.9 11 18.00 5.1 12 18.50 5.2 13 19.00 5.4 14 19.50 5.7 15 19.70 5.8 16 20.10 6.1 17 20.30 6.5 18 20.50 7.5 19 20.70 8.8 20 20.70 8.6 21 20.90 8.8 22 21.10 9.2 23 21.30 9.5 24 21.50 9.7 25 21.70 10.0 26 21.90 10.0 27 22.10 10.3 28 22.30 10.6 29 22.50 10.6 30 22.70 10.6 31 22.90 10.7 32 23.10 11.0 33 23.30 11.0 34 23.50 11.0 35 24.00 11.0 36 25.00 11.3 37 26.00 11.3 38 30.00 11.4 39 35.00 11.7 40 40.00 11.7 41 45.00 11.8 42 50.00 11.8 Data Processing and presentation: Figure1: effect of adding strong alkali to strong acid on the pH of the resulting solution. Since the acid is strong, the initial pH before adding alkali was low and equaled 1.2. ...read more.

Conclusion

Weak acid dissociates partially and has a higher pH than strong acid. As the alkali was added slowly, the [H3O+] decreased. OH?�(aq) + H3O+1 (aq) - 2H2O (l) The pH increased slowly till it reached 6. After that a small addition of the strong alkali caused the pH to jump to 11. This is the vertical region on the graph. It is more in the alkaline region than the acidic region. The rapid change is caused by the low [H3O+]. Addition on the strong alkali increased [OH?�] and thus the pH rapidly. Because the addition of the strong alkali continued, the pH continued to increase slowly. The final pH was almost 12 because it is a strong alkali. The equivalence point is almost 8. It is not equal to 7 because the conjugate base of the weak acid has a tendency to accept a proton from water and OH?� is produced. The solution turns basic. A?� + H2O - HA + OH? Because both the acid and base are monoprotic with equal concentrations the volume of the string base used was almost equal to the volume of the weak acid. ...read more.

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