Volume of NaOH when solution turns pink : 4.5 mL Volume of NaOH at the equivalen
ID: 883037 • Letter: V
Question
Volume of NaOH when solution turns pink : 4.5 mL
Volume of NaOH at the equivalence point : 4.75 mL
pH at the equivalence point : 8.25
Volume at half-equivalence point : 2.375 mL
pH at half equivalence point : 4.75
pH = pKa at this point
Ka (equilibrium constant) = 1.78 x 10^-5
Experimental Ka of actic acid = 1.78 x 10^-5
Theoretical value of Ka of acetic acid = 1.75 x 10^-5
The values of Ka of theoretical and experimental are very close to one another. So their is almost no difference observed between the two values
I got these answers but i am missing the conclusion of the project and Volume of NaOH at equivalence point?
Equilibrium Constants lab report-Table 1. Equilibrium Constants Data Volume of NaOH when solution turns dark pink/orange: 4.5ml Volume of NaOH at the equivalence point (the point on the graph midway between the Syringe Reading, mL pH after each 0.5 mLColor Observations vertical rise: see Lab 7 [19], Figure 2) pH at the equivalence point (should be approximately 8-9) Volume of NaOH at equivalence point: Volume at half-equivalence point pH at the half-equivalence point pH = pka at this point Ka (equilibrium constant) pKa=-log Ka Experimental Ka of acetic acid: Theoretical Ka of acetic acid: Compare your experimental value for the equilibrium constant to the theoretical value Do you notice any variation? If so, why? increment 14.5 14 13.5 13 12.5 12 11.5 ellow .2 4.3 4.3 4.6 4.8 5.1 5.3 5.8 6.2 10.3 10.9 11.2 11.4 11.4 ellow Yellow Yellow Yellow Dark yellow Dark yellow Dark yellow Pink Pink Dark pinlk Light pinlk Light pink Light pinlk Light pinlk 10.5 10 9.5 9 8.5 lue 7.5Explanation / Answer
The project concludes that the pH of solution of weak acid and strong base titration is not neutral even at equivalence point.
Equivalence point is the point where moles of acids equals to moles of base
Moles = Moalrity x volume
So we can determine the equivalence point if we know the moalrity of NaOH and acid and volume of acid used in the titration.
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