Equilibrium Constants lab report-Table 1. Equilibrium Constants Data Volume of N
ID: 883034 • Letter: E
Question
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, m pH after each 0.5 mL Color observations vertical rise: see Lab 7 [19]. Figure 2) pH at the equivalence point (should be approximately 8-9) increment Volume of NaOH at equivalence point: 14.5 41 Yellow Volume at half-equivalence p A2 Yellow pH at the half-equivalence point 13.15 4.3 Yellow pH at this point 13 43 Yellow Ka (equilibrium constant 4.6 12.5 Yellow pka -log Ka. 12 48 Dark yellow Experimental Ka of acetic acid: 11.5 5.1 Dark yellow Theoretical Ka of acetic acid 53 Dark yellow Compare your experimental value for the equilibrium constant to the theoretical value 5.S 10.5 Pink Do you notice any variation? If so, why? 10 62 Pink 9.3 10.3 Dark pink 9 10 Light pink 3.3 1.2 Light pink 1. Light pink ilue 7.3 11.4 Light pinkExplanation / Answer
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.
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