Lab report of Equilibrium constants: the table has recorded the data of the lab.
ID: 883016 • Letter: L
Question
Lab report of Equilibrium constants:
the table has recorded the data of the lab. I just need help with the questions next to it. the first question which is
Volume of NaOH when solutions turn dark pink/orange answer is 4.5ml
also I would like to know what is the conclusion of this lab?
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
Volume of NaOH when solutions turn dark pink/orange = 14.5-10 = 4.5ml (based on syringe reading)
conclusion
Based on pH values Acetic acid is weak so at starting of titration pH near to 7 idicates it is started to nutralize by NaOH.
When 4.5 ml NaOH addition completed the acetic acid completly converts to salt.
After nutralisation if we continues addition of base the pH value increases which indicates the solution becoming basic.
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