Experiment 8 - Experiment 8 Acid-Base Equilibria The...

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Experiment 8 Acid-Base Equilibria The purpose of this experiment was to obtain qualitative values of acid ionization constants be measuring the pH and also to prepare buffer solutions and observe their resistance to changes in pH as compared to non-buffered solutions. Balanced equations for lab reactions: CH 3 COOH(aq) + NaOH(aq) CH 3 COONa(aq) +H 2 O(l) CH 3 COOH(aq) <-->H + (aq) +CH 3 COO - (aq) HCl(aq) + H 2 O(l) H 3 O(aq) + Cl - (aq) NaOH(aq) + H 2 O(l) Na + (aq) + OH - (aq) + H 2 O(l) HC 2 H 3 O 2 (aq) + NaOH Na + (aq) + OH - (aq) + H 2 O(l) + NaC 2 H 3 O 2 (aq) HC 2 H 3 O 2 (aq) + HCl Cl - (aq) + H + (aq) + HC 2 H 3 O 2 (aq) In order to find the acid ionization constant (Ka), acetic acid was titrated with sodium hydroxide and the pH was recorded at each interval (~1.0-.05mL-reference graph in lab report). After the scatter plot was made and the equivalence point was found, Ka was calculated. The Ka of acetic acid was calculated by measuring the pH of a pure acetic acid solution, mixed with various amounts of weak base ultimately solving for Ka using an I.C.E. table. The proceeding step was to observe the resistance to pH change of buffered solution with the addition of strong acid and base. This step was obtained by measuring the pH of a buffered solution and then the pH after the solution was titrated with HCl and NaOH. Finally, this pH change was compared to the change in pH of water
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This note was uploaded on 04/20/2010 for the course CHEM1A/1B Chem Labs taught by Professor Van koppen during the Spring '10 term at UCSB.

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Experiment 8 - Experiment 8 Acid-Base Equilibria The...

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