2.00×10–3 mole sample of pure acetylsalicylic acid was dissolved in 15.00 mL of water and then titrated with 0.100 NaOH(aq). The equivalence point was reached after 20.00 mL of the NaOH solution M had been added. Using the data from the titration, shown in the table below, determine (i) the of the acid dissociation constant, for acetylsalicylic acid and Ka, (ii) the pH of the solution after a total volume of 25.00 mL of the NaOH solution had been added (assume that volumes are additive). Volume of pH 0.100M NaOH Added (mL) 0.00 2.22 5.00 2.97 10.00 3.44 15.00 3.92 20.00 8.13 25.00 ? 20. HOBr(aq) H+(aq) + OBr–(aq) = 2.3 10–9 Ka ↔  Hypobromous acid, HOBr, is a weak acid that dissociates in water, as represented by the equation above. Calculate the value of [H+] in an HOBr solution that has a pH of 4.95. the equilibrium constant expression for the ionization of HOBr in water, then calculate the concentration of HOBr(aq) in an HOBr solution that has [H+] equal to 1.8 10–5 M.  solution of Ba(OH)2 is titrated into a solution of HOBr. (i) Calculate the volume of 0.115 Ba(OH)2(aq) needed to the equivalence point when titrated M into a 65.0 mL sample of 0.146 HOBr(aq). M
2.00×10–3 mole sample of pure acetylsalicylic acid was dissolved in 15.00 mL of water and then titrated with 0.100 M NaOH(aq). The equivalence point was reached after 20.00 mL of the NaOH solution had been added. Using the data from the titration, shown in the table below, determine (i) the of the acid dissociation constant, Ka, for acetylsalicylic acid and (ii) the pH of the solution after a total volume of 25.00 mL of the NaOH solution had been added (assume that volumes are additive). Volume of 0.100M NaOH Added (mL) pH 0.00 2.22 5.00 2.97 10.00 3.44 15.00 3.92 20.00 8.13 25.00 ? 20. HOBr(aq) ↔ H+(aq) + OBr–(aq) Ka = 2.3  10–9 Hypobromous acid, HOBr, is a weak acid that dissociates in water, as represented by the equation above. Calculate the value of [H+] in an HOBr solution that has a pH of 4.95. the equilibrium constant expression for the ionization of HOBr in water, then calculate the concentration of HOBr(aq) in an HOBr solution that has [H+] equal to 1.8  10–5 M. solution of Ba(OH)2 is titrated into a solution of HOBr. (i) Calculate the volume of 0.115 M Ba(OH)2(aq) needed to the equivalence point when titrated into a 65.0 mL sample of 0.146 M HOBr(aq).
unit_8b_acid_base_class_packet.docx