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A student was titrating a solution of HCAH,02 with a Sr(OH)2 solution. Determine the pH at a particular point in the titration. Do this by constructing a BCA table and determining the pH. Complete Parts 1-2 before submitting your answer. 1 2 NEXT > 40.0 mL of a 0.200 M HC4H70, solution was titrated with 100 mL of 0.100 M Sr(OH)2 (a strong base). Fill in the ICE table with the appropriate value for each involved species to determine the moles of reactant and product after the reaction of the acid and base. You can ignore the amount of water in the reaction. HC4H, O2(aq) + OH (aq) H2O(1) C4H702" (aq) Before (mol) Change (mol) After (mol) RESET 0.100 0.200 2.00 * 10- -2.00 x 10" 8.00 x 10" 8.00 * 10" 1.00 x 10 -1.00 x 10 1.20 x 10 -1.20 x 10 % 2.00 x 10 -2.00 x 10 +
A student was titrating a solution of HC4H7O2 with a Sr(OH)2 solution. Determine the pH at a particular point in the titration. Do this by constructing a BCA table and determining the pH. Complete Parts 1-2 before submitting your answer. < PREV 1 2 The value of Ka for HC4H2O2 is 1.5 x 10-5. Based on the result of the acid-base reaction, determine the pH of the solution.. pH = RESET 0 4.42 6.21 1.00 1.85 12.25 9.85 10.12 11.03 12.93 12.08 1.07 14.91