Question

a. Draw the titration curve of 50 mL of 0.01 M HCl (aq) with 0.005 M NaOH (aq). b. For every mL of base added, and until a total of 200 mL, calculate what is present in solution and calculate the pH, plotting it against the volume of base added. c. On the curve you drew, identify the equivalence point (nacid = nbase) and the point at which the pH is equal to the pKa of the acid. d. Now, for part d, draw the titration curve of 50 mL of 0.01 M CH3COOH (aq) (Ka = 1.75x10-5) with 0.005 M NaOH (aq). e. For every mL of base added, and until a total of 200 mL, calculate what is present in solution and calculate the pH, plotting it against the volume of base added. f. On the curve you drew, identify the equivalence point (nacid = nbase) and the point at which the pH is equal to the pKa of the acid.

          a. Draw the titration curve of 50 mL of 0.01 M HCl (aq) with 0.005 M NaOH (aq).
b. For every mL of base added, and until a total of 200 mL, calculate what is present in solution and calculate the pH, plotting it against the volume of base added.
c. On the curve you drew, identify the equivalence point (nacid = nbase) and the point at which the pH is equal to the pKa of the acid.
d. Now, for part d, draw the titration curve of 50 mL of 0.01 M CH3COOH (aq) (Ka = 1.75x10-5) with 0.005 M NaOH (aq).
e. For every mL of base added, and until a total of 200 mL, calculate what is present in solution and calculate the pH, plotting it against the volume of base added.
f. On the curve you drew, identify the equivalence point (nacid = nbase) and the point at which the pH is equal to the pKa of the acid.

Added by Russell P.

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