when 10.00 ml of .200 M NaOH is added to 25.00 ml of .200 M acetic...
7 A 25.00 ml acetic acid solution is trated with 0.110 M NaOH. The end point is reached after 18.55 mL NaOH has been added. a. What was the original concentration of acetic acid? 5 pts bWhat is the initial pH of the acetic acid solution? 5 pts was the plh after the adition of 5.00 mL NaOH to the original solution? 5 pts d. What is the pH at the equivalence point? 5 pts e. What is the pH...
6. How many mL of 0.2 M sodium acetate should be added to 200 mL of 0.2 M acetic acid to make a buffer of pH 5.5? (refer to Table 2-2 on page 60 for pKa values). What is the molarity of the resulting buffer with respect to acetate (acetate + acetic acid)? 7. How many mL of 0.2 M HCl should be added to 50 mL of 0.2 M Tris base (Trishydroxymethyl aminomethane) to make a buffer of pH...
How much volume of a 0.102 M NaOH solution must be added to 25.00 ml of a 0.075 M solution of benzene-1,2,3-tricarboxylic acid to obtain a pH equal to 4.80? pKa values: pKa1 = 2.86, pka2 = 4.30 and pka3 = 6.28.
25.0 mL of 0.75 M NaOH is added to 750.0 mL of a 0.750 M acetic acid solution. What is the pH of the solution before and after the NaOH has been added?
14 mL of 0.0100 M NaOH are added to 25.0 mL of 0.0100 M acetic acid. What is the pH of the resulting solution?
You have 775 mL of an 0.15 M acetic acid solution. What volume (V) of 1.80 M NaOH solution must you add in order to prepare an acetate buffer of pH = 4.65? (The pKa of acetic acid is 4.76.)
You have 125 mL of an 0.19 M acetic acid solution. What volume (V) of 1.10 M NaOH solution must you add in order to prepare an acetate buffer of pH = 4.20? (The pKa of acetic acid is 4.76.)
You have 775 mL of an 0.49 M acetic acid solution. What volume (V) of 2.40 M NaOH solution must you add in order to prepare an acetate buffer of pH = 4.56? (The pKa of acetic acid is 4.76)
A titration of 25.00 mL of an acetic acid solution with 0.1220 M NaOH solution starts at a burette reading for NaOH of 0.17 mL. The phenolphthalein indicator turns light pink in the acid solution for over 30 seconds at a burette reading of 36.32 mL. The volume of NaOH used to neutralize the acid is _______ mL.
Consider the titration of the titration of 50.0 mL of 0.100 M acetic acid (HC2H2O2) with 0.100 M. The pka = 4.76. d. Determine the pH after 50.0 mL of titrant (NaOH) have been added. This is the equivalence point. All of the acid has been converted to its conjugate base, pH is determined by the equilibrium for the conjugate base