Calculate the pH of a buffer system containing 1.0 M CH3COOH and 1.0 M CH3COONa.(Ka of acetic acid is 1.8 x 10^-5)
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what is the ph of a buffer that consists of .45m ch3cooh and .35 m ch3coona? ka=1.8*10^-5
(a) Suppose you have two stock solutions 0.50 M CH3COOH and 0.50 M CH3COONa. Is these were mixed together would this be a buffer? How many milliliters of sodium acetate do you need to add to obtain a pH of 5.45 if you start with 100 mL of acetic acid? Ka = 1.8 X 10-5
You need to prepare a solution with pH = 4.50. You have the following 0.15 M solutions available in the laboratory: CH3COOH, CH3COONa. How many milliliters of each solution would you use to make one liter of this buffer solution?
Ka acetic acid = 1.8