A volume of 0.300 L contains, in addition to water, also 0.250 M acetic acid and 0.560 M sodium acetate. 3 mL of 2 M hydrochloric acid (0.0060 mol hydrochloric acid) is added to this buffer. a) Calculate the pH of the original solution using Henderson-Hasselbalchs equation. pKa (CH3COOH) = 4.75 b) Calculate the pH of the original solution based on the equilibrium that actually occurs in the solution. The experimental acid equilibrium constant for acetic acid, Ka = 1.80 x 10-5 c) How well the pH calculated in (a) and (b) matches. If there is a difference, what is it? on? What is your conclusion about when it is appropriate to use Henderson-Hasselbalchs the equation? d) What is the pH of the new solution, after the addition of hydrochloric acid?

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Acid Base Titration

An acid-base titration is the method of quantitative analysis for determining the concentration of an acid and base by exactly neutralizing it with a standard solution of base or acid having known concentration.