Given a buffer made from a weak acid HA and its Conjugate Base A-. the pka of HA is 5.0. the buffer is PH=5.5, the molarity of this buffer is 250ml. Question: What are the molarites of A- and HA?
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A solution at pH 4.3 is made of a weak acid (pKa=5) and its conjugate base. Which species is present at a higher concentration? What is the pH of a solution containing 0.2 M A- and 1 M HA (pKa=5)? Show your work. What is the ratio of conjugate base to acid of an acetic acid solution (pKa=4.8) with pH=4.8? Show your work.
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1. You want to make 125 mL of 0.1 M acetic acid buffer with pH = 5.25. You are given a stock bottle of 1 M acetic acid and a bottle of solid sodium acetate salt (MW = 82 g/mol). The formula for the dissociation of acetic acid is shown here. The Henderson-Hasselbalch equation: pH = pKa + log [A-]/[HA] CH3COOH < ---> CH3COO- + H+ pKa = 4.75 What is the ratio of [A-]/[HA] when your buffer pH is 5.75?
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A weak acid (HA) has pKa 2.77. Assuming that the volumes are additive, calculate the volume (in mL) of 0.500 M HA, 0.500 M NaA, and water required to make 250.00 mL of a buffer with a buffer strength of 0.400 M and (a) pH 2.77; (b) pH 2.25; and (c) pH 3.00.
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