Calculate the equilibrium pH for a buffer that consists of 0.35M weak acid (HA) and 0.65M of its conjugate base (A-) using both the chemical equilibrium approach AND the Henderson-Hasselbalch equation. pKa of HA = 4.95. Show all your work. Do not use approximation or assumption for chemical equilibrium approach. Do your results agree with each other? Briefly explain the reasoning behind why it does or does not match.
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Calculate the equilibrium pH for a buffer that consists of 0.35M weak acid (HA) and 0.65M...
An unknown weak acid, HA, is used to create a buffer solution. When the concentrations are {HA} = 0.500 M and {A–} = 1.048 M, the pH of the buffer solution is 5.49. Use the Henderson-Hasselbalch equation to find the pKa of the weak acid. Henderson-Hasselbalch equation: pH = pKa + log({A–}/{HA})
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Multi part question
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What is the pH of a buffer solution that is composed of a weak acid, HA (Ka=2.45×10–8), and the conjugate base, A–, after 2.71 mL of 0.135 M HCl solution is added. The initial concentrations of the 142 mL buffer solution are [HA]=0.7 M and [A–]=0.37 M. Enter your value to two (2) decimal places.
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