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If the pH of the buffer (before it is titrated) is 5.70, what is the pKa of the weak acid? Hint: Solve the Henderson-Hasselbalch equation for pKa.

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Related questions

1. A student titrated 25.0 mL of a buffer with 0.126 M HCl. Theobserved titration curve is shown below. What is the concentrationof the weak base in the buffer? Thoroughly document yourlogic.

titration curve is below:

http://i1190.photobucket.com/albums/z451/chemistrypictures/chart1.jpg

2. The student then titrated 25.0 mL of the same buffer with 0.1115M NaOH. The observed titration curve is shown below. What is theconcentration of the weak acid in the buffer?

Titration curve link:

http://i1190.photobucket.com/albums/z451/chemistrypictures/chart2.jpg

3. What is the buffer strength (i. e., the total of [HA] and[A-])?

4. If the pH of the buffer (before it is titrated) is 5.70, what isthe pKa of the weak acid? (Hint: solve the henderson-hasselbalchequation for pKa)

Find the new pH using Henderson -Hasselbalch equation
Add 30 ml of .1M HCl to one liter of .1M sodium acetate buffer, pH 6.46. pKa = 4.76 for acetic acid. What is the pH?

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