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A 1.00 L buffer solution at 25 °C contains 0.250 M formic acid (HCOOH) and 0.25…

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Wize University Chemistry Textbook > Buffers and Titrations

Buffers Problem Type 3

3 Activities

A 1.00 L buffer solution at 25 °C contains 0.250 M formic acid (HCOOH) and 0.250 M sodium formate (NaHCOO). Calculate the pH of the solution after the addition of 100.0 mL of 1.00 M NaOH. The Ka of HCOOH is 1.8 x 10-4.
More Buffers Problem Type 3 Questions:
Henderson Hasselbalch: Buffer Solutions
A buffer is formed by dissolving 5g of sodium benzoate, C6H5COONa, and 6g of benzoic acid, C6H5COOH (Ka =6.5 x 10-5) in 1 L of water.
What is the pH of this buffer?
The buffer is split into two beakers, 500 mL each. To the first beaker is added 1mL of 1.0 M HCl and to the second is added 1 mL of 1.0M NaOH. Calculate the pH of each beaker.
Consider a buffer solution prepared from HOCl and NaOCl. Which is the net ionic equation for the reaction that occurs when NaOH is added to this buffer?