18. Aqueous Equilibrium
Titrations: Diprotic & Polyprotic Buffers
10PRACTICE PROBLEM
In a laboratory experiment, you need to prepare a solution buffered at pH = 6.00. The organism that you are working with is not sensitive to the weak acid malonic acid (H2C3H2O4: Ka1 = 1.5×10–3; Ka2 = 2.0×10–6) and its sodium salts. Solutions of 1.5 M malonic acid and 1.5 M NaOH are available in the laboratory. Calculate the volume of NaOH solution that should be added to the 1.5 L of malonic acid in order to create a buffer solution buffered at pH = 6.00. Assume that volume does not change.
In a laboratory experiment, you need to prepare a solution buffered at pH = 6.00. The organism that you are working with is not sensitive to the weak acid malonic acid (H2C3H2O4: Ka1 = 1.5×10–3; Ka2 = 2.0×10–6) and its sodium salts. Solutions of 1.5 M malonic acid and 1.5 M NaOH are available in the laboratory. Calculate the volume of NaOH solution that should be added to the 1.5 L of malonic acid in order to create a buffer solution buffered at pH = 6.00. Assume that volume does not change.