1) Calculate how many moles of KOOCH would be needed to create 1.00 L of a pH = 9.069 solution. Assume the volume does not change as the solution is formed.

2) A 0.029 mol sample of a weak acid, HA, is dissolved in 541 mL of water and titrated with 0.41 M NaOH. After 31 mL of the NaOH solution has been added, the overall pH = 4.953. Calculate the K_a value for HA.

3) Consider a the titration of 0.795 L of 0.677 M carbonic acid (H₂CO₃) with 1.57 M NaOH. What is the pH at the second equivalence point of the titration?

Question

1) Calculate how many moles of KOOCH would be needed to create 1.00 L of a pH = 9.069 solution. Assume the volume does not change as the solution is formed.

2) A 0.029 mol sample of a weak acid, HA, is dissolved in 541 mL of water and titrated with 0.41 M NaOH. After 31 mL of the NaOH solution has been added, the overall pH = 4.953. Calculate the K_a value for HA.

3) Consider a the titration of 0.795 L of 0.677 M carbonic acid (H₂CO₃) with 1.57 M NaOH. What is the pH at the second equivalence point of the titration?

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