Consider a solution consisting of the following two buffer ...

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Question 1

Calculate the pH of a solution that is 2.00 M HF, 1.00 M NaOH, and 0.699 M NaF. (K_a = 7.2 10^–4)

◦ 3.14
◦ 3.37
◦ 2.69
◦ 2.91
◦ None of these are correct.

Question 2

Consider a solution consisting of the following two buffer systems:
              H₂CO₃HCO₃^– + H⁺     pK_a = 6.4
              H₂PO₄^–HPO₄^2– + H⁺     pK_a = 7.2
At pH 6.4, which one of the following is true of the relative amounts of acid and conjugate base present?

◦ [H₂CO₃] > [HCO₃^–] and [H₂PO₄^–] > [HPO₄^2–]
◦ [H₂CO₃] = [HCO₃^–] and [H₂PO₄^–] > [HPO₄^2–]
◦ [H₂CO₃] = [HCO₃^–] and [HPO₄^2–] > [H₂PO₄^–]
◦ [HCO₃^–] > [H₂CO₃] and [HPO₄^2–] > [H₂PO₄^–]
◦ [H₂CO₃] > [HCO₃^–] and [HPO₄^2–] > [H₂PO₄^–]

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[awywial]

Thanks for the timely response, appreciate it

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