Consider a solution consisting of the following two buffer systems: H₂CO₃ HCO₃^- + 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? A) [H₂CO₃] [HCO₃^-] and [H₂PO₄^-] [HPO₄^2-] B) [HCO₃^-] [H₂CO₃] and [HPO₄^2-] [H₂PO₄^-] C) [H₂CO₃] [HCO₃^-] and [HPO₄^2-] [H₂PO₄^-] D) [H₂CO₃] = [HCO₃^-] and [HPO₄^2-] [H₂PO₄^-] E) [H₂CO₃] = [HCO₃^-] and [H₂PO₄^-] [HPO₄^2-]

Question

Consider a solution consisting of the following two buffer systems: H₂CO₃ HCO₃^- + 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? A) [H₂CO₃] > [HCO₃^-] and [H₂PO₄^-] > [HPO₄^2-] B) [HCO₃^-] > [H₂CO₃] and [HPO₄^2-] > [H₂PO₄^-] C) [H₂CO₃] > [HCO₃^-] and [HPO₄^2-] > [H₂PO₄^-] D) [H₂CO₃] = [HCO₃^-] and [HPO₄^2-] > [H₂PO₄^-] E) [H₂CO₃] = [HCO₃^-] and [H₂PO₄^-] > [HPO₄^2-]

Quizplus · Accepted Answer

The Answer of Consider a solution consisting of the following two buffer systems: H₂CO₃ HCO₃^- + 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? A) [H₂CO₃] > [HCO₃^-] and [H₂PO₄^-] > [HPO₄^2-] B) [HCO₃^-] > [H₂CO₃] and [HPO₄^2-] > [H₂PO₄^-] C) [H₂CO₃] > [HCO₃^-] and [HPO₄^2-] > [H₂PO₄^-] D) [H₂CO₃] = [HCO₃^-] and [HPO₄^2-] > [H₂PO₄^-] E) [H₂CO₃] = [HCO₃^-] and [H₂PO₄^-] > [HPO₄^2-]

Consider a Solution Consisting of the Following Two Buffer Systems