You have solutions of 0.200 M HNO₂ and 0.200 M KNO₂ (K_a for HNO₂ = 4.00 × 10^-4). A buffer of pH 3.000 is needed. What volumes of HNO₂ and KNO₂ are required to make 1 L of buffered solution? A) 286 mL HNO₂; 714 mL KNO₂ B) 714 mL HNO₂; 286 mL KNO₂ C) 413 mL HNO₂; 587 mL KNO₂ D) 500 mL of each E) 587 mL HNO₂; 413 mL KNO₂

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Using the Henderson-Hasselbalch equation, the ratio of [NO2-]/[HNO2] is calculated to be approximately 0.4. This corresponds to 714 mL of HNO2 and 286 mL of KNO2 to achieve the desired pH of 3.000.

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