Since the solution is a buffer, we can use the Henderson-Hasselbalch Equation to calculate the ratio of [NO2-]/[HNO2] to have a pH of 3.71:
In the solution, identify the weak acid and the conjugate base. Recall from the Bronsted-Lowry definition that an acid is a proton (H+) donor and the base is a proton (H+) acceptor.
The Ka of nitrous acid, HNO2, is 4.5x10-4. What [NO2-]/[HNO2] ratio is necessary to make a buffer with a pH of 3.71?
a) 1.9 x 10-8
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