Since the solution is a buffer, we can use the Henderson-Hasselbalch Equation to calculate the ratio of [ClO3-]/[HClO3] to have a pH of 10:
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 bicarbonate ion, HCO3-, is 4.8x10-11. What [ClO3-] /[HClO3] ratio is necessary to make a buffer with a pH of 10.0?
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