Problem: Consider the following titration curves for two weak acids (see the figures), both titrated with 0.100 M NaOH. , Which of the two acids has the larger Ka?

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Weak acid and strong base titration

  • pH gradually increases as it approaches the equivalence point
  • pH at the equivalence point is more than 7.00


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Problem Details

Consider the following titration curves for two weak acids (see the figures), both titrated with 0.100 M NaOH.

 The figure labeled (a) shows pH as a function of volume of base added. The pH is measured from 0 to 14 on the y-axis, while the volume of base added is measured from 0 to 100 milliliters on the x-axis. The curve of the plot goes up gradually from pH 4.3 at 0 milliliters to pH 8.2 at 37 milliliters, next the plot goes up steeply to pH 11.8 at 39 milliliters, and finally the plot goes up gradually to pH 12.2 at 100 milliliters., The figure labeled (b) shows pH as a function of volume of base added. The pH is measured from 0 to 14 on the y-axis, while the volume of base added is measured from 0 to 100 milliliters on the x-axis. The curve of the plot goes up gradually from pH 3.0 at 0 milliliters to pH 6.2 at 29 milliliters, next the plot goes up steeply to pH 11.8 at 31 milliliters, and finally the plot goes up gradually to pH 12.2 at 100 milliliters.

Which of the two acids has the larger Ka?

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Based on our data, we think this problem is relevant for Professor Eubank's class at Florida Southern College.