Acid and Base Titration Curves Video Lessons

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Concept: Understanding an Acid–Base Titration Curve.

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Concept: The Equivalence Point. 

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Example: The following questions refer to the titration curve given below. 1) The titration curve shows the titration of     a) a strong acid with a strong base    b) a weak acid with a strong base    c) a strong base with a strong acid    d) a weak base with a strong acid       2) Which point on the titration curve represents a region where a buffer solution has formed?      a) point A      b) point B      c) point C      d) point D 3) Which point on the titration curve represents the equivalence point?      a) point A      b) point B      c) point C      d) point D 4) Which of the following would be the best indicator to use in the titration?     a) erythrosin B, pKa=2.9    b) methyl blue, pKa=5.4    c) bromthymol blue, pKa= 6.8    d) o-cresonphthalein, pKa=9.0   

Problem: Consider the following curve for the titration of a weak base with a strong acid and answer each of the following questions.At what volume of added acid does pH = 14 – pKb?        

FREE Expert Solution

At 1/2 equivalence point: pH = pKa

pKa + pKb = 14

So we know that at 1/2 equivalence point:

pH = 14 – pKb

From the graph:

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Problem Details

Consider the following curve for the titration of a weak base with a strong acid and answer each of the following questions.
The figure shows pH as a function of the volume of acid added. pH is measured from 0 to 14 on the x-axis and volume is measured from 0 to 50 milliliters on the x-axis. The curve starts at pH 12 at 0 milliliters. Then it decreases slowly to pH 10 at 23 milliliters added, then falls to pH 2 at 25 milliliters added. Then the curve decreases slowly again to pH 1 at 50 milliliters.

At what volume of added acid does pH = 14 – pKb?        

Learn this topic by watchingAcid and Base Titration Curves Concept Videos
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