3.9
Titration of Polyprotic Base with a Strong Acid
The titration of a polyprotic base such as sodium carbonate with a strong acid such as hydrochloric acid results in two equivalence points on the titr…
A polyprotic bronsted base like sodium carbonate reacts with water in two successive steps.
In its titration with hydrochloric acid, the initial pH estimated from the first dissociation constant of sodium carbonate is 11.6. The solution slowly turns acidic, demonstrating two equivalence points on the titration curve.
At the first equivalence point, all the carbonate ions are converted to bicarbonate ions. The second equivalence point corresponds to the complete conversion of bicarbonate ions to carbonic acid, which in an acidic solution dissociates to carbon dioxide and water.
While the region before the first equivalence point contains the carbonate/bicarbonate buffer, the area between the first and second equivalence points holds the bicarbonate/carbonic acid buffer.
The indicators for detecting the first and second endpoints are phenolphthalein and methyl orange, respectively.
Here, the methyl orange exhibits a gradual color change resulting in poor endpoint detection. So, a mixture of methyl orange and xylene cyanol is used, which sharpens the second endpoint observation.
Q1: Why does a polyprotic base like sodium carbonate produce two equivalence points during titration with strong acid?
Sodium carbonate is a polyprotic base that reacts with hydrochloric acid in two successive steps. At the first equivalence point, all carbonate ions convert to bicarbonate ions. At the second equivalence point, bicarbonate ions completely convert to carbonic acid, which dissociates into carbon dioxide and water in acidic solution. This two-step conversion creates two distinct equivalence points on the titration curve.
Q2: What is the initial pH of a sodium carbonate solution before titration begins?
The initial pH of a sodium carbonate solution is approximately 11.6, estimated from the first dissociation constant of sodium carbonate. This basic pH reflects the solution's initial composition as a polyprotic base before any strong acid is added during the titration process.
Q3: What buffer systems form during the titration of sodium carbonate with hydrochloric acid?
Two buffer systems form during titration. Before the first equivalence point, the carbonate/bicarbonate buffer exists. Between the first and second equivalence points, the bicarbonate/carbonic acid buffer is present. These buffers resist pH changes as the strong acid is gradually added to the polyprotic base solution.
Q4: Which indicators are used to detect the endpoints in polyprotic base titration?
Phenolphthalein detects the first endpoint when carbonate ions convert to bicarbonate ions. For the second endpoint, a mixture of methyl orange and xylene cyanol is used instead of methyl orange alone. This mixture sharpens the second endpoint observation because methyl orange exhibits a gradual color change that results in poor endpoint detection when used alone.
Q5: How does the titration curve change as sodium carbonate reacts with hydrochloric acid?
The solution slowly turns acidic as hydrochloric acid is added to sodium carbonate, producing a titration curve with two distinct equivalence points. The curve reflects the sequential conversion of carbonate to bicarbonate at the first equivalence point, then bicarbonate to carbonic acid at the second equivalence point, demonstrating the polyprotic nature of the base.
Q6: What happens to carbonic acid after the second equivalence point is reached?
After the second equivalence point, all bicarbonate ions have been converted to carbonic acid. In the acidic solution created by excess hydrochloric acid, carbonic acid dissociates into carbon dioxide gas and water. This dissociation removes carbonic acid from the solution as the titration continues beyond the second equivalence point.
Q7: Why is a mixture of methyl orange and xylene cyanol used instead of methyl orange alone?
Methyl orange exhibits a gradual color change that results in poor endpoint detection when used alone for the second equivalence point. Adding xylene cyanol to methyl orange sharpens the second endpoint observation, providing a clearer visual indicator for the analyst to accurately identify when the titration is complete.