Complete Video of the Reactions

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Summary

A strong acid, a weak acid, and a buffer solution are each added to sodium bicarbonate and the reaction rates are compared. The 7 thumbnail images summarize the content of the video. Click an image to see the image gallery.

Narration

Hydrochloric acid, a strong acid, added to the first test tube reacts almost instantaneously with the sodium bicarbonate. In the middle test tube, the reaction of sodium bicarbonate with acetic acid, a weak acid, is slower. A buffer solution made from acetic acid and the base sodium acetate is the liquid in the third test tube. This buffer solution is reacting with the sodium bicarbonate much more slowly than the acids in the other two test tubes.

The reaction rate of a strong acid is the greatest, the reactivity of a weak acid is less, and the reactivity of the buffer solution is significantly less. The rates of reaction depend on the relative concentrations of hydrogen ions in the solution that reacts with the sodium bicarbonate. The concentration of hydrogen ions is greatest in the strong acid, smaller in the weak acid, and smallest in the buffer solution.

Discussion

There are several factors that can affect reaction rate. One of these is the concentration(s) of the species participating in the reaction. In most cases, the more concentrated the solution, the greater the reaction rate.

A strong acid solution will have a higher concentration of hydronium ions than an equimolar solution of a weak acid. Adding the conjugate base to a weak acid in order to form a buffer solution reduces the hydronium ion concentration even further.

Keywords

Acids / Bases | Kinetics

These ChemEd DL Resource Groups Include This Video

Relative Reactivity: Strong Acid, Weak Acid, Buffer Solution
Rates of Reactions
Reactions in Aqueous Solutions
Acid Base Reactions


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