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General Chemistry

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Acid-base Equilibrium

Question
7 out of 10
 

Strong acids and bases ionize completely in aqueous solutions. Weak acids and bases ionize only partially in aqueous solutions. An acid-base reaction is shown below. A titration was done by adding a base to a known concentration and fixed volume of an acid. The reaction follows:

The dissociation of a weak acid can be represented as:

Chemists often use Henderson-Hasselbach equation to calculate the pH of solutions containing a weak acid of known pKa, provided that the other concentrations are known. Henderson-Hasselbach equation is:

This equation is also used to calculate the buffering capability of solutions. It is roughly estimated that a given buffer is most likely to be effective at pH levels between (pKa + 1) and (pKa – 1).


The titration curve of the acid-base reaction (Reaction 1) is best represented by:

A
B
C
D
Ans. A For this question, we are looking for a strong acid-strong base curve. Why? Well, the answer is simple. In Reaction 1, we have a strong monoprotic acid (HClO4) reacting against a strong base (NaOH). The only curve that satisfies this criterion is given in Choice A.

Acid-base Equilibrium Flashcard List

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