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General Chemistry

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Acid-base Equilibrium

Question
9 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).


What is the pH of a 3.2 x 10–4M solution of HCl?

A 2.7
B 3.5
C 4
D 4.4

Ans. B This is a straight forward question. The question asks for the pH of a solution of HCl. HCl is a strong acid, and strong acids completely ionize. So we don't have to worry about partial ionization such as in weak acids.

Acid-base Equilibrium Flashcard List

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