You might develop a talbe like this one: 0.10 M acetic acid, pH= 3.51, [H+] = ?,

Question

You might develop a talbe like this one:

0.10 M acetic acid, pH= 3.51, [H+] = ?, [C2H3O2-]=?, [HC2H3O2]=?

0.010 M acetic acid, pH= 4.30, [H+] = ?, [C2H3O2-]=?, [HC2H3O2]=?

0.0010 M acetic acid, pH= 5.75, [H+] = ?, [C2H3O2-]=?, [HC2H3O2]=?

0.0001 M acetic acid, pH= 6.28, [H+] = ?, [C2H3O2-]=?, [HC2H3O2]=?

1. Is the ionization of acetic acid a relatively complete reaction, or is it a partial one that represents an equilibrium?

2. What general pattern do you observe in the concentration of acetic acid versus pH?

3. Compare the relationship among the three values ([H+ ], [C 2H 3O - ], [H C 2H 3O 2]) for each initialconcentration of acetic acid. Try different mathematical operations to see if you can find a (numerical) pattern to explain your observations (multiply, divide, etc.). You can try multiplying all three or a combination of multiplying and dividing (i.e., dividing one by the product of the other two, etc.).

Explanation / Answer

1. The ionization of acetic acid (a weak acid) is partially complete. When the concentration of acetic acid, acetate and hydronium ion do not change with time, that state is said to be an equilibrium.

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