Why Is the ICE Table Set Up This Way for CH3COOH and NaCH3COO Solution?

In summary, the question is asking for the pH of a solution containing 0.100 M CH3COOH and 0.100 M NaCH3COO with a Ka value of 1.8x10-5. It is not necessary to use an ICE table to solve this problem, as the concentrations of both the acid and its conjugate base can be assumed to be equal. The presence of Na+ does not affect the stoichiometry, hence the molarities of NaCH3COO and CH3COO- are equal. The Henderson-Hasselbalch equation can also be used to solve this problem.
  • #1
Raul3140
4
0

Homework Statement



What will be the pH of a solution that contains 0.100 M CH3COOH and 0.100 M NaCH3COO?Ka = 1.8x10-5
IMPORTANT: THE REACTION IS NOT BETWEEN CH3COOH AND CH3COO-

- My question here is why the ice table was setup as so by the instructor? see below...



Homework Equations





The Attempt at a Solution



CH3COOH + H20 ---> CH3COO- + H3O
.100M-x .100m+x +x

Where did the Na go? Why did the Molarity of NaCH3COO = Molarity of CH3COO- ?
 
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  • #2
Raul3140 said:
My question here is why the ice table was setup as so by the instructor? see below...

No idea. No need for an ICE table. You can safely assume concentrations of both acid and conjugate base are these introduced into solution.

Where did the Na go?

Doesn't matter, Na+ is just a spectator.

Why did the Molarity of NaCH3COO = Molarity of CH3COO- ?

Dissociation stoichiometry, plus the assumption explained above.

Compare Henderson-Hasselbalch equation.
 

Related to Why Is the ICE Table Set Up This Way for CH3COOH and NaCH3COO Solution?

1. What is a buffer solution?

A buffer solution is a solution that resists changes in pH when small amounts of acid or base are added. It is made up of a weak acid or base and its conjugate salt.

2. What is the common ion effect in buffer solutions?

The common ion effect in buffer solutions is the phenomenon where the addition of a common ion, such as the conjugate salt of the weak acid or base, decreases the ionization of the weak acid or base. This results in a decrease in the pH of the buffer solution.

3. Why is the common ion effect important in buffer solutions?

The common ion effect is important in buffer solutions because it helps maintain the stability of the solution's pH. Without the common ion effect, the pH of a buffer solution would change significantly when small amounts of acid or base are added, making it less effective as a buffer.

4. How does adding a common ion affect the buffer capacity?

Adding a common ion decreases the buffer capacity of a solution. This is because the common ion competes with the weak acid or base for the addition of hydrogen or hydroxide ions, reducing the ability of the buffer to resist changes in pH.

5. Is the common ion effect the only factor that affects buffer capacity?

No, the common ion effect is not the only factor that affects buffer capacity. Other factors include the concentrations of the weak acid or base and its conjugate salt, as well as the overall volume of the solution.

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