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Sagot :
Answer:
To find the pH of a buffer solution containing acetic acid (CH₃COOH) and sodium acetate (CH₃COON equation:
\[
\text{pH} = \text{pKa} + \log\left(\frac{[\text{A}^-]}{[\text{HA}]}\right)
\]
where:
- \([\text{A}^-]\) is the concentration of the base (sodium acetate),
- \([\text{HA}]\) is the concentration of the weak acid (acetic acid),
acid dissociation constant, and
- pKa is{Ka})\).
### Step 1: Calculate the pKa
Given:
\[
K_a = 1.77 \times 10^{-5}
\]
Now calculate pKa:
\[
\text{pKa} = -\log(1.77 \times 10^{-5}) \approx 4.753
\]
### Step 2: Plug in the values into the Henderson-Hassel{A}^-] = 0.800 \, \text{M}\) (sodium acetate)
- \([\text{HA}] = 1.00 \, \text{M}\) (acetic acid)
Now, substitute these values into the equation:
\[
\text{pH} = 4.753 + \log\left(\frac{0.800}{1.00}\right)
\]
### Step 3: Calculate the log term
\[
\log\left(\frac{0.800}{1.00}\right) = \log(0.800) \approx -0.097
\]
### Step 4: Calculate the pH
Now substitute back into the equation:
\[
\text{pH} = 4.753 - 0.097 \approx 4.656
\]
### Conclusion
The pH of the buffer solution is approximately **4.656**.
I hope you understand because that's how I solve it
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