IDNStudy.com, ang perpektong platform para sa eksaktong at mabilis na mga sagot. Sumali sa aming platform upang makatanggap ng mabilis at eksaktong tugon mula sa mga propesyonal sa iba't ibang larangan.
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
Maraming salamat sa iyong pakikilahok. Patuloy na magbahagi ng iyong mga ideya at kasagutan. Ang iyong kaalaman ay mahalaga sa ating komunidad. IDNStudy.com ang iyong mapagkakatiwalaang kasama para sa lahat ng iyong mga katanungan. Bisitahin kami palagi.
