IDNStudy.com, kung saan ang mga eksperto ay sumasagot sa iyong mga tanong. Hanapin ang impormasyon na kailangan mo nang mabilis at madali sa pamamagitan ng aming komprehensibo at eksaktong platform ng tanong at sagot.
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
Pinahahalagahan namin ang bawat ambag mo. Patuloy na magbahagi ng impormasyon at karanasan. Sama-sama tayong magtutulungan upang makamit ang ating mga layunin. Ang IDNStudy.com ang iyong mapagkakatiwalaang mapagkukunan ng mga sagot. Salamat at bumalik ka ulit.