What is the ph of a buffer that consists of 0.45 m ch3cooh and 0.35 m ch3coona?
1 answer:
Hello!
The pH of a buffer that consists of 0,45 M CH₃COOH and 0,35 M CH₃COONa can be calculated using the Henderson-Hasselbach equation. To input the values into this equation, we'll need the pKa of CH₃COOH, which can be found in tables. This value is 4,75. The Henderson-Hasselbach equation is as follows:
![pH=pKa + log( \frac{[A^{-} ]}{[HA]} ) \\ pH=4,75 + log( \frac{0,35 M}{0,45M} ) \\ pH=4,64](https://tex.z-dn.net/?f=pH%3DpKa%20%2B%20log%28%20%5Cfrac%7B%5BA%5E%7B-%7D%20%5D%7D%7B%5BHA%5D%7D%20%29%20%5C%5C%20pH%3D4%2C75%20%2B%20log%28%20%5Cfrac%7B0%2C35%20M%7D%7B0%2C45M%7D%20%29%20%5C%5C%20pH%3D4%2C64)
So, the pH of such buffer would be 4,64.
Have a nice day!
The pH of a buffer that consists of 0,45 M CH₃COOH and 0,35 M CH₃COONa can be calculated using the Henderson-Hasselbach equation. To input the values into this equation, we'll need the pKa of CH₃COOH, which can be found in tables. This value is 4,75. The Henderson-Hasselbach equation is as follows:
So, the pH of such buffer would be 4,64.
Have a nice day!
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Answer:
Coefficient of is more than 4
Explanation:
Oxidation:
- Balance charge:
......(1)
Reduction:
- Balance Cr:
- Balance O and H in acidic medium:
- Balance charge:
.......(2)
gives balanced equation:
So coefficient of is more than 4